Thermodynamics - Nonstandard Conditions - Gibbs Free Energy - K

The concentration of A is initially 0.150 M before it proceeds to equilibrium. What is the equilibrium concentration of B? A(g) ⇌ B(g) ΔG° = −2.25 kJ A. 0.107 M B. 0.150 M C. 0.043 M

A

What can be said about the relative amounts of reactants and products when K is greater than one? A. There are more products than reactants. B. There are more reactants than products. C. The amounts of reactants and products are approximately the same.

A

What is G when G° is 2.80 kJ and Q equals 8.94 at 25°C? N₂O₄(g) ⇌ 2 NO₂(g) A. 8.23 kJ B. 5.43 kJ C. 3.26 kJ D. −2.63 kJ

A

What is G when G° is −1010. kJ and Q equals 18.97 at 25°C? 4 NH₃(g)+ 5 O₂(g) ⇌ 4 NO(g)+ 6 H₂O(g) A. -1003 kJ B. -1017 kJ C. 6281 kJ D. -1009 kJ

A

What is the change in the free energy, G°, for the reaction? 2 CO(g) + O₂(g) → 2 CO₂(g) Substance | Gf° (kJ/mol) CO(g) | -137.2 CO₂(g) | -394.4 A. 21.0 kJ B. 1.76 kJ C. 9.11 kJ D. 2.1 × 10⁴ kJ

A

What is the change in the free energy, G°, for the reaction? 6 CO₂(g) + 6 H₂O(g) → C₆H₁₂O₆(s) + 6 O₂(g) Substance | Gf° (kJ/mol) CO₂(g) | -394.4 H₂O(g) | -228.6 C₆H₁₂O₆(g) | -910.4 A. 2827.0 kJ B. -287.5 kJ C. -744.7 kJ D. 83.8 kJ

A

What is the equilibrium constant, K, for the following reaction at 25°C? 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) ΔG° = −148.6 kJ A. 1.14 × 10²⁶ B. 1.00 × 10⁶⁰ C. 1.06 D. 1.15

A

What is the equilibrium constant, K, for the following reaction at 25°C? MgCO₃(s) ⇌ MgO(s) + CO₂(g) ΔG° = 48.2 kJ A. 3.56 × 10⁻⁹ B. 3.16 × 10⁻²⁰ C. 0.981 D. 0.956

A

What is ΔG° for the following reaction at 25°C? CoBr₂(g) ⇌ CO(g) + Br₂(g) Kc = 0.19 A. 4.11 kJ B. 0.345 kJ C. 4.11 × 10³ kJ D. 1.79 kJ

A

What is ΔG° for the following reaction at 25°C? NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq) K = 1.8 × 10⁻⁵ A. 27.1 kJ B. 2.27 × 10³ C. 11.8 kJ D. 2.71 × 10⁴ kJ

A

If the equilibrium constant at 298 K is 8.8 at 298 K, at what temperature is the equilibrium constant equal to 2.6? 2 NO₂(g) ⇌ N₂O₄(g) H = −57.2 kJ A. 83.9 K B. 314 K C. 5.66 × 10⁴ K D. −5.75 K

B

The concentration of A is initially 0.100 M before it proceeds to equilibrium. What is the equilibrium concentration of B? A(g) ⇌ B(g) ΔG° = 31.5 kJ A. 0.100 B. 3.05 × 10⁻⁷ C. 3.05 × 10⁻⁵

B

The concentration of A is initially 0.200 M before it proceeds to equilibrium. What is the equilibrium concentration of B? A(g) ⇌ B(g) ΔG° = 17.5 kJ A. 4.28 × 10⁻³ B. 1.71 × 10⁻⁴ M C. 0.200 M

B

The equilibrium concentrations of A and B are 0.0434 M and 0.0923 M, respectively. What is ΔG° at 25°C? A(g) ⇌ 2 B(g) A. −3.59 kJ B. 4.04 kJ C. 3.39 kJ D. −1.87 kJ

B

What can be said about the relative amounts of reactants and products when K is approximately one? A. There are more products than reactants. B. The amount of reactants and products are approximately the same. C. There are more reactants than products.

B

What can be said about the relative amounts of reactants and products when K is less than one? A. The amounts of reactants and products are approximately the same. B. There are more reactants than products. C. There are more products than reactants.

B

What is G when G° is 2827 kJ and the pressure of each gas is 0.0391 atm at 25°C? 6 CO₂(g) + 6 H₂O(g) → C₆H₁₂O₆(s) + 6 O₂(g) A. 2831 kJ B. 2875 kJ C. 2778 kJ D. 52 kJ

B

What is G when G° is −32.96 kJ and Q equals 42.15 at 25°C? N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g) A. −32.18 kJ B. −23.69 kJ C. 9.24 kJ D. −42.23 kJ

B

What is the equilibrium constant, K, for the following reaction at 25°C? HA(aq) → H+(aq) + A−(aq) ΔG° = −317 kJ A. 1.34 B. 3.89 × 10⁵⁵ C. 1.14 D. 8.87 × 10¹²⁷

B

What is the value of G when a system is at equilibrium? A. G > 0 B. G = 0 C. G < 0

B

If the equilibrium constant is 4.9 × 10⁻⁶ at 298 K, at what temperature is the value 9.3 × 10⁻⁵? 2 ICl(g) ⇌ I₂(g) + Cl₂(g) H = 26.9 kJ A. 1.10 K B. 9.51 × 10³ K C. 408 K D. 1.10 × 10³ K

C

If the equilibrium constant is 4.9 × 10⁻⁶ at 298 K, what is the value at 373 K? 2 ICl(g) ⇌ I₂(g) + Cl₂(g) H = 26.9 kJ A. 2.24 × 10⁴ B. 1.99 × 10⁵ C. 4.46 × 10⁻⁵ D. 1.04 × 10⁻⁵³

C

If the equilibrium constant is 8.8 at 298 K, what is the value at 353 K? 2 NO₂(g) ⇌ N₂O₄(g) H = −57.2 kJ A. 4.05 × 10⁻⁴ B. 8.73 C. 0.239 D. 321

C

The equilibrium concentrations of A and B are 0.0354 M and 0.121 M, respectively. What is ΔG° at 25°C? A(g) ⇌ B(g) A. 3.04 kJ B. −0.255 kJ C. −3.04 kJ D. 0.255 kJ

C

What is G when G° is −257.2 kJ and the pressure of each gas is 0.0358 atm at 25°C? CO(g) + ½ O₂(g) ⇌ CO₂(g) A. −261.3 kJ B. 3.87 kJ C. −253.1 kJ D. −256.9 kJ

C

What is the enthalpy of vaporization if K = 3.2 × 10⁻³ at 0°C and 8.1 × 10⁻³ at 50°C? A(g) ⇌ B(g) A. 2.50 kJ/mol B. 7.75 × 10⁻³ kJ/mol C. 13.6 kJ/mol D. 197 kJ/mol

C

What is ΔG° for the following reaction at 25°C? CO(g) + 2 H₂(g) ⇌ CH₃OH(g) K = 2.1 × 10⁻⁴ A. 1.76 kJ B. 9.11 kJ C. 21.0 kJ D. 2.1 × 10⁴ kJ

C

The equilibrium concentrations of A and B are 0.0241 M and 0.0822 M, respectively. What is ΔG° at 25°C? 2 A(g) ⇌ B(g) A. −3.04 kJ B. −1.32 kJ C. −1.03 kJ D. −12.3 kJ

D

What is G when G° is −76.0 kJ and the pressure of each gas is 0.0255 atm at 25°C? 4 HCl(g) + O₂(g) ⇌ H₂O(g) + 2 Cl₂(g) A. −74.5 kJ B. −94.2 kJ C. 18.1 kJ D. −57.8 kJ

D

What is the change in the free energy, G°, for the reaction? 2 CO(g) + O₂(g) → 2 CO₂(g) Substance | Gf° (kJ/mol) CO(g) | -137.2 CO₂(g) | -394.4 A. −257.2 kJ B. −1063.2 kJ C. −531.6 kJ D. −514.4 kJ

D

What is the change in the free energy, G°, for the reaction? 4 KClO₃(s) + 3 H₂S(aq) → 4 KCl(s) + 3 H₂SO₄(aq) Substance | Gf° (kJ/mol) KCLO₃(g) | -296.3 H₂S(g) | -27.7 KCL(g) | -408.5 H₂SO₄(g) | -744.6 A. −829.1 kJ B. −2765.7 kJ C. −2150.7 kJ D. −2599.5 kJ

D