Write a balanced equation for the reaction which occurs with the CaCI2 solution and the soap (a fatty acid salt). **Use “(fatty acid-CO2)-Na+” as the structure for the soap instead of drawing out the entire fatty acid structure

The rate law equation for this reaction is:

rate = (1.99 x 10^68 L^12/mol^12 s)[F]^21[H]^-9

To find the rate law equation for this reaction, we'll use the given experimental data to determine the order of the reaction with respect to F and H. The rate law equation will be in the form:

rate = k[F]^x[H]^y

We can use the data from the first two experiments to determine the order of the reaction with respect to F:

Exp1: rate1 = k(0.000345)^x(0.000765)^y

Exp2: rate2 = k(0.000690)^x(0.000765)^y

Divide rate2 by rate1:

(rate2/rate1) = (0.000690/0.000345)^x

(3.24 x 10^8)/(3.24 x 10^2) = (2)^x

2.0 x 10^6 = 2^x

Since 2^21 = 2097152, which is approximately 2.0 x 10^6, we can conclude that x = 21. So, the reaction is 21st order with respect to F.

Now, we can use the data from experiments 1 and 3 to determine the order of the reaction with respect to H:

Exp1: rate1 = k(0.000345)^21(0.000765)^y

Exp3: rate3 = k(0.000345)^21(0.00765)^y

Divide rate3 by rate1:

(rate3/rate1) = (0.00765/0.000765)^y

(3.24 x 10^-7)/(3.24 x 10^2) = (10)^y

1.0 x 10^-9 = 10^y

From this, we can conclude that y = -9. So, the reaction is -9th order with respect to H.

Now, we can write the rate law equation:

rate = k[F]^21[H]^-9

Next, we'll calculate the rate constant k using the data from any of the experiments. Let's use the data from Experiment 1:

rate1 = 3.24 x 10^2 M/sec

[F]1 = 0.000345 mol/L

[H]1 = 0.000765 mol/L

3.24 x 10^2 = k(0.000345)^21(0.000765)^-9

After calculating, we find:

k ≈ 1.99 x 10^68 L^12/mol^12 s

So, the rate law equation for this reaction is:

rate = (1.99 x 10^68 L^12/mol^12 s)[F]^21[H]^-9

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[tex]V_{tot} = \frac{587 g}{1,07 g/mL} = 549 mL[/tex]

0,022 kg = 22 g

[tex]\frac{m}{V} = \frac{22 g × 100}{549 mL} = 4,0 % [/tex]

The mass of calcium in the original urine sample would be 0.0140 g.

First, we need to find the masses of calcium and magnesium oxalates in the original sample. Let x be the mass of calcium oxalate and y be the mass of magnesium oxalate. Then we have:

x + y = mass of the mixed oxalate precipitate

Next, we need to use the information given to find the mass of calcium in the original sample. The mass of calcium oxide formed after ignition is equal to the mass of calcium oxalate in the original sample. We can calculate the mass of calcium oxide using the mass of calcium carbonate formed and the molar mass ratio of calcium carbonate to calcium oxide.

The balanced chemical equations for the reactions are:

CaC2O4 -> CaCO3 + CO2

CaCO3 -> CaO + CO2

The molar mass of CaCO3 is 100.09 g/mol, and the molar mass of CaO is 56.08 g/mol.

From the given information, we have:

0.0433 g = (x + y)(100.09 g/mol + 80.15 g/mol) / (128.10 g/mol + 80.15 g/mol)

0.0285 g = x(56.08 g/mol) + y(40.31 g/mol)

Solving these equations simultaneously, we get:

x = 0.0140 g

y = 0.0053 g

Therefore, the mass of calcium in the original sample (which is equal to the mass of calcium oxide formed after ignition) is:

0.0140 g

So the mass of calcium in the original sample is 0.0140 g.

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The compound's boiling point is around 73.65 °C.

Unexpected Responses. Favorable reactions are those that cause the system's enthalpy to drop while its entropy rises. The reaction happens naturally when both of these conditions are true. Both endothermic and exothermic reactions, which absorb heat and release it, can occur spontaneously.

We can use the Gibbs-Helmholtz equation to solve for the boiling point:

ΔG = ΔH - TΔS

At boiling point, ΔG = 0, so we can solve for T:

T = ΔH/ΔS

Substituting the given values:

T = (32.77 kJ·mol−1) / (94.72 J·mol−1·K−1)

T = 346.8 K

Converting to Celsius:

Boiling point = 346.8 K - 273.15 = 73.65 °C

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The reaction's G value at 805 K is -2625.7 kJ.

Sulfur dioxide gas is the byproduct of the interaction between sulphur and oxygen. Sulphurous acid is created when sulphur dioxide dissolves in water. Sulfuric acid causes blue litmus paper to turn red. Non-metal oxides typically have an acidic character.

ΔG = ΔH - TΔS

where ΔH is the enthalpy change, ΔS is the entropy change, T is the temperature in Kelvin, and ΔG is the change in Gibbs free energy.

Substituting the given values:

ΔG = -2374 kJ - (805 K)(312.2 J/K)

ΔG = -2374 kJ - 251717 J

ΔG = -2374 kJ - 251.7 kJ

ΔG = -2625.7 kJ

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The sheriff was poisoned by the use of the arsenic poison.

Arsenic is a toxic substance that can be deadly if ingested or inhaled in high concentrations. It works by disrupting important cellular processes and functions within the body.

When arsenic is ingested, it is absorbed through the digestive system and enters the bloodstream. From there, it is transported to various organs and tissues throughout the body, including the liver, kidneys, and lungs.

Arsenic interferes with the enzymes and proteins that are essential for cellular metabolism, DNA synthesis, and other important cellular processes. This disruption can cause a range of symptoms, including abdominal pain, diarrhea, vomiting, and dehydration.

Arsenic can also cause damage to the nervous system, leading to neurological symptoms such as confusion, seizures, and numbness or tingling in the extremities.

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54.2 g of CaCl2 must be dissolved in 1000 g of water to raise the boiling point to 100.75°C.

To solve this problem, we can use the formula:

ΔTb = Kb × m × i

where ΔTb is the boiling point elevation, Kb is the molal boiling point elevation constant for water, m is the molality of the solution, and i is the van't Hoff factor, which represents the number of particles into which the solute dissociates.

We can rearrange this formula to solve for the molality of the solution:

m = ΔTb / (Kb × i)

We know that ΔTb is 0.75°C (100.75°C - 100°C), Kb is 0.51°C/m, and i for CaCl2 is 3 (since it dissociates into 3 ions in water). Substituting these values, we get:

m = 0.75°C / (0.51°C/m × 3) = 0.490 m

To find the mass of CaCl2 needed to make a 0.490 m solution in 1000 g of water, we can use the formula:

moles of solute = molality × mass of solvent (in kg)

We convert 1000 g of water to 1 kg, and then use the molecular weight of CaCl2 to convert from moles to grams:

moles of CaCl2 = 0.490 m × 1 kg = 0.490 mol

mass of CaCl2 = 0.490 mol × 110.98 g/mol = 54.2 g

Therefore, 54.2 g of CaCl2 must be dissolved in 1000 g of water to raise the boiling point to 100.75°C.

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Answer: the wavelength of the photon is approximately 3.58 × 10^-18 meters.

Explanation: where E is the energy of the photon, h is Planck's constant, f is the frequency of the photon, c is the speed of light, and λ is the wavelength of the photon.

We can rearrange this equation to solve for the wavelength:

λ = hc/E

where all variables have their previously defined meanings.

First, we need to convert the energy from joules to electronvolts (eV), which is a more commonly used unit for photon energy:

8.87 × 10^-28 J = 8.87 × 10^-28 J / 1.602 × 10^-19 J/eV = 5.53 × 10^-10 eV

Next, we can substitute the given values into the equation:

λ = (6.626 × 10^-34 J s) × (2.998 × 10^8 m/s) / (5.53 × 10^-10 eV)

Simplifying, we get:

λ = 3.580 × 10^-18 m

Finally, we can express the wavelength in scientific notation with three significant figures:

λ = 3.58 × 10^-18 m

a)  The conjugate base of aspirin (acetylsalicylic acid) is formed when the acidic proton (H+) is removed from the carboxylic acid group (-COOH) in the molecule.

b)  More aspirin will be available for absorption in the duodenum (97%) compared to the stomach (12%).

a. The conjugate base of aspirin (acetylsalicylic acid) is formed when the acidic proton (H+) is removed from the carboxylic acid group (-COOH) in the molecule.

b. The percentage of aspirin available for absorption depends on the degree of ionization of the molecule, which is related to the pH of the surrounding medium. At pH values below the pKa (2.97), most of the molecules exist in the protonated form (HA), while at pH values above the pKa, most of the molecules exist in the deprotonated form (A-).

Using the Henderson-Hasselbalch equation:

pH = pKa + log([A-]/[HA])

We can calculate the ratio of deprotonated (A-) to protonated (HA) forms at different pH values. At pH 2.0, the ratio is:

2.0 = 2.97 + log([A-]/[HA])

log([A-]/[HA]) = -0.97

[A-]/[HA] = 0.12

So, at pH 2.0, only 12% of the aspirin molecules are in the deprotonated form and available for absorption.

At pH 4.5, the ratio is:

4.5 = 2.97 + log([A-]/[HA])

log([A-]/[HA]) = 1.53

[A-]/[HA] = 31.6

So, at pH 4.5, 97% of the aspirin molecules are in the deprotonated form and available for absorption.

Therefore, more aspirin will be available for absorption in the duodenum (97%) compared to the stomach (12%).

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The density of sulfur dioxide gas at a temperature of 15°C and pressure of 300 torr is 0.001022 g/cm³, or 0.001022 g/mL, or 1.022 kg/m³, or 0.01022 g/L when converted to atm.

What is density?

To calculate the density of sulfur dioxide gas at a temperature of 15°C and a pressure of 300 torr, we can use the ideal gas law:

PV = nRT

where P is the pressure in atmospheres, V is the volume in liters, n is the number of moles, R is the ideal gas constant (0.08206 L·atm/(mol·K)), and T is the temperature in Kelvin.

First, we need to convert the given temperature of 15°C to Kelvin:

T = 15°C + 273.15 = 288.15 K

Next, we can rearrange the ideal gas law to solve for the number of moles:

n = PV/RT

where we can use the given pressure of 300 torr and convert it to atm by dividing by 760 torr/atm:

P = 300 torr / 760 torr/atm = 0.3947 atm

Substituting the values into the equation, we get:

n = (0.3947 atm) V / (0.08206 L·atm/(mol·K) × 288.15 K)

Now, we can use the molar mass of sulfur dioxide, which is 64.06 g/mol, to convert the number of moles to mass:

mass = n × molar mass

Finally, we can calculate the density of sulfur dioxide gas using the mass and volume:

density = mass / V

To convert the density from g/L to g/cm³, we divide by 1000.

Putting it all together, we get:

n = (0.3947 atm) V / (0.08206 L·atm/(mol·K) × 288.15 K)

n = 0.01595 V

mass = n × molar mass = 0.01595 V * 64.06 g/mol = 1.022 gV

density = mass / V = 1.022 gV / V = 1.022 g/L = 0.001022 g/cm³

Therefore, the density of sulfur dioxide gas at a temperature of 15°C and pressure of 300 torr is 0.001022 g/cm³, or 0.001022 g/mL, or 1.022 kg/m³, or 0.01022 g/L when converted to atm.

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Complete question is: The density of Sulfur dioxide gas at a temperature of 15oC and pressure of 300 torr is 0.01022 atm.

It's important to note that equilibrium is a dynamic state, meaning that while the conditions mentioned above are true, there may still be continuous microscopic fluctuations or changes within the system, but the macroscopic properties remain constant.

What is Equilibrium?

Equilibrium refers to a state of balance or stability in a system where there is no net change or overall tendency for change to occur. In various scientific disciplines, including physics, chemistry, and biology, equilibrium is a fundamental concept that describes the balance between opposing forces or processes.

Balance of forces: The net force acting on the system is zero. This means that the forces acting in opposite directions are balanced, and there is no overall acceleration of the system.

Balance of torques: The net torque (or moment) acting on the system is zero. This means that the torques acting in opposite directions are balanced, and there is no rotational acceleration of the system.

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Light takes 20,100 seconds or 5.583 hours to travel 6.03 billion km.

To calculate the time it takes for light to travel 6.03 billion km, we can use the formula:

time = distance / speed of light

where distance is 6.03 x 10^9 km and the speed of light is approximately 299,792,458 meters per second (m/s).

First, we need to convert the distance from kilometers to meters:

distance = 6.03 x 10^9 km x 10^3 m/km = 6.03 x 10^12 m

Now we can calculate the time:

time = distance / speed of light

= 6.03 x 10^12 m / 299,792,458 m/s

= 20,107.394 seconds

To 3 significant figures, the answer is 20,100 seconds or 5.583 hours (since there are 3600 seconds in an hour).

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The molar mass of hydrogen is approximately 1 g/mol. This means that 1 mole of hydrogen atoms has a mass of 1 gram. So, to find the number of atoms in 20 grams of hydrogen, we need to first find how many moles of hydrogen there are, using the following equation:

moles of hydrogen = mass of hydrogen / molar mass of hydrogen

Plugging in the values, we get:

moles of hydrogen = 20 g / 1 g/mol = 20 mol

So there are 20 moles of hydrogen present in 20 g of hydrogen.

Finally, we can find the number of atoms of hydrogen using Avogadro's number, which gives the number of particles (such as atoms, molecules, or ions) in one mole of a substance. Avogadro's number is approximately 6.02 x 10^23 particles per mole. So we can find the number of atoms of hydrogen as follows:

number of atoms of hydrogen = moles of hydrogen x Avogadro's number

Plugging in the values, we get:

number of atoms of hydrogen = 20 mol x 6.02 x 10^23 atoms/mol

number of atoms of hydrogen = 1.204 x 10^25 atoms

Therefore, there are approximately 1.204 x 10^25 atoms of hydrogen in 20 g of H2.

Answer:The heat required to convert a given mass of a substance from one phase to another can be calculated using the following formula:

q = m × ΔH

where:

q = heat (in joules or kilojoules)

m = mass of the substance (in grams or kilograms)

ΔH = enthalpy change (in J/g or kJ/mol) associated with the phase transition

In this case, we need to calculate the heat required to convert 2.90 g of water at 67.0 °C to steam at 100.0 °C. The specific heat capacity of water is 4.184 J/g • °C, and the enthalpy of vaporization (ΔHvap) of water is 40.7 kJ/mol.

First, we need to calculate the heat required to raise the temperature of the water from 67.0 °C to its boiling point of 100.0 °C:

q1 = m × c × ΔT1

q1 = 2.90 g × 4.184 J/g • °C × (100.0 °C - 67.0 °C)

q1 = 2.90 g × 4.184 J/g • °C × 33.0 °C

q1 = 4591.632 J

Next, we need to calculate the heat required to vaporize the water at its boiling point:

q2 = n × ΔHvap

q2 = (m/M) × ΔHvap

q2 = (2.90 g / 18.015 g/mol) × 40.7 kJ/mol

q2 = 0.1619 kJ

Finally, we can add the two heat values to obtain the total heat required:

q = q1 + q2

q = 4591.632 J + 0.1619 kJ

q = 4.7521 kJ

So, the amount of heat required to convert 2.90 g of water at 67.0 °C to 2.90 g of steam at 100.0 °C is approximately 4.7521 kJ.

Explanation:

Answer: 40. g

Explanation:

To find the grams in 0.89 moles of CO2, we just need to use the molar mass of CO2. The molar mass which tells us how many grams are in a mole for an element or compound.

The molar mass of CO2 is equal to the molar mass of carbon, 12.0107, and 2 oxygens, 2*15.9994 (you can find the molar mass of an element on any periodic table). Add these, and you get the molar mass of CO2 to be 44.01 g/mol, a helpful value to remember.

Now, just multiply the molar mass by the amount of moles to find grams.

[tex]\frac{44.01g}{mole} * 0.89mole[/tex], moles cancel out, [tex]\frac{44.01g}{mole} * 0.89mole=40.48g[/tex]

There are 2 significant figures in the question, so I will round this answer to 2 significant figures, 40. g

The mass of sodium nitrate that must be added to saturate the solution at 50°C would be 14 grams.

The solubility of a compound typically increases with temperature, so more solute can dissolve in the solvent as the temperature increases. To calculate how much sodium nitrate needs to be added to saturate the solution at 50°C, we can use the solubility data and the fact that the amount of solute that can dissolve in a given amount of solvent is dependent on the temperature.

First, let's calculate the solubility of sodium nitrate at 50°C. According to the solubility curve for NaNO3, the solubility of NaNO3 at 35°C is 88 g/100 mL, and at 50°C it is approximately 114 g/100 mL. Therefore, we know that a saturated solution at 50°C can dissolve up to 114 g of NaNO3 per 100 mL of water.

Since the original solution contains 100 g of NaNO3 in 100 mL of water at 35°C, we know that it is already saturated at that temperature. To calculate how much more NaNO3 we need to add to saturate the solution at 50°C, we can use the following equation:

mass of NaNO3 added = (desired amount of NaNO3) - (initial amount of NaNO3)

mass of NaNO3 added = (114 g/100 mL × 100 mL) - (100 g/100 mL × 100 mL)

mass of NaNO3 added = 14 g

Therefore, we need to add 14 grams of sodium nitrate to the solution at 50°C to saturate it.

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7a. Using the mole ratio from the balanced chemical equation, we can set up the following proportion:

n(N₂)/n(NH₃) = 1/2

where n(N₂) is the number of moles of N₂ and n(NH₃) is the number of moles of NH₃. Solving for n(N₂), we get:

n(N₂) = (10.0 mol NH₃) / (2 mol N₂/mol NH₃) = 5.00 mol N2

Therefore, 5.00 moles of nitrogen would be needed to make 10.0 moles of ammonia.

7b. Using the same mole ratio as above, we can set up the following proportion:

n(NH₃)/n(H₂) = 2/3

where n(H₂) is the number of moles of H₂. Solving for n(NH₃), we get:

n(NH₃) = (9.00 mol H2) x (2 mol NH3/3 mol H₂) = 6.00 mol NH₃

Therefore, 6.00 moles of ammonia could be made by completely reacting 9.00 moles of hydrogen.

7c. Again, using the same mole ratio as above, we can set up the following proportion:

n(N₂)/n(H₂) = 1/3

where n(N₂) is the number of moles of N₂. Solving for n(H₂), we get:

n(H₂) = (7.41 mol N2) x (3 mol H₂/1 mol N₂) = 22.2 mol H₂

Therefore, 22.2 moles of hydrogen would be needed to react completely with 7.41 moles of nitrogen.

8a. The amounts of reactants consumed and the amount of product made can be calculated using stoichiometry, which is based on the mole ratio from the balanced chemical equation. However, the mole ratio from the balanced chemical equation cannot be interpreted as a ratio of masses, since the molar mass (and thus the mass) of each substance is different.

8b. The mole ratio from the balanced chemical equation is based on the number of moles of each substance, which is proportional to the mass of each substance. Therefore, by using the molar mass of each substance, we can convert the mole ratio to a mass ratio. However, the mole ratio itself cannot be interpreted as a ratio of masses.

9a. Yes, the mole ratio from a balanced chemical equation can be interpreted as a ratio of masses. This is because the mole ratio is determined based on the stoichiometric coefficients in the balanced equation, which represent the number of moles of each substance involved in the reaction. Since the molar mass (mass per mole) of each substance is known, the mole ratio can be used to determine a mass ratio.

9b. The mathematical concept that explains how the mole ratio from a balanced chemical equation can be interpreted as a ratio of masses is the mole-to-mole conversion factor. This conversion factor is based on the stoichiometric coefficients in the balanced equation, which represent the mole ratio between the reactants and products. By multiplying the mole ratio by the molar mass of a substance, the ratio can be converted to a mass ratio.

To solve the problem "What mass of nitrogen is needed to produce 30.0 g of ammonia?", we would need to use the concept of stoichiometry and mole-to-mole conversions. We can start by writing the balanced chemical equation for the reaction:

N₂(g) + 3H₂(g) → 2NH₃(g)

From the equation, we can see that the mole ratio of N2 to NH₃ is 1:2. We can use this ratio to determine the number of moles of N2 needed to produce 1 mole of NH₃:

1 mole N₂ : 2 moles NH₃

Next, we can use the molar mass of NH₃ to convert the moles of NH₃ to grams:

2 moles NH₃ x 17.03 g NH₃/mole = 34.06 g NH₃

So, for every 34.06 g of NH₃ produced, we need 1 mole of N₂. Using this information, we can set up a proportion to solve for the mass of N₂ needed to produce 30.0 g of NH₃:

1 mole N₂ : 34.06 g NH₃ = x moles N₂ : 30.0 g NH₃

Solving for x, we get:

x moles N₂ = (30.0 g NH₃ x 1 mole N₂) / 34.06 g NH₃ = 0.881 moles N₂

Finally, we can convert the moles of N₂ to grams using the molar mass of N₂:

0.881 moles N₂ x 28.01 g N₂/mole = 24.67 g N₂

Therefore, we would need 24.67 g of nitrogen to produce 30.0 g of ammonia.

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NH₂ can be found in various molecules, such as ammonia (NH₃) or hydrazine (N₂H₄), but is not a specific compound or molecule.

The chemical equation for the reaction of NH₂ and H₂ is:

NH₂ + 2H₂ -> 2NH₃

NH₃ is the chemical formula for ammonia, which is a compound made up of one nitrogen atom and three hydrogen atoms. It is a colorless gas with a pungent odor, and it is commonly used in the production of fertilizers, cleaning products, and various other chemicals.

From the balanced equation:

1 mole of NH₂ reacts with 2 moles of H₂ to produce 2 moles of NH₃

Therefore, to fully use 2.5 moles of NH₂, we would need 2.5 x 2 = 5 moles of H₂.

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Explanation: the answer is 3840 because 2950+890=3840

Ascorbic acid, also known as Vitamin C, is a water-soluble vitamin that plays an important role in many biological processes in the human body

For the first part

Step 1: Write the dissociation reactions of H₂C₆H₆O₂ in water:

H₂C₆H₆O₂ ⇌ H⁺ + HC₆H₆O²⁻

HC₆H₆O²⁻ ⇌ H⁺ + C₆H₆O₂²⁻

Step 2: Write the equilibrium expressions for each dissociation reaction:

Kₐ₁= [H⁺][HC₆H₆O²⁻ ] / [H₂C₆H₆O₂]

Kₐ₂= [H⁺][C₆H₆O₂²⁻] / [ HC₆H₆O²⁻]

Step 3: Use the given values of Kₐ₁ and Kₐ₂ to set up an ICE table and solve for [H⁺] and pH.

Kₐ₁  = 8.00×10⁻⁵

Kₐ₂ = 1.60×10⁻¹²

[H₂C₆H₆O₂] = 0.190 M

Let x be the concentration of [H⁺] from the dissociation of H₂C₆H₆O₂

[H⁺] = x M

[HC₆H₆O²⁻] = x M

[C₆H₆O₂²⁻] = x(Kₐ₁/Kₐ₂) M

Now, we can substitute the values into the equilibrium expressions to get:

Kₐ₁ = (x)(x) / (0.190-x)

Kₐ₂ = (x)(x(Ka1/Ka2)) / x

Simplifying and solving for x, we get:

x = 7.62 × 10⁻⁴ M

pH = -log[H⁺] = 3.12

Therefore, the pH of a 0.190 M ascorbic acid solution is 3.12.

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The standard change in Gibbs free energy for the given reaction at 25°C is -757.9 kJ/mol.

Gibbs energy, also known as Gibbs free energy, is a thermodynamic quantity used to determine the maximum amount of work that can be obtained from a system at a constant temperature and pressure. It is denoted by the symbol G and is named after the American physicist Josiah Willard Gibbs who introduced the concept in the late 19th century.

Gibbs energy is defined as the difference between the enthalpy of a system and the product of the temperature and the entropy of the system:

G = H - TS

where H is the enthalpy, T is the temperature in Kelvin, and S is the entropy of the system.

The Gibbs energy is related to the equilibrium constant of a reaction through the following equation:

ΔG = -RTlnK

To calculate the standard change in Gibbs free energy for the given reaction at 25°C, we need to use the ΔG°f values (standard Gibbs free energy of formation) for the reactants and products involved in the reaction.

The ΔG°f values for Fe₂O₃(s), Al(s), Al₂O₃(s), and Fe(s) can be found in a table of thermodynamic data and are:

ΔG°f [Fe₂O₃(s)] = -824.2 kJ/mol

ΔG°f [Al(s)] = 0 kJ/mol

ΔG°f [Al₂O₃(s)] = -1582.3 kJ/mol

ΔG°f [Fe(s)] = 0 kJ/mol

The standard change in Gibbs free energy for the reaction can be calculated using the following equation:

Δ°rxn = ΣΔG°f(products) - ΣΔG°f(reactants)

Substituting the values, we get:

Δ°rxn = [ΔG°f(Al₂O₃(s)) + 2ΔG°f(Fe(s))] - [ΔG°f(Fe₂O₃(s)) + 2ΔG°f(Al(s))]

Δ°rxn = [(-1582.3 kJ/mol) + 2(0 kJ/mol)] - [(-824.2 kJ/mol) + 2(0 kJ/mol)]

Δ°rxn = -757.9 kJ/mol

Therefore, the standard change in Gibbs free energy for the given reaction at 25°C is -757.9 kJ/mol.

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C. The pH stays about the same.

Answer:

C.The pH stays about the same.

Explanation:

Buffer reactions maintain stable pH of solutions.

a. The product of the reaction between [tex]H_{3}C[/tex]-C=CH₂ and [tex]Br_{2}[/tex] is 1,2-dibromo-2-methylpropane:  [tex]H_{3}C[/tex]-C=CH₂ + [tex]Br_{2}[/tex]  → BrCH₂ -CH(Br)-[tex]CH_{3}[/tex]

b. The product of the reaction between  [tex]H_{3}C[/tex]-CH=CH-[tex]CH_{3}[/tex] and conc.  [tex]H_{2}SO _{4}[/tex] is 2-methylpropene:

[tex]H_{3}C[/tex]-CH=CH-[tex]CH_{3}[/tex] + [tex]H_{2}SO _{4}[/tex] →  [tex]H_{3}C[/tex]-C([tex]CH_{3}[/tex])=CH₂ + H₂O

c. The product of the reaction between [tex]KMnO_{4}[/tex] (aq) and any organic compound is typically a mixture of products, depending on the specific organic compound being reacted. Therefore, the structure of the product cannot be determined without additional information about the organic compound being reacted.

d. NR means that no reaction occurs.

What is product of the reaction ?

In chemistry, the product of a reaction refers to the substances that are formed as a result of a chemical reaction. These substances are formed by the rearrangement of atoms and molecules in the reactants. The products of a chemical reaction are typically represented by a chemical equation, which shows the reactants on the left side of the equation and the products on the right side of the equation. In many cases, the products of a chemical reaction have different properties than the reactants, and they can be used in a variety of applications in chemistry, biology, and other fields.

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Answer:

silicon dioxide,xenon

Explanation:

A sample of oxygen gas at 70 degrees Celsius is not twice as hot as a sample of oxygen gas at 35 degrees Celsius.

What is Temperature?

Temperature is a physical property that describes the degree of hotness or coldness of a substance, typically measured with a thermometer in units such as Celsius or Fahrenheit. It is a measure of the average kinetic energy of the particles that make up a substance, with higher temperatures indicating greater kinetic energy and lower temperatures indicating less kinetic energy.

The temperature difference between the two samples is 35 degrees Celsius, not 70 degrees Celsius. Temperature is a measure of the average kinetic energy of the particles in a substance, and it is on an absolute scale (Kelvin).

As we can see, the temperature in Kelvin of oxygen gas at 70 degrees Celsius (343.15 K) is not twice the temperature of oxygen gas at 35 degrees Celsius (308.15 K). Therefore, a sample of oxygen gas at 70 degrees Celsius is not twice as hot as a sample of oxygen gas at 35 degrees Celsius.

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Around 80.5 KJ

Multiply Heat of Fusion and Mass to get the q value.

The order for reactant A is 2 and the order for reactant B is 1. For the first reaction, the overall order of the reaction is 3 and for the second reaction, the overall order of the reaction is 5.

The order of a reaction is the sum of the exponents in the rate law expression that relates the rate of a chemical reaction to the concentrations of the reactants.

To determine the order of each reactant, we need to compare the initial rates of reaction at different concentrations while keeping the concentration of the other reactant constant.

For reactant A:

Exp#1 (0.100 M A, 0.100 M B): initial rate = k(0.100)^2(0.100) = 0.001 k

Exp#2 (0.200 M A, 0.100 M B): initial rate = k(0.200)^2(0.100) = 0.004 k

Exp#3 (0.100 M A, 0.200 M B): initial rate = k(0.100)^2(0.200) = 0.002 k

We can see that when the concentration of A doubles (Exp#1 to Exp#2), the initial rate quadruples, which indicates that A is second order. When the concentration of B doubles (Exp#1 to Exp#3), the initial rate doubles, which indicates that B is first order.

Therefore, the order for reactant A is 2 and the order for reactant B is 1.

To determine the overall order of the reaction, we add the orders of the reactants:

Overall order = 2 (order of A) + 1 (order of B) = 3

Therefore, the overall order of the reaction is 3.

For the second reaction, we can see that the rate depends on the concentration of both reactants, and we cannot determine their individual orders without further information or experiments. However, we can determine the overall order of the reaction by adding the exponents of the concentration terms in the rate law:

Overall order = 1 + 4 = 5

Therefore, the overall order of the reaction is 5.

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When sodium carbonate is titrated against HCl in the presence of the indicator phenolphthalein, it is transformed to NaCl.

To decolorize phenolphthalein, 50 mL of a combination of NaOH and Na2CO3titrated with N10 HCl using phenolphthalein indicator required 50 mL of HCl. At this point, methyl orange was added, and the acid addition was continued. The second endpoint was obtained when another 10 ml of N10 HCl was added.

You can use more than one indicator since the interaction between sodium carbonate and hydrochloric acid occurs in two phases. The first stage is better served by phenolphthalein, whereas the second is best served by methyl orange.

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