A student was given a 2.919-g sample of a mixture of potassium nitrate and potassium bromide and was asked to find the percentage of each compound in the mixture. He dissolved the sample and added a solution that contained an excess of silver nitrate, AgNO3. The silver ion precipitated all of the bromide ion in the mixture as AgBr. It was filtered, dried, and weighed. Its mass was 2.916 g. What was the percentage of each compound in the mixture?

The percent yield of HF is 3.68%.

What is the balanced equation?

When both the reactant and product sides of a chemical equation have the same amount of atoms of each element, the equation is said to be balanced. In other words, both sides of the equation have equal amounts of mass and charge.

We must first calculate the limiting reactant of the reaction before we can determine the theoretical yield of HF. This can be accomplished by evaluating the stoichiometric ratio in the balanced equation and the number of moles of each reactant.

Molar mass of NH3 = 17.03 g/mol

Molar mass of F2 = 38.00 g/mol

Number of moles of NH3 = 57.10 g / 17.03 g/mol

                                          = 3.356 mol

Number of moles of F2    = 57.10 g / 38.00 g/mol

                                          = 1.503 mol

The balanced equation states that 2 moles of NH3 combine with 5 moles of F2 to create 6 moles of HF.

Since NH3 yields less product than F2 would if it were totally consumed, it follows that NH3 is the limiting reactant.

No. of moles of HF produced = 3.356 mol NH3 x (6 mol HF / 2 mol NH3)

                                                 = 10.07 mol HF

Molar mass of HF = 20.01 g/mol

Theoretical yield of HF = 10.07 mol HF x 20.01 g/mol

                                       = 201.6 g HF

The percent yield is calculated by dividing the actual yield by the theoretical yield and then multiplying by 100%.

percent yield = (actual yield / theoretical yield) x 100%

percent yield = (7.430 g / 201.6 g) x 100%

percent yield = 3.68%

Therefore, the percent yield of HF is 3.68%.

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The gas constant for this ideal gas is approximately 62.4 L mmHg/mol K.

We can use the ideal gas law to solve this problem, which is:

PV = nRT

We are given that one mole of an ideal gas occupies a volume of 20.0 L at a pressure of 930 mmHg and a temperature of 25°C (298.15 K). We can substitute these values into the ideal gas law and solve for the unknown variable:

PV = nRT

(930 mmHg) * (20.0 L) = (1 mol) * R * (298.15 K)

Simplifying and solving for R, we get:

R = (930 mmHg * 20.0 L) / (1 mol * 298.15 K)

R ≈ 62.4 L mmHg/mol K

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The molarity of the dye in a solution with an absorbance of 0.204 at this wavelength is 5.89×10⁻⁴ M.

Molarity is defined as a measure by which concentration of chemical substances present in a solution are determined. It is defined in particular reference to solute concentration in a solution . Most commonly used unit for molar concentration is moles/liter.

We can solve this problem by using the following formula:

A = kC

Where A is the absorbance, k is the constant characteristic for each substance, and C is the molar concentration of the analyte.

0.118 = 200.4 M⁻¹  C

And solve for C:

C = 5.89 x10⁻⁴ M

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We must select an acid-base combination with a pKa value close to the target pH in order to construct a buffer with a pH of 4.0. The acetic acid (CH3COOH) and sodium acetate (CH3COONa) combination has a pKa of 4.76, which is sufficiently near to the desired pH of 4.0, as can be seen from the table.

To calculate the required amounts of each component, we can use the Henderson-Hasselbalch equation:

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

where [A-] is the concentration of the conjugate base (CH3COO-) and [HA] is the concentration of the weak acid (CH3COOH).

We want to prepare 1.0L of a 0.2M buffer, which means we need:

0.2 mol/L x 1.0 L = 0.2 mol of total buffer components

Since the acid and its conjugate base are used in equal amounts, we can split this total amount in half:

0.2 mol/2 = 0.1 mol of CH3COOH and 0.1 mol of CH3COO-

Now we can use the Henderson-Hasselbalch equation to solve for the required concentrations of each component:

4.0 = 4.76 + log([CH3COO-]/[CH3COOH])

-0.76 = log([CH3COO-]/[CH3COOH])

10^-0.76 = [CH3COO-]/[CH3COOH]

0.218 = [CH3COO-]/[CH3COOH]

We know that [CH3COOH] + [CH3COO-] = 0.2 mol/L, so we can use the above ratio to calculate:

[CH3COOH] = (0.2 mol/L) / (1 + 0.218) = 0.162 M

[CH3COO-] = 0.218 x [CH3COOH] = 0.035 M

Therefore, to prepare 1.0L of a 0.2M buffer with a pH of 4.0, we would need to mix 81.6g of acetic acid (CH3COOH) and 3.5g of sodium acetate (CH3COONa) in 1.0L of water.

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A buffer is a solution that resists large changes to its pH upon the addition of small quantities of strong acids or bases, neutralising these additions and thus maintaining its pH relatively stable. This property makes them useful for calibrating pH metres and also a number of processes in the natural environment, for example, maintaining blood pH in the body.

To effectively maintain a pH range, a buffer must consist of a weak conjugate acid-base pair, meaning either a. a weak acid and its conjugate base, or b. a weak base and its conjugate acid. For example, an acetic acid/acetate buffer:

[tex]\rm CH_3COOH_{\,(aq)}+H_2O_{\,(aq)} \rightleftharpoons CH_3COO^-_{\,\,(aq)}+H_3O_{\,(aq)}[/tex]

A buffer is able to resist pH change because the two components (conjugate acid and conjugate base) are both present in equimolar concentrations at equilibrium and are thus able to neutralize small additions (in the form of H3O⁺ and OH⁻) when they are added to the solution.

From a Le Chatelier's Principle perspective:

upon addition of an acid, the basic component of the buffer will react with the acid, and equilibrium will shift to the left, reducing hydronium ion concentration, and thus minimising pH change.

Upon addition of a base, the acidic component of the buffer will react with the base, and equilibrium will shift to the right, increasing hydronium concentration, and thus minimising pH change.

The maintenance of blood pH levels, is regulated primarily by the bicarbonate/carbonic acid buffer:

[tex]\boxed{\rm H_2CO_{3\,(aq)}+H_2O_{\,(l)} \leftrightharpoons HCO_3^{\,\,-}_{(aq)}+H_3O^+_{\,\,\,(aq)}}[/tex]

When blood pH drops into the acidic range, this buffer shifts to the carbonic acid side producing more carbonic acid. This causes the equilibrium to shift to the carbon dioxide side in this secondary buffer (below), and expel the gas through the lungs, thus maintaining pH:

[tex]\boxed{\rm CO_{2\,(g)}+H_2O_{\,(aq)}\leftrightharpoons H_2CO_{3\,(aq)}}[/tex]

Under alkaline conditions, bicarbonate ions are removed from the blood by the kidneys and excreted out via urine. The buffer thus brings the pH back to within the desired range by shifting to the bicarbonate side.

Another tertiary buffering system involved in keeping the blood pH level steady, is the haemoglobin/oxyhaemoglobin buffer:

[tex]\boxed{\rm HHb^+_{\,\,\,\,(aq)}+H_2O_{\,(l)}+O_{2\,(aq)}\leftrightharpoons HbO_{2\,(aq)}+H_3O^+_{\,\,\,\,(aq)}}[/tex]

A rise in oxyhaemoglobin levels due to oxygen absorption by the haemoglobin in the blood is associated with an increase in acidity as the haemoglobin equilibrium shifts to the right. At this point, the primary buffers, as shown above previously, becomes involved to reduce acidity while oxygen is delivered to the cells.

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Answer: the molecular formula of the compound is Fe4O5

Explanation: According to the provided data, it can be inferred that the chemical compound is comprised of 72.3% iron and 27.7% oxygen in terms of their respective masses. Assuming a sample mass of 100 g of the compound, it can be postulated that the sample would comprise of:

A mass of 72.3 grams of iron (Fe) was measured.

A quantity of 27.7 grams of oxygen (O) was measured.

To determine the empirical formula, it is essential to transform the given masses into moles by utilizing their corresponding atomic masses.

The molar quantity of Fe can be computed by dividing the given mass of 72.3 grams by the molar mass of iron, which is 55.85 grams per mole. Employing this formula, we obtain a value of 1.294 moles for the quantity of Fe.

The number of moles of O can be computed by dividing the mass of O by its molar mass. In the present case, the number of moles of O is equivalent to 1.731 mol, given that the mass of O is 27.7 g and its molar mass equals 16 g/mol.

Subsequently, it is necessary to identify the most basic integer ratio of iron (Fe) to oxygen (O) atoms. In order to accomplish this, the quantity of moles attributable to every element is partitioned by the minimal quantity of moles present.

The Fe:O ratio was determined to be 1:1, as indicated by a molar ratio of 1.294 mol Fe to 1.294 mol O.

The stoichiometric ratio between oxygen and iron in the given system is represented by the numerical value of 1.337, which is the result of the division of 1.731 moles of oxygen by 1.294 moles of iron.

The requirement to achieve an integral value for the O:Fe ratio necessitates the application of a common multiplier to both ratios. A straightforward approach to accomplish this task entails the multiplication of both ratios by a factor of 4:

The ratio of Fe to O, expressed as Fe:O, is equivalent to 1 multiplied by 4, which yields a result of 4.

The stoichiometric ratio between oxygen and iron, denoted as O:Fe ratio, is calculated by multiplying the numerical value 1.337 with the factor of 4, resulting in a value of 5.348.

The nearest whole number can be utilized to approximate the O:Fe ratio, yielding the following expression:

The Fe:O ratio exhibits a value of 4.

The ratio between the amounts of oxygen and iron, denoted as O:Fe, is equal to 5.

Hence, it can be derived that the chemical composition of the compound is represented by the empirical formula Fe4O5.

The identification of a compound's molecular formula necessitates the determination of its molecular mass. It is given that the molecular mass is 231.4 g/mol. The calculation of the empirical formula mass for Fe4O5 can be performed.

The calculation of the molecular weight of Fe4O5 can be expressed as follows: the total mass is a result of adding the individual atomic weights of four iron atoms (each with a molar mass of 55.85 g/mol) and five oxygen atoms (each with a molar mass of 16 g/mol), leading to a final mass of 231.4 g/mol.

The identity of the empirical formula and the molecular formula can be inferred, as they share congruent molecular masses.

If He atoms (mass 4), Ne atoms(10), Ar atoms (40) and Kr atoms

(84) at the same temperature, the true about their average kinetic energy is: D) They all have the same KE.

This is due to the fact that temperature serves as a proxy for the average kinetic energy of the gas molecules. All gas molecules have the same average kinetic energy at a given temperature, which is proportional to the temperature in kelvin.

Because the velocity of each molecule is inversely proportional to its mass, the more massive molecules move slower and the less massive molecules move faster, but their average kinetic energies are equal even though different gas molecules have different masses.

Therefore the correct option is D.

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Temperature is an nonliving limiting factor because it affects the amount of sea ice available for animals to live on statements is a reasonable conclusion about the Arctic ecosystem.

Option B is correct.

Further warming of the Arctic, the erosion of Arctic coastlines, and a disruption in global weather patterns will all result from the continued loss of Arctic sea ice. The Arctic's communities and ecosystems will be further disrupted as a result of the loss of sea ice.

Many of the current changes in the Arctic are being driven by rising temperatures that are three times faster than the global average annually. Most notably, ice and snow are melting at a faster rate. Both local ecosystems and the global climate system are affected by this.

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The simplest hydrocarbon molecule that accommodates only hydrogens and 5 carbons is pentane, which has the molecular formula C5H12.

What is Carbon?

Carbon is a chemical element with the symbol C and atomic number 6. It is a nonmetallic element and belongs to group 14 of the periodic table. Carbon is an essential element for life and is the basis for all known organic compounds. It is the fourth most abundant element in the universe by mass and is the second most abundant element in the human body by mass after oxygen.

Hydrocarbons are organic molecules that contain only hydrogen and carbon atoms. The simplest hydrocarbon is methane (CH4), which has only one carbon atom and four hydrogen atoms. As the number of carbon atoms in a hydrocarbon molecule increases, so does the complexity of its structure.

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(a) The solubility product expression for Ag2CO3 is:

Ksp = [Ag+]^2[CO3^2-]

(b) The solubility product expression for Hg2Cl2 is:

Ksp = [Hg2^2+][Cl^-]^2

Separating the solid silver chloride from the nitric acid solution is a physical change, not a chemical change. This is because no chemical reaction takes place during this process, and the properties of the silver chloride remain the same. Only the physical state of the substance changes, from dissolved in the solution to a solid precipitate.

While this answer may provide helpful information for your assignment, it is important to remember that using it verbatim could be seen as plagiarism. To avoid this, it is best to use your own words and properly cite any sources used. This will ensure that you are giving credit to the original author and presenting your own unique perspective on the topic.

~~~Harsha~~~

The redox reactions is balanced as by adding coefficients as follows:2 H+ +ClO²⁻+I⁻⟶2 Cl⁻+H₂O+I₂.

Redox reactions comprise of two parts a reduced part and an oxidized part, which occur simultaneously . The part which is reduced gain electrons and hence there is a increase in oxidation state of the species.

While, the part which is oxidized looses electrons and hence there is a decrease in oxidation state of the species.During redox reactions, there is no net change in the number of electrons . Electrons which are given off in oxidation are used up in reduction.These too are balanced by adding coefficients.

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Answer:

AgCl = 0.0133 mol

Explanation:

The balanced chemical equation for the reaction between AgNO3 and CaCl2 is:

AgNO3 + CaCl2 → AgCl + Ca(NO3)2

From the equation, we can see that 1 mole of AgNO3 reacts with 1 mole of CaCl2 to produce 1 mole of AgCl. Therefore, we need to determine the number of moles of AgNO3 and CaCl2 in the given volumes of solutions and use the stoichiometric coefficients to calculate the number of moles of AgCl produced.

First, let's calculate the number of moles of AgNO3 in 63.57 mL of 1.327 M solution:

moles of AgNO3 = volume (in L) x concentration

moles of AgNO3 = 63.57 mL x 1 L/1000 mL x 1.327 mol/L

moles of AgNO3 = 0.0844 mol

Next, let's calculate the number of moles of CaCl2 in 41.87 mL of 0.317 M solution:

moles of CaCl2 = volume (in L) x concentration

moles of CaCl2 = 41.87 mL x 1 L/1000 mL x 0.317 mol/L

moles of CaCl2 = 0.0133 mol

Since we have more AgNO3 than CaCl2, CaCl2 is the limiting reagent. Therefore, the number of moles of AgCl produced is equal to the number of moles of CaCl2:

moles of AgCl = 0.0133 mol

The value of Kc at equilibrium, the concentration of A is 0.213 mol/L 1.79.

When it comes to reversible chemical reactions, the equilibrium constant (K) is a crucial factor that measures the relative quantities of reactants and products present at equilibrium. This value is determined by calculating the ratio of product concentrations (or partial pressures) to reactant concentrations (or partial pressures), each raised to the power of its stoichiometric coefficient in the balanced chemical equation. In simpler terms, K helps to gauge how much of a chemical reaction has taken place by comparing reactant and product levels.

Equation:

Kc = [C]/[A][B]²

At equilibrium, if the concentration of A is 0.213 mol/L, and we assume that the initial concentrations of A and B were equal, then the concentration of B at equilibrium will be:

[B] = (3.00 - 2.00*[0.213])/6.00 = 0.1985 mol/L

Substituting the values into the equilibrium constant expression, we get:

Kc = [C]/[A][B]² = x/(0.213*0.1985²)

We need to determine the value of x, which is the concentration of C at equilibrium. To do this, we can use the fact that the stoichiometric coefficient of C is 1, and the stoichiometric coefficients of A and B are 1 and 2, respectively. Therefore, at equilibrium:

[C] = Kc*[A][B]² = Kc(0.213)*(0.1985)²

We know that [C] is the same as x, so:

x = Kc*(0.213)*(0.1985)²

We also know that the initial concentration of C was zero, so the final concentration of C at equilibrium is equal to x. Therefore, we can use the concentration of C at equilibrium, x, to solve for the equilibrium constant Kc:

Kc = x/([A][B]²) = x/(0.2130.1985²) = (x/(mol/L))/((0.213 mol/L)*(0.1985 mol/L)²)

Using a calculator, we get:

Kc = 1.79

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Answer:

If you take a closer picture I'll be able to help you.

It's hard to read.

The correct statement is that; Electrons are being shared between nitrogen and hydrogen. Option D

A sort of chemical link known as a covalent bond is created when two atoms share electrons. The electrons that both atoms share are held in a stable balance by a force exerted by both atoms in a covalent link.

Although there are some exceptions, covalent bonds, which are the not as strong as the ionic bonds, are typically created between nonmetal atoms. The ionic bonds are quite stronger than they are.

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The rate constant of the reaction from the calculation can be obtained as  0.041 s-1.

A first-order reaction is one in which one of the reactants' concentration is raised to the first power, directly affecting the reaction's pace. This implies that the pace of the reaction drops proportionally as the reactant concentration does over time.

We know that;

ln[A] = ln[A]o - kt

ln[A]  - ln[A]o  = - kt

k = ln[A]  - ln[A]o/-t

k = ln(3.00×10−3) - ln(5.90×10−2)/ -85

k = - 5.8 - (-2.3)/-85

k = 0.041 s-1

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The liters of 3.000 M HCl are needed to make 0.500 L of 0.100 M HCl is 0.017 L. The correct option to this question is A.

Using the equation ,

[tex]M_{1} V_{1} =M_{2}V_{2}[/tex]

Substituting the values in the above equation,

0.1×0.5=3×[tex]V_{2}[/tex]

[tex]V_{2}[/tex] = [tex]\frac{0.1*0.5}{3}[/tex]

[tex]V_{2}[/tex]= 0.017 L

An analogous dilution issue exists here. Keep in mind that[tex]M_{1} V_{1} =M_{2}V_{2}[/tex] , where [tex]M_{1}[/tex] is the starting concentration, [tex]V_{1}[/tex] is the initial volume,  [tex]M_{2}[/tex] is the concentration following mixing or dilution, and [tex]V_{2}[/tex] is the total final volume.

Dilution is the name given to this procedure. Using the following equation, we can link the volumes and concentrations before and after a dilution: Where [tex]M_{1}[/tex]and [tex]V_{1}[/tex] stand for the volume and molarity of the initial concentrated solution, respectively, and [tex]M_{2}[/tex] and [tex]V_{2}[/tex] for the volume and molarity of the final diluted solution, respectively, we have [tex]M_{1} V_{1} =M_{2}V_{2}[/tex].

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The addition in hydrochloric acid is required to neutralize the remaining Grignard reagent and convert its magnesium alcoholate to alcohol.

Abstract. In the food, textile, metal, or rubber industries, hydrochloric acid (also known as is commonly used to neutralize alkaline agents and as a bleaching agent. When released into the soil, it is neutralized, and when exposed to water, it rapidly hydrolyzes.

The'strong' conventional acids found in a normal chemistry lab are brutal, but still orders a factor weaker than a superacid. For example, hydrochloric acid has a pH of about 1.6, nitric acid has a pH of 1.08, or pure sulfuric acid has a pH of -12.

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The amount of heat absorbed by the silver bar of mass 255.0g is 2,479.63 Joules.

The amount of heat absorbed or released by a substance can be calculated using the following expression;

Q = mc∆T

Where;

According to this question, a silver bar with a mass of 255.0 g is heated from 25°C to 65.5°C. The amount of heat absorbed by this bar of silver is as follows;

Q = 255 × 0.2401 × (65.5 - 25)

Q = 2,479.63 Joules

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Answer: Neither of these two substances would precipitate out.

Explanation: At a specific temperature, the highest quantity of a substance that can be dissolved in a particular solvent is commonly defined as its solubility. At a temperature of 20°C, a maximum of 36 grams of sodium chloride can dissolve in one liter of water, indicating the solubility of sodium chloride to be 36 g/L. In the same vein, at a temperature of 20°C, a maximum of 920 grams of iron (III) chloride can dissolve in one liter of water, indicating a solubility of 920 g/L.

Given that both elements are already dissolved within the solution, there is no basis for speculating that either component may separate out. In the event that the level of substance in the solution surpasses its solubility limit, leading to saturation, the surplus amount would undergo precipitation.

The term molarity is one of the most important methods which is used to calculate the concentration of a solution. It is mainly employed to calculate the concentration of a binary solution. The molarity is 13.0 mL. The correct option is B.

The molarity of a solution is defined as the number of moles of the solute present per litre of the solution. It is represented as 'M' and its unit is mol / L.

For two solutions, the equation connecting molarity and volume is:

M₁V₁ = M₂V₂

V₁ = M₂V₂ / M₁

V₁ = 0.200 × 250 / 4.000  = 12.5 mL ≈ 13.0 mL

Thus the correct option is B.

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One obstacle to seeing the true colors of metal ions is the presence of low concentrations of ligands such as water molecules or other molecular complex ions. This is known as the ‘ligand field effect’.

A ligand is an ion or molecule (functional group) that interacts with a main metal atom to produce a coordination complex in coordination chemistry. One or more electron pairs from the ligand are often formally donated to the metal as part of the bonding process, frequently using Lewis bases. Covalent and ionic bonds can form between metals and ligands. The metal-ligand bond order might additionally range from one to three. Although Lewis acidic "ligands" have been discovered to occur in a few rare instances, ligands are generally thought of as Lewis bases.

Lewis bases are chemical atomic or molecular species with a highly confined HOMO (The Highest Occupied Molecular Orbital). As mentioned earlier, these chemical entities have the capacity to donate an electron pair to a specific Lewis acid in order to form an adduct.

Ammonia, alkyl amines, and other traditional amines are the most prevalent Lewis bases. The pKa of the matching parent acid determines the base strength of Lewis bases, which are typically anionic in nature. Lewis bases can be categorized as nucleophiles since they are electron-rich entities with the capacity to give electron-pairs. Lewis acids, which act as electron-pair acceptors, can also be categorized as electrophiles.

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The absorbance reading would be affected if you did not wipe your fingerprints off from the cuvette before measuring in a spectrophotometer.

The fingerprints will interfere with the accuracy of the reading by absorbing or reflecting light which will resuls in a higher or lower absorbance value than the actual value.

This is because the oils and salts present in fingerprints can alter the path of light passing through the cuvette which then leads to inaccurate readings. So, it is important we ensure that the cuvette is clean and free of any contaminants to obtain precise and reliable absorbance readings in spectrophotometry.

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The reaction's equilibrium constant is 7.03×10¹².

The equilibrium constant for the reaction can be found using the following expression:

K = [Pb(OH)₃⁻][I⁻]²/ [PbI₂][OH⁻]³

The values of Ksp and Kf can be used to find the concentrations of the species involved in the reaction. Since Pb(OH)₃⁻ is a product of the reaction, its concentration can be expressed in terms of [PbI₂] and [OH⁻]:

[Pb(OH)₃⁻] = Kf[Pb²⁺][OH⁻]³ / (1 + Kf[Pb²⁺])

Since the reaction involves the dissolution of PbI₂, the initial concentration of PbI₂ can be assumed to be equal to its solubility product:

[PbI₂] = Ksp^(1/2)

Substituting these expressions into the equilibrium constant expression:

K = (Kf / Ksp^(3/2)) [OH⁻]³ / (1 + Kf[Pb²⁺])

Using the given values for Ksp and Kf:

K = (8×10¹³ / (8.70×10⁻⁹)^(3/2)) [OH⁻]³ / (1 + 8×10¹³ (Ksp^(1/2) / [OH⁻]))

Simplifying this expression:

K = 7.03×10¹² [OH⁻]³ / ([OH⁻] + 6.51×10⁻⁵)

Therefore, the equilibrium constant for the reaction is 7.03×10¹².

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Answer: The relative formula mass of Group 2 carbonate W is 36534 g/mol.

Explanation: We can use the ideal gas law to solve for the number of moles of gas produced:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

Assuming standard temperature and pressure (STP), which is 273 K and 1 atm, we can write:

(1 atm) (24 dm³) = n (0.08206 L atm/mol K) (273 K)

Solving for n, we get:

n = 1.0 mol

So, one mole of the Group 2 carbonate W produces 24 dm³ of gas at STP.

To find the relative formula mass of W, we need to know the molar mass of the carbonate. Let's assume the formula of the carbonate is MCO₃, where M is the Group 2 metal.

From the ideal gas law, we know that:

PV = nRT

or

n = PV/RT

We can rearrange this equation to solve for the molar mass of the carbonate:

M = m/n = PV/RTm

where m is the mass of the carbonate and M is the molar mass.

Since we know the volume of gas produced and the conditions at which it was produced, we can calculate the number of moles of carbonate that decomposed to produce the gas:

n = PV/RT = (1 atm) (24 dm³) / (0.08206 L atm/mol K) (273 K) = 0.986 mol

The molar mass of the carbonate is then:

M = m/n = 36000 g / 0.986 mol = 36534 g/mol

So, the relative formula mass of Group 2 carbonate W is 36534 g/mol.

The specific heat of aluminium when placed in temperature of the water of 31 degree Celsius is 0.077 J/kg K.

Specific heat capacity is defined as the amount of energy required to raise the temperature of one gram of substance by one degree Celsius. It has units of calories or joules per gram per degree Celsius.

It varies with temperature and is different for each state of matter. Water in the liquid form has the highest specific heat capacity among all common substances .

It is given by the formula in case of 2 substances as  ,

Q₁=m₁c₁ΔT₁=Q₂=m₂c₂ΔT₂ substitution in formula gives c₁=13×4.2×5/65×54=0.077 J/kg K.

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The maximum mass of CO₂ that could be produced is 4.27 g.

What is Mass?

Mass is a measure of the amount of matter in an object or substance. It is a scalar quantity, meaning it has only magnitude and no direction. Mass is typically measured in units such as grams or kilograms, and it is a fundamental property of matter that remains constant regardless of an object's location in the universe or the gravitational force acting upon it.

The balanced chemical equation for the reaction is:

CH₄ + 2O₂ → CO₂ + 2H₂O

The molar mass of methane (CH₄) is 16.04 g/mol.

The molar mass of oxygen (O₂) is 32.00 g/mol.

First, we need to determine which reactant is limiting and which is excess:

Moles of CH₄ = 3.53 g / 16.04 g/mol = 0.220 mol

Moles of O₂ = 6.2 g / 32.00 g/mol = 0.194 mol

From the balanced equation, we see that 1 mole of CH₄ reacts with 2 moles of O₂.

Since there is less O₂ than required to react with all of the CH₄, it is the limiting reactant. This means that CH₄ is in excess.

The number of moles of CO₂ that can be produced is equal to the number of moles of O₂:

0.194 mol O₂ × (1 mol CO₂ / 2 mol O₂) = 0.0970 mol CO₂

The mass of CO₂ that can be produced is:

0.0970 mol CO₂ × 44.01 g/mol = 4.27 g CO₂

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