How many hydrogen molecules (h2) are needed to convert the triacylglycerol shown to saturated fat

The volume of the gas at 23.20∘C and 0.990 atm is 7.12L.

The volume of a gas can be calculated using the combined gas law equation as follows;

PaVa/Ta = PbVb/Tb

Where;

According to this question, a sample of an ideal gas initially has a volume of 3.75 L at 10.60 ∘C and 1.80 atm. The resulting volume can be calculated as follows;

1.8 × 3.75/283.6 = 0.990 × Vb/296.2

0.0238 × 296.2 = 0.990Vb

Vb = 7.0498 ÷ 0.990

Vb = 7.12L

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The volume of ammonia needed to react completely with 30 Liters of NO at STP is 45 L.

The volume of ammonia needed to react completely with 30 Liters of NO at STP is calculated as follows;

4NH₃  + 6NO    →   5N₂   +  6H₂O

From the reaction given above, we can see that;

4 moles of ammonia ------------> 6 moles of NO

ratio = 4 : 6

The volume of ammonia required is calculated as;

4 -------------- > 6

30 L -----------> ?

? = (30 L x 6 ) / 4

? = 45 L

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We need to carry at least 187 CCCs on board the space shuttle to absorb all the CO2 produced by the crew during the 18-day mission.

To solve this problem, we need to use the following information:

First, we need to calculate the total amount of CO2 that will be expelled during the mission:

Total CO2 = 6 crew members x 42.0 g CO2/hour x 24 hours/day x 18 days = 136,080 g CO2

Next, we need to calculate the amount of LIOH needed to absorb this CO2. The balanced chemical equation for the reaction between CO2 and LIOH is:

CO2 + 2 LIOH → Li2CO3 + H2O

The molar mass of CO2 is 44.01 g/mol, and the molar mass of LIOH is 23.95 g/mol.

This means that 2 moles of LIOH are needed to absorb 1 mole of CO2.

So, to absorb 136,080 g of CO2, we need:

136,080 g CO2 x (1 mol CO2/44.01 g) x (2 mol LIOH/1 mol CO2) x (23.95 g LIOH/1 mol) = 139,648 g LIOH

Since each CCC contains 750 g of LIOH, we need:

139,648 g LIOH / 750 g CCC = 186.2 CCCs

Therefore, we need to carry at least 187 CCCs on board the space shuttle to absorb all the CO2 produced by the crew during the 18-day mission.

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The balanced chemical equation for the reaction between hydrochloric acid (HCl) and sodium bicarbonate [tex](NaHCO_3)[/tex] is:

[tex]HCl + NaHCO_3\ - > NaCl + CO_2 + H_2O[/tex]

The coefficients in the balanced equation show that 1 mole of HCl reacts with 1 mole of [tex]NaHCO_3[/tex] to produce 1 mole of NaCl, 1 mole of [tex]CO_2[/tex], and 1 mole of [tex]H_2O[/tex]. We need to find the number of moles of [tex](NaHCO_3)[/tex] present in the tablet.

2 grams of [tex]NaHCO_3[/tex] is equivalent to 0.02 moles, and 18 grams of HCl is equivalent to 0.45 moles. Since [tex](NaHCO_3)[/tex] is limiting reagent, only 0.02 moles of NaCl and [tex]CO_2[/tex] will be produced. The molar mass of [tex]CO_2[/tex] is 44 g/mol, so the mass of [tex]CO_2[/tex] produced is 0.88 g. The molar mass of NaCl is 58.44 g/mol, mass of NaCl produced is 1.17 g.

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The total mass of products obtained when 130 g of zinc react completely with HCl is 274 g (3rd option)

First, we shall determine the mass of each product obtained. Details below:

For ZnCl₂

2HCl + Zn -> ZnCl₂ + H₂

From the balanced equation above,

65 g of Zn reacted to produce 135 g of ZnCl₂

Therefore,

130 g of Zn will react to produce = (130 × 135) / 65 = 270 g of ZnCl₂

Thus, the mass of ZnCl₂ obtained is 270 g

For H₂

2HCl + Zn -> ZnCl₂ + H₂

From the balanced equation above,

65 g of Zn reacted to produce 2 g of H₂

Therefore,

130 g of Zn will react to produce = (130 × 2) / 65 = 4 g of H₂

Thus, the mass of H₂ obtained is 4 g

Finally, we shall determine the total mass of the product produced. Details below:

Total mass of product = mass of ZnCl₂ + mass of H₂

Total mass of product = 270 + 4

Total mass of product = 274 g (3rd option)

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Answer:

39.7

Explanation:

Therefore, the final temperature of the water is 39.7°C.

The number is converted to 60. 2 × 10²²

Index forms are simply described as mathematical forms that are used in the representation of numbers that are too small or too large in more convenient forms.

These index forms are also referred to as scientific notation or standard forms.

Some rules of index forms are;

From the information given, we have that;

0. 0602 × 10 ²⁵

Subtract three from the exponent value and move three spaces right, we have;

60. 2 × 10²⁵⁻³

60. 2 × 10²²

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Answer:

If an atom loses or gains electrons, it will become a positively or negatively charged particle, called an ion. The loss of one or more electrons results in more protons than electrons and an overall positively charged ion, called a cation.

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The pressure of N₂ gas produced when 42.57 g of NH₃ is reacted with excess NO in a sealed container is 4.95 atm

First, we shall determine the mole of 42.57 g of NH₃ that reacted. Details below:

Mole = mass / molar mass

Mole of NH₃ = 42.57 / 1 7

Mole of NH₃ = 2.50 moles

Next, we shall determine the mole of N₂ gas produced. Details below:

4NH₃ + 6NO -> 5N₂ + 6H₂O

From the balanced equation above,

4 moles of NH₃ reacted to produced 5 moles of N₂

Therefore,

2.50 moles of NH₃ will react to produce = (2.5 × 5) / 4 = 3.125 moles of N₂

Finally, we shall determine the pressure of N₂ gas produced. This is shown below:

PV = nRT

P × 28 = 3.125 × 0.0821 × 540

Divide both sides by 28

P = (3.125 × 0.0821 × 540) / 28

P = 4.95 atm

Thus, we can conclude that the pressure of N₂ gas produced is 4.95 atm

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the balanced equation and there reactions are as follow:

K₂O + H₂O → 2KOH

The reaction between potassium oxide and water produces potassium hydroxide (KOH).

F₂ + 2NaBr → 2NaF + Br₂

The reaction between fluorine gas and sodium bromide produces sodium fluoride and bromine.

2Ba(CIO3)₂ → 2BaCl₂ + 3O₂

The decomposition of barium chlorate produces barium chloride and oxygen gas.

SrBr₂ + (NH₄)₂CO₃ → SrCO₃ + 2NH₄Br

The reaction between strontium bromide and ammonium carbonate produces strontium carbonate and ammonium bromide.

C₈H₁₈ + 12O₂ → 8CO₂ + 9H₂O

The combustion of octane with oxygen produces carbon dioxide and water.

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The root mean squared velocity of molecules is 461.15 m/s

The root-mean square (RMS) velocity is the value of the square root of the sum of the squares of the stacking velocity values divided by the number of values.

The root-mean-square speed addresses both molecular weight and temperature, two parameters that have a direct influence on a material’s kinetic energy. The Maxwell-Boltzmann equation, which is the foundation of gas kinetic theory, defines the speed distribution for gas at a specific temperature.

Given,

Pressure = 1 atm = 101300 Pa

Density = 1.4290 kg/m³

c = [tex]\sqrt{\frac{3P}{d} }[/tex]

c = [tex]\sqrt{\frac{303900}{1.4290} }[/tex]

c = 461.15 m/s

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The correct molar mass for nickel chloride is 94.14 g/mol (option C).

Molar mass is the mass of a given substance divided by its amount, measured in moles. It is commonly expressed in grams (sometimes kilograms) per mole.

The molar mass of a substance can be calculated by summing up the atomic masses of the element components.

According to this question, the atomic mass of nickel is 58.693 amu while that of chlorine gas is 35.45 amu. The molar mass of nickel chloride can be calculated as follows;

molar mass = 35.45 amu + 58.693 amu = 94.14 g/mol

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The molar volume of a gas can be calculated using the ideal gas law:

PV = nRT

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

To solve for the molar volume of CO2 at 39°C (312 K) and 652 torr (0.859 atm), we can rearrange the ideal gas law as follows:

V = (nRT) / P

First, we need to calculate the number of moles of CO2. We can use the following equation, which relates the pressure, volume, number of moles, and temperature of a gas:

PV = nRT

Solving for n, we get:

n = (PV) / (RT)

Substituting the given values, we get:

n = (0.859 atm * V) / (0.08206 L·atm/mol·K * 312 K)

Now we can substitute this expression for n into the equation for the molar volume:

V = (nRT) / P

V = [(0.859 atm * V) / (0.08206 L·atm/mol·K * 312 K)] * (0.08206 L·atm/mol·K * 312 K) / (0.859 atm)

Simplifying, we get:

V = 24.45 L/mol

Therefore, the molar volume of CO2 at 39°C and 652 torr is 24.45 L/mol.

Answer: As they develop theories, chemists use models to attempt to explain their findings. Chemists assess the model they are using as new evidence becomes available and, if required, continue to refine it by making modifications.

Explanation:

The minimum concentration of fluoride ions necessary to precipitate [tex]CaF_2[/tex] from a [tex]5.25 * 10^{-3}[/tex] M solution of [tex]Ca(NO_3)_2[/tex] is [tex]6.09 * 10^{-5}[/tex] M.

The solubility product expression for [tex]CaF_2[/tex] is:

[tex]Ksp = [Ca_2^+}][F^-]^2[/tex]

We can use this expression to find the minimum concentration of fluoride ions necessary to precipitate [tex]CaF_2[/tex] from a [tex]5.25 * 10^{-3} M[/tex] solution of [tex]Ca(NO_3)_2[/tex].

First, we need to determine the initial concentration of [tex]Ca_2^+[/tex] ions in solution. Since [tex]Ca(NO_3)_2[/tex] dissociates into two [tex]Ca_2^+[/tex] ions and two [tex]NO_3^-[/tex]ions, the initial concentration of [tex]Ca_2^+[/tex] ions is:

[tex]Ca_2^+[/tex] = [tex]2 * 5.25 * 10^{-3} M = 1.05 * 10^{-2} M[/tex]

Next, we can use the solubility product expression to solve for the minimum concentration of fluoride ions required to precipitate [tex]CaF_2[/tex]:

Ksp = [[tex]Ca_2^+[/tex]][tex][F^-]^2[/tex]

[tex]3.9 * 10^{-11} = (1.05 * 10^{-2} M)([F^-]^2)[/tex]

[tex][F^-]^2 = (3.9 * 10^{-11})/(1.05 * 10^{-2} M) = 3.71 * 10^{-9}[/tex]

[tex][F^-] = \sqrt{(3.71 * 10^{-9}) } = 6.09 * 10^{-5} M[/tex]

Therefore, the minimum concentration of fluoride ions necessary to precipitate [tex]CaF_2[/tex] from a [tex]5.25 * 10^{-3}[/tex] M solution of [tex]Ca(NO_3)_2[/tex] is [tex]6.09 * 10^{-5}[/tex]M.

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Hydrazine, reacts with the oxygen to form the nitrogen gas and the water. The percent yield of the reaction is 3.18 %.

The balanced reaction is :

N₂H₄  + O₂  --->  N₂ + 2H₂O

The mass of the N₂H₄  = 3.55 g

The moles of N₂H₄ = mass / molar mass

The moles of N₂H₄ = 3.55 / 32

The moles of N₂H₄ = 0.110 mol

The theoretical yield = 0.110 mol × 28 g/mol

The theoretical yield = 3.08 g

The gas equation is :

P V = n R T

n = P V / R T

n = (1 × 0.850 ) / ( 0.0823 ×295 )

n = 0.0035 mol

The actual yield = 0.0035 × 28

The actual yield = 0.098 g

The percent yield = ( 0.098 / 3.08 ) × 100 %

The percent yield = 3.18 %.

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To identify the unknown alkene based on its H NMR spectrum, a qualified organic chemist would need to analyze the chemical shifts, integration values, and splitting patterns of the peaks in the spectrum, and compare them with known reference data and other spectroscopic techniques (such as C NMR, IR, and mass spectrometry) to make an accurate determination.

The alkene is likely to be a symmetrical alkene with two equivalent methyl groups attached to the double bond. This can be seen from the singlet at 1.7 ppm, which is characteristic of a methyl group, appearing twice in the spectrum. The ozonolysis of the alkene would lead to the formation of two carbonyl compounds, which are then oxidized to carboxylic acids under the given oxidizing conditions. Therefore, the alkene in question is likely to be cis-2-butene.

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The aluminum block absorbed 0.875 kJ of heat energy when it was dropped into the coffee.

let's calculate the heat lost by the coffee when it is cooled from its initial temperature of 90.0°C to its final temperature of 55.0°C:

Q1 = m1 * C1 * (90.0°C - 55.0°C)

Q1 = 850 g * 4.184 J/g °C * (90.0°C - 55.0°C)

Q1 = 125660 J

where m1 is the mass of the coffee, C1 is the specific heat of water.

Next, let's calculate the heat gained by the aluminum block when it is heated from 4.4°C to the final temperature of the mixture, which is 55.0°C:

Q2 = m2 * C2 * (55.0°C - 4.4°C)

Q2 = 18 g * 0.89 J/g °C * (55.0°C - 4.4°C)

Q2 = 875.16 J

where m2 is the mass of the aluminum block, and C2 is the specific heat of aluminum.

Since the energy lost by the coffee is gained by the aluminum block, we can set Q1 equal to Q2:

Q1 = Q2

125660 J = 875.16 J + m2 * C2 * (55.0°C - 4.4°C)

Solving for m2, we get:

m2 = (125660 J - 875.16 J) / (0.89 J/g °C * (55.0°C - 4.4°C))

m2 = 152.2 g

Therefore, the mass of the aluminum block that was dropped into the coffee is 152.2 g. To calculate the heat energy absorbed by the aluminum block, we can use the heat gained by the aluminum block that we calculated earlier:

Q2 = 875.16 J

Converting this to kJ, we get:

Q2 = 0.875 kJ

Therefore, the aluminum block absorbed 0.875 kJ of heat energy when it was dropped into the coffee.

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(a) The formal charge of Cl in the hypochlorite ion (ClO-) is +1.

(b) The formal charge of Cl in the perchlorate ion (ClO4-) with single bonds is +3.

For chlorine (Cl):

Valence electrons: 7

Non-bonding electrons: 6 (3 lone pairs)

Bonding electrons: 2 (1 single bond with oxygen)

Formal charge of Cl = 7 - 6 - (1/2 * 2) = 7 - 6 - 1 = +1

Hence, the formal charge of Cl in the hypochlorite ion is +1.

(c) The oxidation number of Cl in the hypochlorite ion is +1.

(d) The oxidation number of Cl in the perchlorate ion with single bonds is +7.

(e) In a redox reaction, the hypochlorite ion (ClO-) would be more easily reduced because it has a lower oxidation number (+1) compared to the perchlorate ion (+7).

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The partial pressure of the Helium gas is  0.9 atm.

The pressure that a gas exerts on its own when it is collected over water, independent of the pressure that the water vapor in the collecting vessel also produces, is known as its partial pressure.

When gas is collected over water, some of the water vapor will dissolve in it and change the overall pressure in the collecting vessel. Water vapor has its own partial pressure, which is affected by the relative humidity and temperature of the air around it. This is why it behaves in this way.

We have that;

Vapor pressure of the gas = 19.8 mmHg or 0.026 atm

Partial pressure of the Helium gas = 0.926 atm - 0.026 atm

= 0.9 atm

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We can use the formula:

Q = mcΔT

where Q is the heat absorbed or released, m is the mass, c is the specific heat, and ΔT is the change in temperature.

First, let's calculate the heat absorbed by the crown:

Q1 = mcΔT

Q1 = (1130 g)(0.129 J/g C)(98.8 C - 25.83 C)

Q1 = 107,776.6 J

Next, let's calculate the heat released by the crown into the water:

Q2 = mcΔT

Q2 = (m)(c)(ΔT)

Q2 = (1340 g)(4.184 J/g C)(27.84 C - 25.83 C)

Q2 = 11096.64 J

Since Q1 = -Q2 (heat lost by the crown is equal to heat gained by the water),

mcΔT = -mcΔT

We can then solve for the specific heat of the crown:

c = -(Q2/mΔT)

c = -(11096.64 J)/(1130 g)(27.84 C - 25.83 C)

c = 0.131 J/g C

The specific heat of pure gold is 0.129 J/g C, and the specific heat of the crown is 0.131 J/g C. Since the specific heat of the crown is slightly higher than that of pure gold, it is possible that the crown is not pure gold. However, other factors such as impurities or alloying metals can also affect the specific heat, so further analysis would be necessary to confirm if the crown is pure gold.

Answer:

0.636 moles of CO2

Explanation:

The molar mass of CO2 is 44.01 g/mol (12.01 g/mol for one carbon atom and 2 x 16.00 g/mol for two oxygen atoms). To find the number of moles in 28g of CO2, you can divide the mass by the molar mass: 28g / 44.01 g/mol = 0.636 moles of CO2.

Mark would need a thermometer to determine the temperature change of a solution during a chemical reaction. A thermometer is a tool used to measure temperature and can be used to monitor and record changes in temperature during a chemical reaction. So the answer is thermometer .

There are different types of thermometers, such as liquid-in-glass thermometers, bimetallic strip thermometers, digital thermometers, and infrared thermometers, among others. The choice of thermometer depends on the specific requirements of the experiment or process being carried out.

By measuring the initial and final temperatures of the solution before and after the chemical reaction, Mark can determine the temperature change, which is an important parameter in many chemical reactions as it provides information about the heat energy involved in the reaction, and helps in understanding the thermodynamics and kinetics of the process. Therefore the answer is thermometer .

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C₂H₄O₂ + NaHCO₃ —> NaC₂H₃O₂ + H₂O + CO₂ the amount of Carbon dioxide produced is 5.28 mg.

Water, CO₂ , and C₂H₃NaO₂ were produced when acetic acid and NaHCO₃ were combined. The chemistry is as follows: The reaction between vinegar and baking soda was endothermic.

Acetic acid:  2(12.01 g/mol) + 4(1.01 g/mol) + 2(16.00 g/mol)

                                              = 60.05 g/mol

NaHCO₃ 22.99 g/mol + 1.01 g/mol + 3(16.00 g/mol)

                                             = 84.01 g/mol

100 mg of Acetic acid is equal to 0.1 g, and 10 mg of NaHCO₃ is equal to 0.01 g.

Number of moles of Acetic acid = 0.1 g / 60.05 g/mol

                                             = 0.00167 mol

Number of moles of NaHCO₃  = 0.01 g / 84.01 g/mol

                                               = 0.00012 mol

Since NaHCO₃ has fewer moles, it is the limiting reactant.

Therefore, 0.00012 mol of NaHCO₃  will produce 0.00012 mol of CO₂

The mass of CO₂ produced can be calculated as follows:

Mass of CO₂ = Number of moles of CO₂  x Molar mass of CO₂

Mass of CO₂ = 0.00012 mol x 44.01 g/mol

                             = 0.00528 g or 5.28 mg

Therefore, the amount of CO₂ produced is 5.28 mg.

The theoretical yield of CO₂ is 0.00012 mol x 44.01 g/mol

                               = 0.00528 g or 5.28 mg.

This is equal to the actual yield of CO₂ produced.

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The correct number of molecules of ammonium acetate used, given that the student uses 0.100 mole of ammonium acetate in the reaction is 6.022×10²² molecules

The following data were obtained from the reaction:

The correct number of molecules of ammonium acetate used can be obtained as shown below:

From Avogadro's hypothesis,

1 mole of ammonium acetate = 6.022×10²³ molecules

Therefore,

0.1 mole of ammonium acetate = 0.1 × 6.022×10²³

0.1 mole of ammonium acetate = 6.022×10²² molecules

Thus, the number of molecules of ammonium acetate used is 6.022×10²² molecules

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The best statement that describes the three enzymes is: The enzymes have different structures because they have a different sequence of amino acids. Opton A is correct.

Enzymes are biological catalysts that facilitate chemical reactions in living organisms. Enzymes are proteins, and their function is determined by their three-dimensional structure, which is determined by the sequence of amino acids that make up the protein.

In this scenario, the three enzymes have different structures, which suggests that they have a different sequence of amino acids. This difference in amino acid sequence results in different folding patterns and ultimately different shapes of the enzymes. The specific shape of an enzyme determines its ability to catalyze a particular chemical reaction. Hence, the different structures of these enzymes indicate that they may perform different functions or catalyze different chemical reactions.

Option A, "The enzymes have different structures because they have a different sequence of amino acids," is the correct answer as it aligns with the fundamental principle of protein structure and function.

Option B, "The enzymes have the same sequence of amino acids because they are all digestive enzymes," is incorrect because enzymes can have different sequences of amino acids even if they perform the same function.

Option C, "The enzymes perform different functions because they have the same sequence of amino acids," is incorrect because the sequence of amino acids determines the enzyme's structure and thus its function.

Option D, "The enzymes break down the same molecules because they have a different sequence of amino acids," is also incorrect because different amino acid sequences can result in different substrate specificity, which means that the enzymes can break down different molecules. Therefore option A is correct.

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The information given can be used to construct the empirical formula for a tin oxide. We must first determine the mass of tin in the sample. This may be achieved by deducting the mass of the crucible, cover, and sample (21.76 g) from the mass of the empty crucible and cover (19.66 g).

This gives us a mass of 2.10 g of tin in the sample. The mass of oxygen in the sample must then be determined. To achieve this, we must deduct the mass of the crucible, cover, and sample (21.76 g) from the mass of the same components (22.29 g) prior to protracted heating. This provides us with an oxygen mass of 0.53 g.

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