Question 1

K_c is 1.67 × 10²⁰ at 25°C for the formation of iron(III)oxalate complex ion: Fe³⁺(aq)+ 3 C₂O₄^2-(aq)⇌ [Fe(C₂O₄)₃]^3-(aq). If 0.0200 M Fe³⁺ is initially mixed with 1.00 M oxalate ion,what is the concentration of Fe³⁺ ion at equilibrium?

Accepted Answer

The equilibrium constant expression for the formation of the iron(III)oxalate complex ion is:K_c = [Fe(C₂O₄)₃^3-] / [Fe³⁺][C₂O₄^2-]³At equilibrium, the concentration of the complex ion is:[Fe(C₂O₄)₃^3-] = K_c[Fe³⁺][C₂O₄^2-]³Substituting the given values into this equation, we get:1.67 × 10²⁰ = [Fe(C₂O₄)₃^3-] / (0.0200 M)(1.00 M)³Solving for [Fe(C₂O₄)₃^3-], we get:[Fe(C₂O₄)₃^3-] = 1.44 × 10^-22 MTherefore, the concentration of Fe³⁺ ion at equilibrium is:[Fe³⁺] = K_c[Fe(C₂O₄)₃^3-] / [C₂O₄^2-]³Substituting the given values into this equation, we get:[Fe³⁺] = (1.67 × 10²⁰)(1.44 × 10^-22 M) / (1.00 M)³Solving for [Fe³⁺], we get:[Fe³⁺] = 1.44 × 10^-22 MTherefore, the correct answer is A) 1.44 × 10^-22 M.

Question 2

A reaction in which reactants form products in the forward reaction and products simultaneously form reactants in the reverse reaction is said to be ________.

Accepted Answer

The answer of A reaction in which reactants form products...

Question 3

For the reaction CaCO₃(s)⇌ CaO(s)+ O₂(g)the equilibrium expression is K_p = ________.

Accepted Answer

The answer of For the reaction CaCO₃(s)⇌ CaO(s)+ O₂(g)the equilibrium...

Question 4

At 298 K,K_p = 2.1 × 10⁴ for the reaction CO(g)+ 2 H₂(g)⇌ CH₃OH(g).What is the value of K_c at this temperature?

Accepted Answer

The answer of At 298 K,K_p = 2.1 × 10⁴...

Question 5

For the reaction H₂(g)+ S(s)⇌ H₂S(g),if the rate constant for the forward reaction is greater than the rate constant for the reverse reaction,the value of K_c must be ________ (equal to,greater than,less than)1.

Accepted Answer

The answer of For the reaction H₂(g)+ S(s)⇌ H₂S(g),if the...

Question 6

At 1000 K,K_p = 19.9 for the reaction Fe₂O₃(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO₂(g).What is the value of K_p for the reaction 2 Fe(s)+ 3 CO₂(g)⇌ Fe₂O₃(s)+ 3 CO(g)?

Accepted Answer

The answer of At 1000 K,K_p = 19.9 for the...

Question 7

At an elevated temperature,K_p = 0.19 for the reaction 2 NOCl(g)⇌ 2 NO(g)+ Cl₂(g).If the initial partial pressures of NOCl,NO,and Cl₂ are 0.50 atm,0.25 atm,and 0.45 atm,respectively,a net ________ (forward,reverse)reaction must occur in order to achieve equilibrium.

Accepted Answer

The answer of At an elevated temperature,K_p = 0.19 for...

Question 8

K_c = 1.2 × 10^-42at 500 K for the reaction shown below. H₂(g)⇌ 2 H(g) If [H₂] = 1 × 10^-2 M and [H] = 1.2 × 10^-22 M,in order to achieve equilibrium a net reaction must occur from ________ to ________ until Q_c = ________.

Accepted Answer

The answer of K_c = 1.2 × 10^-42at 500...

Question 9

For the reaction shown below the equilibrium constant expression for K_c= ________. HF(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ F^-(aq)

Accepted Answer

The answer of For the reaction shown below the equilibrium...

Question 10

At 1000 K,K_p = 19.9 for the reaction Fe₂O₃(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO₂(g).What is the value of K_p for the reaction 6 Fe(s)+ 9 CO₂(g)⇌ 3 Fe₂O₃(s)+ 9 CO(g)?

Accepted Answer

The answer of At 1000 K,K_p = 19.9 for the...

Question 11

For the reaction A₂ + 2 B₃ ⇌ 2 AB₃,the rate of the forward reaction is 0.25 M/s and the rate of the reverse reaction is 0.75 M/s.The reaction is not at equilibrium.In order to attain equilibrium the reaction must proceed in the ________ (forward,reverse)direction in order to achieve equilibrium.

Accepted Answer

The answer of For the reaction A₂ + 2 B₃...

Question 12

K_c = 57.0at 700 K for the reaction shown below. H₂(g)+ I₂(g)⇌ 2 HI(g) If [H₂(g)] = [I₂(g)] = 0.200 M at equilibrium,the molar concentration [HI((g)] = ________ at equilibrium.

Accepted Answer

The answer of K_c = 57.0at 700 K for...

Question 13

For the reaction shown below,N₂O₄ and NO₂ have equilibrium concentrations,[N₂O₄]_eq = 2.160 × 10^-⁴ and [NO₂]_eq = 1.001 × 10^-³,respectively.The equilibrium constant,K_c,for this reaction equals ________. N₂O₄(g)⇌ 2 NO₂(g)

Accepted Answer

The answer of For the reaction shown below,N₂O₄ and NO₂...

Question 14

At an elevated temperature,K_p = 4.2 × 10^-9 for the reaction 2 HBr(g)⇌ H₂(g)+ Br₂(g).If the initial partial pressures of HBr,H₂,and Br₂ are 1.0 × 10^-2 atm,2.0 × 10^-4 atm,and 2.0 × 10^-4 atm,respectively,what is the equilibrium partial pressure of H₂?

Accepted Answer

The answer of At an elevated temperature,K_p = 4.2 ×...

Question 15

At 298 K,K_c = 1.7 × 10^-56 for the reaction 3 O₂(g)⇌ 2 O₃(g).What is the value of K_p at this temperature?

Accepted Answer

The answer of At 298 K,K_c = 1.7 × 10^-56...

Question 16

For the reaction 2 A + B₂ ⇌ 2 AB,the rate of the forward reaction is 0.75 M/s and the rate of the reverse reaction is 0.25 M/s.The reaction is not at equilibrium.In order to attain equilibrium the reaction must proceed in the ________ (forward,reverse)direction in order to achieve equilibrium.

Accepted Answer

The answer of For the reaction 2 A + B₂...

Question 17

For the reaction shown below the value of K_p is ________ than the value of K_c,because Δn = ________. N₂O₄(g)⇌ 2 NO₂(g)

Accepted Answer

The answer of For the reaction shown below the value...

Question 18

The reaction CaCO₃(s)⇌ CaO(s)+ O₂(g)is endothermic 298 K.The effect of adding additional CaO to the system at equilibrium will ________ (decrease,increase,have no effect on)the total quantity of CaCO₃ once equilibrium is reestablished.

Accepted Answer

The answer of The reaction CaCO₃(s)⇌ CaO(s)+ O₂(g)is endothermic 298...

Question 19

If additional SCN^- is added to the equilibrium system shown below,Le Châtelier's principle predicts a net reaction from ________ to ________,causing the red color to become ________. Fe³⁺(aq)+ SCN^-(aq)⇌ FeSCN²⁺(aq) yellow colorless red

Accepted Answer

The answer of If additional SCN^- is added to the...

Question 20

In a reversible reaction,when the rate of the forward reaction equals the rate of the reverse reaction,the reaction is at ________.

Accepted Answer

The answer of In a reversible reaction,when the rate of...

Quiz 13: Chemical Equilibrium

K_c is 1.67 × 10²⁰ at 25°C for the formation of iron(III) oxalate complex ion: Fe³⁺(aq) + 3 C₂O₄^2-(aq) ⇌ [Fe(C₂O₄) ₃]^3-(aq) . If 0.0200 M Fe³⁺ is initially mixed with 1.00 M oxalate ion,what is the concentration of Fe³⁺ ion at equilibrium?

A reaction in which reactants form products in the forward reaction and products simultaneously form reactants in the reverse reaction is said to be ________.

For the reaction CaCO₃(s)⇌ CaO(s)+ O₂(g)the equilibrium expression is K_p = ________.

At 298 K,K_p = 2.1 × 10⁴ for the reaction CO(g)+ 2 H₂(g)⇌ CH₃OH(g).What is the value of K_c at this temperature?

For the reaction H₂(g)+ S(s)⇌ H₂S(g),if the rate constant for the forward reaction is greater than the rate constant for the reverse reaction,the value of K_c must be ________ (equal to,greater than,less than)1.

At 1000 K,K_p = 19.9 for the reaction Fe₂O₃(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO₂(g).What is the value of K_p for the reaction 2 Fe(s)+ 3 CO₂(g)⇌ Fe₂O₃(s)+ 3 CO(g)?

At an elevated temperature,K_p = 0.19 for the reaction 2 NOCl(g)⇌ 2 NO(g)+ Cl₂(g).If the initial partial pressures of NOCl,NO,and Cl₂ are 0.50 atm,0.25 atm,and 0.45 atm,respectively,a net ________ (forward,reverse)reaction must occur in order to achieve equilibrium.

K_c = 1.2 × 10^-42at 500 K for the reaction shown below. H₂(g)⇌ 2 H(g) If [H₂] = 1 × 10^-2 M and [H] = 1.2 × 10^-22 M,in order to achieve equilibrium a net reaction must occur from to until Q_c = ________.

For the reaction shown below the equilibrium constant expression for K_c= ________. HF(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ F^-(aq)

At 1000 K,K_p = 19.9 for the reaction Fe₂O₃(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO₂(g).What is the value of K_p for the reaction 6 Fe(s)+ 9 CO₂(g)⇌ 3 Fe₂O₃(s)+ 9 CO(g)?

K_c = 57.0at 700 K for the reaction shown below. H₂(g)+ I₂(g)⇌ 2 HI(g) If [H₂(g)] = [I₂(g)] = 0.200 M at equilibrium,the molar concentration [HI((g)] = ________ at equilibrium.

For the reaction shown below,N₂O₄ and NO₂ have equilibrium concentrations,[N₂O₄]_eq = 2.160 × 10^-⁴ and [NO₂]_eq = 1.001 × 10^-³,respectively.The equilibrium constant,K_c,for this reaction equals ________. N₂O₄(g)⇌ 2 NO₂(g)

At an elevated temperature,K_p = 4.2 × 10^-9 for the reaction 2 HBr(g)⇌ H₂(g)+ Br₂(g).If the initial partial pressures of HBr,H₂,and Br₂ are 1.0 × 10^-2 atm,2.0 × 10^-4 atm,and 2.0 × 10^-4 atm,respectively,what is the equilibrium partial pressure of H₂?

At 298 K,K_c = 1.7 × 10^-56 for the reaction 3 O₂(g)⇌ 2 O₃(g).What is the value of K_p at this temperature?

For the reaction 2 A + B₂ ⇌ 2 AB,the rate of the forward reaction is 0.75 M/s and the rate of the reverse reaction is 0.25 M/s.The reaction is not at equilibrium.In order to attain equilibrium the reaction must proceed in the ________ (forward,reverse)direction in order to achieve equilibrium.

For the reaction shown below the value of K_p is ________ than the value of K_c,because Δn = ________. N₂O₄(g)⇌ 2 NO₂(g)

The reaction CaCO₃(s)⇌ CaO(s)+ O₂(g)is endothermic 298 K.The effect of adding additional CaO to the system at equilibrium will ________ (decrease,increase,have no effect on)the total quantity of CaCO₃ once equilibrium is reestablished.

If additional SCN^- is added to the equilibrium system shown below,Le Châtelier's principle predicts a net reaction from to ,causing the red color to become . Fe³⁺(aq)+ SCN^-(aq)⇌ FeSCN²⁺(aq) yellow colorless red

In a reversible reaction,when the rate of the forward reaction equals the rate of the reverse reaction,the reaction is at ________.

Quiz 13: Chemical Equilibrium

Kc is 1.67 × 1020 at 25°C for the formation of iron(III) oxalate complex ion: Fe3+(aq) + 3 C2O42-(aq) ⇌ [Fe(C2O4) 3]3-(aq) . If 0.0200 M Fe3+ is initially mixed with 1.00 M oxalate ion,what is the concentration of Fe3+ ion at equilibrium?

A reaction in which reactants form products in the forward reaction and products simultaneously form reactants in the reverse reaction is said to be ________.

For the reaction CaCO3(s)⇌ CaO(s)+ O2(g)the equilibrium expression is Kp = ________.

At 298 K,Kp = 2.1 × 104 for the reaction CO(g)+ 2 H2(g)⇌ CH3OH(g).What is the value of Kc at this temperature?

For the reaction H2(g)+ S(s)⇌ H2S(g),if the rate constant for the forward reaction is greater than the rate constant for the reverse reaction,the value of Kc must be ________ (equal to,greater than,less than)1.

At 1000 K,Kp = 19.9 for the reaction Fe2O3(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO2(g).What is the value of Kp for the reaction 2 Fe(s)+ 3 CO2(g)⇌ Fe2O3(s)+ 3 CO(g)?

At an elevated temperature,Kp = 0.19 for the reaction 2 NOCl(g)⇌ 2 NO(g)+ Cl2(g).If the initial partial pressures of NOCl,NO,and Cl2 are 0.50 atm,0.25 atm,and 0.45 atm,respectively,a net ________ (forward,reverse)reaction must occur in order to achieve equilibrium.

Kc = 1.2 × 10-42 at 500 K for the reaction shown below. H2(g)⇌ 2 H(g) If [H2] = 1 × 10-2 M and [H] = 1.2 × 10-22 M,in order to achieve equilibrium a net reaction must occur from ________ to ________ until Qc = ________.

For the reaction shown below the equilibrium constant expression for Kc = ________. HF(aq)+ H2O(l)⇌ H3O+(aq)+ F-(aq)

At 1000 K,Kp = 19.9 for the reaction Fe2O3(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO2(g).What is the value of Kp for the reaction 6 Fe(s)+ 9 CO2(g)⇌ 3 Fe2O3(s)+ 9 CO(g)?

For the reaction A2 + 2 B3 ⇌ 2 AB3,the rate of the forward reaction is 0.25 M/s and the rate of the reverse reaction is 0.75 M/s.The reaction is not at equilibrium.In order to attain equilibrium the reaction must proceed in the ________ (forward,reverse)direction in order to achieve equilibrium.

Kc = 57.0 at 700 K for the reaction shown below. H2(g)+ I2(g)⇌ 2 HI(g) If [H2(g)] = [I2(g)] = 0.200 M at equilibrium,the molar concentration [HI((g)] = ________ at equilibrium.

For the reaction shown below,N2O4 and NO2 have equilibrium concentrations,[N2O4]eq = 2.160 × 10-4 and [NO2]eq = 1.001 × 10-3,respectively.The equilibrium constant,Kc,for this reaction equals ________. N2O4(g)⇌ 2 NO2(g)

At an elevated temperature,Kp = 4.2 × 10-9 for the reaction 2 HBr(g)⇌ H2(g)+ Br2(g).If the initial partial pressures of HBr,H2,and Br2 are 1.0 × 10-2 atm,2.0 × 10-4 atm,and 2.0 × 10-4 atm,respectively,what is the equilibrium partial pressure of H2?

At 298 K,Kc = 1.7 × 10-56 for the reaction 3 O2(g)⇌ 2 O3(g).What is the value of Kp at this temperature?

For the reaction 2 A + B2 ⇌ 2 AB,the rate of the forward reaction is 0.75 M/s and the rate of the reverse reaction is 0.25 M/s.The reaction is not at equilibrium.In order to attain equilibrium the reaction must proceed in the ________ (forward,reverse)direction in order to achieve equilibrium.

For the reaction shown below the value of Kp is ________ than the value of Kc,because Δn = ________. N2O4(g)⇌ 2 NO2(g)

The reaction CaCO3(s)⇌ CaO(s)+ O2(g)is endothermic 298 K.The effect of adding additional CaO to the system at equilibrium will ________ (decrease,increase,have no effect on)the total quantity of CaCO3 once equilibrium is reestablished.

If additional SCN- is added to the equilibrium system shown below,Le Châtelier's principle predicts a net reaction from ________ to ________,causing the red color to become ________. Fe3+(aq)+ SCN-(aq)⇌ FeSCN2+(aq) yellow colorless red

In a reversible reaction,when the rate of the forward reaction equals the rate of the reverse reaction,the reaction is at ________.

K_c is 1.67 × 10²⁰ at 25°C for the formation of iron(III) oxalate complex ion: Fe³⁺(aq) + 3 C₂O₄^2-(aq) ⇌ [Fe(C₂O₄) ₃]^3-(aq) . If 0.0200 M Fe³⁺ is initially mixed with 1.00 M oxalate ion,what is the concentration of Fe³⁺ ion at equilibrium?

For the reaction CaCO₃(s)⇌ CaO(s)+ O₂(g)the equilibrium expression is K_p = ________.

At 298 K,K_p = 2.1 × 10⁴ for the reaction CO(g)+ 2 H₂(g)⇌ CH₃OH(g).What is the value of K_c at this temperature?

For the reaction H₂(g)+ S(s)⇌ H₂S(g),if the rate constant for the forward reaction is greater than the rate constant for the reverse reaction,the value of K_c must be ________ (equal to,greater than,less than)1.

At 1000 K,K_p = 19.9 for the reaction Fe₂O₃(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO₂(g).What is the value of K_p for the reaction 2 Fe(s)+ 3 CO₂(g)⇌ Fe₂O₃(s)+ 3 CO(g)?

At an elevated temperature,K_p = 0.19 for the reaction 2 NOCl(g)⇌ 2 NO(g)+ Cl₂(g).If the initial partial pressures of NOCl,NO,and Cl₂ are 0.50 atm,0.25 atm,and 0.45 atm,respectively,a net ________ (forward,reverse)reaction must occur in order to achieve equilibrium.

K_c = 1.2 × 10^-42at 500 K for the reaction shown below. H₂(g)⇌ 2 H(g) If [H₂] = 1 × 10^-2 M and [H] = 1.2 × 10^-22 M,in order to achieve equilibrium a net reaction must occur from to until Q_c = ________.

For the reaction shown below the equilibrium constant expression for K_c= ________. HF(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ F^-(aq)

At 1000 K,K_p = 19.9 for the reaction Fe₂O₃(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO₂(g).What is the value of K_p for the reaction 6 Fe(s)+ 9 CO₂(g)⇌ 3 Fe₂O₃(s)+ 9 CO(g)?

K_c = 57.0at 700 K for the reaction shown below. H₂(g)+ I₂(g)⇌ 2 HI(g) If [H₂(g)] = [I₂(g)] = 0.200 M at equilibrium,the molar concentration [HI((g)] = ________ at equilibrium.

For the reaction shown below,N₂O₄ and NO₂ have equilibrium concentrations,[N₂O₄]_eq = 2.160 × 10^-⁴ and [NO₂]_eq = 1.001 × 10^-³,respectively.The equilibrium constant,K_c,for this reaction equals ________. N₂O₄(g)⇌ 2 NO₂(g)

At an elevated temperature,K_p = 4.2 × 10^-9 for the reaction 2 HBr(g)⇌ H₂(g)+ Br₂(g).If the initial partial pressures of HBr,H₂,and Br₂ are 1.0 × 10^-2 atm,2.0 × 10^-4 atm,and 2.0 × 10^-4 atm,respectively,what is the equilibrium partial pressure of H₂?

At 298 K,K_c = 1.7 × 10^-56 for the reaction 3 O₂(g)⇌ 2 O₃(g).What is the value of K_p at this temperature?

For the reaction 2 A + B₂ ⇌ 2 AB,the rate of the forward reaction is 0.75 M/s and the rate of the reverse reaction is 0.25 M/s.The reaction is not at equilibrium.In order to attain equilibrium the reaction must proceed in the ________ (forward,reverse)direction in order to achieve equilibrium.

For the reaction shown below the value of K_p is ________ than the value of K_c,because Δn = ________. N₂O₄(g)⇌ 2 NO₂(g)

The reaction CaCO₃(s)⇌ CaO(s)+ O₂(g)is endothermic 298 K.The effect of adding additional CaO to the system at equilibrium will ________ (decrease,increase,have no effect on)the total quantity of CaCO₃ once equilibrium is reestablished.

If additional SCN^- is added to the equilibrium system shown below,Le Châtelier's principle predicts a net reaction from to ,causing the red color to become . Fe³⁺(aq)+ SCN^-(aq)⇌ FeSCN²⁺(aq) yellow colorless red