Question 1

Calculate Δ_rS° for the following reaction. The S^∘for each species is shown below the reaction. C₂H₂(g)+ 2H₂(g)→ C₂H₆(g) S°(J K^-1 mol^-1)200.9 130.7 229.2

Accepted Answer

The answer of Calculate Δ_rS° for the following reaction. The...

Question 2

Identify the compound with the standard Gibbs energy of formation equal to zero.

Accepted Answer

The compound with a standard Gibbs energy of formation equal to zero is the element in its standard state. In this case, the only compound that is an element in its standard state is N₂(g), nitrogen gas, so the answer is B.

Question 3

Given the following equation, N₂O(g)+ NO₂(g)→ 3NO(g)Δ_rG° = -23.0 kJ mol^-1 Calculate Δ_rG° for the following reaction: 3N₂O(g)+ 3NO₂(g)→ 9NO(g)

Accepted Answer

For the given equation, Δ_rG° = -23.0 kJ mol^-1. The coefficients of both reactants and products are multiplied by 3 in the given equation, which means the reaction is scaled by a factor of 3. According to thermodynamics, entropy is an extensive property, which means it scales with the size of the system. Therefore, the entropy change of the reaction will also be scaled by a factor of 3. Hence, Δ_rG° for the scaled reaction will be: -23.0 kJ mol^-1 x 3 = -69.0 kJ mol^-1 Therefore, the correct answer is C.

Question 4

What is the change in Gibbs energy of a process?

Accepted Answer

The change in Gibbs energy (ΔG) is the maximum amount of energy available to do work in a process, which can be used to drive chemical reactions or physical processes. It takes into account both the entropy and enthalpy changes of the system, and determines whether the process is spontaneous (ΔG<0), non-spontaneous (ΔG>0), or at equilibrium (ΔG=0).

Question 5

Estimate Δ_rG° for the following reaction at 387 K. HCN(g)+ 2H₂(g)→ CH₃NH₂(g)Δ_rH°= -158.0 kJ mol^-1; Δ_rS°= -219.9 J K^-1 mol^-1

Accepted Answer

The answer of Estimate Δ_rG° for the following reaction at...

Question 6

Determine Δ_rG° at 298 K using the following information: CaCO₃(s)→ CaO(s)+ CO₂(g)Δ_rH°= +179.2 kJ mol^-1; Δ_rS°= +160.2 J K^-1 mol^-1

Accepted Answer

The answer of Determine Δ_rG° at 298 K using the...

Question 7

Given the following equation, N₂O(g)+ NO₂(g)→ 3NO(g)Δ_rG°= -23.0 kJ mol^-1 Calculate Δ_rG^o for the following reaction: 3NO(g)→ N₂O(g)+ NO₂(g)

Accepted Answer

The answer of Given the following equation, N₂O(g)+ NO₂(g)→ 3NO(g)Δ_rG°_...

Question 8

Calculate Δ_rS° for the following reaction. The S° for each species is shown below the reaction. N₂H₄(l)+ H₂(g)→ 2NH₃(g) S° (J K^-1 mol^-1)121.2 130.7 192.8

Accepted Answer

The answer of Calculate Δ_rS° for the following reaction. The...

Question 9

Calculate Δ_rS° for the following reaction. The S° for each species is shown below the reaction. 4NH₃(g)+ 5O₂(g)→ 4NO(g)+ 6H₂O(g) S°(J K^-1 mol^-1)192.8 205.2 210.8 188.8

Accepted Answer

The answer of Calculate Δ_rS° for the following reaction. The...

Question 10

Calculate Δ_rG° at 298 K using the following information: 2H₂S(g)+ 3O₂(g)→ 2SO₂(g)+ 2H₂O(g)Δ_rG°= ? Δ_fG°(kJ mol^-1)-33.4 -300.1 -228.6

Accepted Answer

The answer of Calculate Δ_rG° at 298 K using the...

Question 11

Estimate Δ_rG° for the following reaction at 449.0 K. CH₂O(g)+ 2H₂(g)→ CH₄(g)+ H₂O(g)Δ_rH°= -94.9 kJ mol^-1; Δ_rS°= -224.2 J K^-1 mol^-1

Accepted Answer

The answer of Estimate Δ_rG° for the following reaction at...

Question 12

Determine Δ_rG° at 298 K using the following information: H₂(g)+ CO(g)→ CH₂O(g) Δ_rH°= +1.9 kJ mol^-1; Δ_rS°= -109.6 J K^-1mol^-1

Accepted Answer

The answer of Determine Δ_rG° at 298 K using the...

Question 13

What is the name of the reaction that does NOT achieve the theoretical limits with respect to the change in Gibbs energy in thermodynamics?

Accepted Answer

Irreversible reactions do not achieve the theoretical limits with respect to the change in Gibbs energy because they proceed in only one direction and do not approach equilibrium. In contrast, reversible reactions can reach the theoretical limits because they can proceed in both the forward and reverse directions to approach equilibrium.

Question 14

What is the name of the reaction that achieves the theoretical limits with respect to the change in Gibbs energy in thermodynamics?

Accepted Answer

The reversible reaction achieves the theoretical limits with respect to the change in Gibbs energy in thermodynamics. This is because in a reversible reaction, the system can reach equilibrium state with the surroundings and the Gibbs energy change for the reaction can be minimized as close to zero as possible.

Question 15

Given the following equation, N₂O(g)+ NO₂(g)→ 3 NO(g)Δ_rG° = -23.0 kJ mol^-1 Calculate Δ_rG° for the following reaction: 9NO(g)→ 3N₂O(g)+ 3NO₂(g)

Accepted Answer

The answer of Given the following equation, N₂O(g)+ NO₂(g)→ 3...

Question 16

Estimate Δ_rG° for the following reaction at 775 K. 2Hg(g)+ O₂(g)→ 2HgO(s) Δ_rH°= -304.2 kJ mol^-1; Δ_rS°= -414.2 J K^-1 mol^-1

Accepted Answer

The answer of Estimate Δ_rG° for the following reaction at...

Question 17

Identify the compound with the lowest standard Gibbs energy of formation.

Accepted Answer

The compound with the lowest standard Gibbs energy of formation is the one with the most negative value. According to standard values, NaCl(s) has a standard Gibbs energy of formation of -384.12 kJ/mol, which is the most negative value among the given compounds. Therefore, the answer is A.

Question 18

Identify the compound with the highest standard Gibbs energy of formation.

Accepted Answer

The answer of Identify the compound with the highest standard...

Question 19

Calculate ΔρS° for the following reaction. The S° for each species is shown below the reaction. P₄(g)+ 10Cl₂(g)→ 4PCl₅(g) S°(J K^-1 mol^-1)280.0 223.1 364.6

Accepted Answer

The answer of Calculate ΔρS° for the following reaction. The...

Question 20

Determine Δ_rG° at 298 K using the following information: FeO(s)+ CO(g)→ Fe(s)+ CO₂(g)Δ_rH°= -11.0 kJ mol^-1; Δ_rS°= -17.4 J K^-1 mol^-1

Accepted Answer

First, we need to use the formula: ΔG° = ΔH° - TΔS° We are given: ΔH° = -11.0 kJ/mol ΔS° = -17.4 J/mol*K = -0.0174 kJ/mol*K T = 298 K Substitute these values into the formula and solve for ΔG°: ΔG° = (-11.0 kJ/mol) - (298 K)(-0.0174 kJ/mol*K) ΔG° = -11.0 kJ/mol + 5.19 kJ/mol ΔG° = -5.81 kJ/mol Since ΔG° is negative, the reaction is spontaneous. However, the question is asking for Δ_rG°, which is the standard free energy change at 298 K. This means we need to adjust our answer to account for the standard state conditions. We know that: ΔG° = ΔG°f (products) - ΔG°f (reactants) We can look up the standard free energy of formation values for FeO(s), CO(g), Fe(s), and CO₂(g) and substitute them into the formula. Let's label them as follows: FeO(s) --> A CO(g) --> B Fe(s) --> C CO₂(g) --> D We get: ΔG° = [ΔG°f (CO₂(g))] - [ΔG°f (FeO(s))] - [ΔG°f (CO(g))] = [20.2 kJ/mol] - [ -271.9 kJ/mol] - [-137.2 kJ/mol] = 191.1 kJ/mol Note that the values we looked up are in kJ/mol, so our final answer must also be in kJ/mol. Therefore, the answer is B) -5.8 kJ/mol.

Quiz 17: Gibbs Energy and Thermodynamics

Calculate Δ_rS° for the following reaction. The S^∘for each species is shown below the reaction. C₂H₂(g) + 2H₂(g) → C₂H₆(g) S°(J K^-1 mol^-1) 200.9 130.7 229.2

Identify the compound with the standard Gibbs energy of formation equal to zero.

Given the following equation, N₂O(g) + NO₂(g) → 3NO(g) Δ_rG° = -23.0 kJ mol^-1 Calculate Δ_rG° for the following reaction: 3N₂O(g) + 3NO₂(g) → 9NO(g)

What is the change in Gibbs energy of a process?

Estimate Δ_rG° for the following reaction at 387 K. HCN(g) + 2H₂(g) → CH₃NH₂(g) Δ_rH°= -158.0 kJ mol^-1; Δ_rS°= -219.9 J K^-1 mol^-1

Determine Δ_rG° at 298 K using the following information: CaCO₃(s) → CaO(s) + CO₂(g) Δ_rH°= +179.2 kJ mol^-1; Δ_rS°= +160.2 J K^-1 mol^-1

Given the following equation, N₂O(g) + NO₂(g) → 3NO(g) Δ_rG°= -23.0 kJ mol^-1 Calculate Δ_rG^o for the following reaction: 3NO(g) → N₂O(g) + NO₂(g)

Calculate Δ_rS° for the following reaction. The S° for each species is shown below the reaction. N₂H₄(l) + H₂(g) → 2NH₃(g) S° (J K^-1 mol^-1) 121.2 130.7 192.8

Calculate Δ_rS° for the following reaction. The S° for each species is shown below the reaction. 4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(g) S°(J K^-1 mol^-1) 192.8 205.2 210.8 188.8

Calculate Δ_rG° at 298 K using the following information: 2H₂S(g) + 3O₂(g) → 2SO₂(g) + 2H₂O(g) Δ_rG°= ? Δ_fG°(kJ mol^-1) -33.4 -300.1 -228.6

Estimate Δ_rG° for the following reaction at 449.0 K. CH₂O(g) + 2H₂(g) → CH₄(g) + H₂O(g) Δ_rH°= -94.9 kJ mol^-1; Δ_rS°= -224.2 J K^-1 mol^-1

Determine Δ_rG° at 298 K using the following information: H₂(g) + CO(g) → CH₂O(g) Δ_rH°= +1.9 kJ mol^-1; Δ_rS°= -109.6 J K^-1mol^-1

What is the name of the reaction that does NOT achieve the theoretical limits with respect to the change in Gibbs energy in thermodynamics?

What is the name of the reaction that achieves the theoretical limits with respect to the change in Gibbs energy in thermodynamics?

Given the following equation, N₂O(g) + NO₂(g) → 3 NO(g) Δ_rG° = -23.0 kJ mol^-1 Calculate Δ_rG° for the following reaction: 9NO(g) → 3N₂O(g) + 3NO₂(g)

Estimate Δ_rG° for the following reaction at 775 K. 2Hg(g) + O₂(g) → 2HgO(s) Δ_rH°= -304.2 kJ mol^-1; Δ_rS°= -414.2 J K^-1 mol^-1

Identify the compound with the lowest standard Gibbs energy of formation.

Identify the compound with the highest standard Gibbs energy of formation.

Calculate ΔρS° for the following reaction. The S° for each species is shown below the reaction. P₄(g) + 10Cl₂(g) → 4PCl₅(g) S°(J K^-1 mol^-1) 280.0 223.1 364.6

Determine Δ_rG° at 298 K using the following information: FeO(s) + CO(g) → Fe(s) + CO₂(g) Δ_rH°= -11.0 kJ mol^-1; Δ_rS°= -17.4 J K^-1 mol^-1

Quiz 17: Gibbs Energy and Thermodynamics

Calculate ΔrS° for the following reaction. The S∘ for each species is shown below the reaction. C2H2(g) + 2H2(g) → C2H6(g) S°(J K-1 mol-1) 200.9 130.7 229.2

Identify the compound with the standard Gibbs energy of formation equal to zero.

Given the following equation, N2O(g) + NO2(g) → 3NO(g) ΔrG° = -23.0 kJ mol-1 Calculate ΔrG° for the following reaction: 3N2O(g) + 3NO2(g) → 9NO(g)

What is the change in Gibbs energy of a process?

Estimate ΔrG° for the following reaction at 387 K. HCN(g) + 2H2(g) → CH3NH2(g) ΔrH°= -158.0 kJ mol-1; ΔrS°= -219.9 J K-1 mol-1

Determine ΔrG° at 298 K using the following information: CaCO3(s) → CaO(s) + CO2(g) ΔrH°= +179.2 kJ mol-1; ΔrS°= +160.2 J K-1 mol-1

Given the following equation, N2O(g) + NO2(g) → 3NO(g) ΔrG° = -23.0 kJ mol-1 Calculate ΔrGo for the following reaction: 3NO(g) → N2O(g) + NO2(g)

Calculate ΔrS° for the following reaction. The S° for each species is shown below the reaction. N2H4(l) + H2(g) → 2NH3(g) S° (J K-1 mol-1) 121.2 130.7 192.8

Calculate ΔrS° for the following reaction. The S° for each species is shown below the reaction. 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) S°(J K-1 mol-1) 192.8 205.2 210.8 188.8

Calculate ΔrG° at 298 K using the following information: 2H2S(g) + 3O2(g) → 2SO2(g) + 2H2O(g) ΔrG° = ? ΔfG°(kJ mol-1) -33.4 -300.1 -228.6

Estimate ΔrG° for the following reaction at 449.0 K. CH2O(g) + 2H2(g) → CH4(g) + H2O(g) ΔrH°= -94.9 kJ mol-1; ΔrS°= -224.2 J K-1 mol-1

Determine ΔrG° at 298 K using the following information: H2(g) + CO(g) → CH2O(g) ΔrH°= +1.9 kJ mol-1; ΔrS°= -109.6 J K-1 mol-1

What is the name of the reaction that does NOT achieve the theoretical limits with respect to the change in Gibbs energy in thermodynamics?

What is the name of the reaction that achieves the theoretical limits with respect to the change in Gibbs energy in thermodynamics?

Given the following equation, N2O(g) + NO2(g) → 3 NO(g) ΔrG° = -23.0 kJ mol-1 Calculate ΔrG° for the following reaction: 9NO(g) → 3N2O(g) + 3NO2(g)

Estimate ΔrG° for the following reaction at 775 K. 2Hg(g) + O2(g) → 2HgO(s) ΔrH°= -304.2 kJ mol-1; ΔrS°= -414.2 J K-1 mol-1

Identify the compound with the lowest standard Gibbs energy of formation.

Identify the compound with the highest standard Gibbs energy of formation.

Calculate ΔρS° for the following reaction. The S° for each species is shown below the reaction. P4(g) + 10Cl2(g) → 4PCl5(g) S°(J K-1 mol-1) 280.0 223.1 364.6

Determine ΔrG° at 298 K using the following information: FeO(s) + CO(g) → Fe(s) + CO2(g) ΔrH°= -11.0 kJ mol-1; ΔrS°= -17.4 J K-1 mol-1

Calculate Δ_rS° for the following reaction. The S^∘for each species is shown below the reaction. C₂H₂(g) + 2H₂(g) → C₂H₆(g) S°(J K^-1 mol^-1) 200.9 130.7 229.2

Given the following equation, N₂O(g) + NO₂(g) → 3NO(g) Δ_rG° = -23.0 kJ mol^-1 Calculate Δ_rG° for the following reaction: 3N₂O(g) + 3NO₂(g) → 9NO(g)

Estimate Δ_rG° for the following reaction at 387 K. HCN(g) + 2H₂(g) → CH₃NH₂(g) Δ_rH°= -158.0 kJ mol^-1; Δ_rS°= -219.9 J K^-1 mol^-1

Determine Δ_rG° at 298 K using the following information: CaCO₃(s) → CaO(s) + CO₂(g) Δ_rH°= +179.2 kJ mol^-1; Δ_rS°= +160.2 J K^-1 mol^-1

Given the following equation, N₂O(g) + NO₂(g) → 3NO(g) Δ_rG°= -23.0 kJ mol^-1 Calculate Δ_rG^o for the following reaction: 3NO(g) → N₂O(g) + NO₂(g)

Calculate Δ_rS° for the following reaction. The S° for each species is shown below the reaction. N₂H₄(l) + H₂(g) → 2NH₃(g) S° (J K^-1 mol^-1) 121.2 130.7 192.8

Calculate Δ_rS° for the following reaction. The S° for each species is shown below the reaction. 4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(g) S°(J K^-1 mol^-1) 192.8 205.2 210.8 188.8

Calculate Δ_rG° at 298 K using the following information: 2H₂S(g) + 3O₂(g) → 2SO₂(g) + 2H₂O(g) Δ_rG°= ? Δ_fG°(kJ mol^-1) -33.4 -300.1 -228.6

Estimate Δ_rG° for the following reaction at 449.0 K. CH₂O(g) + 2H₂(g) → CH₄(g) + H₂O(g) Δ_rH°= -94.9 kJ mol^-1; Δ_rS°= -224.2 J K^-1 mol^-1

Determine Δ_rG° at 298 K using the following information: H₂(g) + CO(g) → CH₂O(g) Δ_rH°= +1.9 kJ mol^-1; Δ_rS°= -109.6 J K^-1mol^-1

Given the following equation, N₂O(g) + NO₂(g) → 3 NO(g) Δ_rG° = -23.0 kJ mol^-1 Calculate Δ_rG° for the following reaction: 9NO(g) → 3N₂O(g) + 3NO₂(g)

Estimate Δ_rG° for the following reaction at 775 K. 2Hg(g) + O₂(g) → 2HgO(s) Δ_rH°= -304.2 kJ mol^-1; Δ_rS°= -414.2 J K^-1 mol^-1

Calculate ΔρS° for the following reaction. The S° for each species is shown below the reaction. P₄(g) + 10Cl₂(g) → 4PCl₅(g) S°(J K^-1 mol^-1) 280.0 223.1 364.6

Determine Δ_rG° at 298 K using the following information: FeO(s) + CO(g) → Fe(s) + CO₂(g) Δ_rH°= -11.0 kJ mol^-1; Δ_rS°= -17.4 J K^-1 mol^-1