The following pictures represent the equilibrium state for four different reactions of the type AS1U1B12S1U1B0 + XS1U1B12S1U1B0 ⇌ 2 AX (X = B,C,D,E).A atoms are unshaded.X atoms are shaded. -Which reaction has the smallest equilibrium constant?

A) A2 + B2 ⇌ 2 AB B) A2 + C2 ⇌ 2 AC C) A2 + D2 ⇌ 2 AD D) A2 + E2 ⇌ 2 AE A) A2 + B2 ⇌ 2 AB B) A2 + C2 ⇌ 2 AC C) A2 + D2 ⇌ 2 AD D) A2 + E2 ⇌ 2 AE

Write the equilibrium equation for the reverse reaction: 2 CH4 (g)+ 3 O2 (g)⇌ 2 CO (g)+ 4 H2O (g)

A) Kc´ = B) Kc´ = C) Kc´ = D) Kc´ = A) Kc´ = B) Kc´ = C) Kc´ = D) Kc´ =

The equilibrium constant Kc for the reaction HF(aq)+ H2O(l)⇌ H3O+(aq)+F-(aq)is 3.5 × 10-4.What is the equilibrium concentration of H3O+ if the initial concentration of HF is 1.0 M?

A) 1)0 M B) 3)5 × 10-2 M C) 1)9 × 10-2 M D) 1)9 × 10-4 M A) 1)0 M B) 3)5 × 10-2 M C) 1)9 × 10-2 M D) 1)9 × 10-4 M

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) 1)44 × 10-22 M B) 0)0100 M C) 8)35 × 1019 M D) 6)94 × 1021 M A) 1)44 × 10-22 M B) 0)0100 M C) 8)35 × 1019 M D) 6)94 × 1021 M

The pink and blue species below form a violet colored mixture at equilibrium: [Co(H2O)6]2+ (aq)+ 4 Cl- (aq)⇌ [CoCl4]2- (aq)+ 6 H2O (l) (pink)(blue) If the concentration of [Co(H2O)6]2+ is increased,what happens to the solution?

A) The concentration of [CoCl4]2- increases. B) The concentration of [CoCl4]2- decreases. C) The solution becomes colorless. D) No color change is observed. A) The concentration of [CoCl4]2- increases. B) The concentration of [CoCl4]2- decreases. C) The solution becomes colorless. D) No color change is observed.

If Kc = 2.0 x 1033 at 25°C,for the following reaction: H2(g)+ Cl2(g)⇌ 2 HCl(g),then find Kp at the same temperature.

A) 8)2 × 1031 B) 9)7 × 1032 C) 2)0 × 1033 D) 4)9 × 1034 A) 8)2 × 1031 B) 9)7 × 1032 C) 2)0 × 1033 D) 4)9 × 1034

At a certain temperature,Kc equals 1.4 × 102 for the reaction: 2 CO(g)+ O2(g)⇌ 2 CO2(g). If a 2.50-L flask contains 0.400 mol of CO2 and 0.100 mol of O2 at equilibrium,how many moles of CO are also present in the flask?

A) 0)422 mol B) 0)169 mol C) 0)107 mol D) 0)0114 mol A) 0)422 mol B) 0)169 mol C) 0)107 mol D) 0)0114 mol

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the reaction: PCl5(g)⇌ PCl3(g)+ Cl2(g) At 250°C,0.250 M PCl5 is added to a flask.If Kc = 1.80,what are the equilibrium concentrations of each gas?

A) [PCl5] = 0.0280 M,[PCl3] = 0.222 M,[Cl2] = 0.222 M B) [PCl5] = 1.25 M,[PCl3] = 0.474 M,[Cl2] = 0.474 M C) [PCl5] = 1.80 M,[PCl3] = 1.80 M,[Cl2] = 1.80 M D) [PCl5] = 2.27 M,[PCl3] = 2.02 M,[Cl2] = 2.02 M A) [PCl5] = 0.0280 M,[PCl3] = 0.222 M,[Cl2] = 0.222 M B) [PCl5] = 1.25 M,[PCl3] = 0.474 M,[Cl2] = 0.474 M C) [PCl5] = 1.80 M,[PCl3] = 1.80 M,[Cl2] = 1.80 M D) [PCl5] = 2.27 M,[PCl3] = 2.02 M,[Cl2] = 2.02 M

Write the equilibrium equation for the reverse reaction: 2 CH4(g)+ 3 O2(g)⇌ 2 CO(g)+ 4 H2O(g)

A) Kp' = B) Kp' = C) Kp' = D) Kp' = A) Kp' = B) Kp' = C) Kp' = D) Kp' =

Exam 13: Chemical Equilibrium

The following pictures represent the equilibrium state for four different reactions of the type A₂ + X₂ ⇌ 2 AX (X = B,C,D,E).A atoms are unshaded.X atoms are shaded. -Which reaction has the smallest equilibrium constant?

(Multiple Choice)

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Question 81

Write the equilibrium equation for the reverse reaction: 2 CH₄ (g)+ 3 O₂ (g)⇌ 2 CO (g)+ 4 H₂O (g)

(Multiple Choice)

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Question 82

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.

(Short Answer)

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Question 83

The following pictures represent the initial state and the equilibrium state for the gaseous state reaction of A₂ molecules (shaded spheres)with B atoms (unshaded spheres)to give AB molecules. -If the volume of the equilibrium mixture is decreased,what will happen to the number of AB molecules and the number of B atoms?

(Multiple Choice)

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Question 84

If K_c is the equilibrium constant for a forward reaction,2 A⇌ B,what is K_c´ for the reaction 4 A⇌ 2B?

(Multiple Choice)

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Question 85

Which statement is true for a reaction with K_c equal to 2.43 × 10^-12?

(Multiple Choice)

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Question 86

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

(Short Answer)

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Question 87

The equilibrium constant K_cfor the reaction HF(aq)+ H₂O(l)⇌ H₃O⁺(aq)+F^-(aq)is 3.5 × 10^-4.What is the equilibrium concentration of H₃O⁺ if the initial concentration of HF is 1.0 M?

(Multiple Choice)

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Question 88

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?

(Multiple Choice)

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Question 89

The pink and blue species below form a violet colored mixture at equilibrium: [Co(H₂O)₆]²⁺ (aq)+ 4 Cl^- (aq)⇌ [CoCl₄]^2- (aq)+ 6 H₂O (l) (pink)(blue) If the concentration of [Co(H₂O)₆]²⁺ is increased,what happens to the solution?

(Multiple Choice)

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Question 90

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

(Short Answer)

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Question 91

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)

(Short Answer)

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Question 92

If K_c = 2.0 x 10³³ at 25°C,for the following reaction: H₂(g)+ Cl₂(g)⇌ 2 HCl(g),then find K_p at the same temperature.

(Multiple Choice)

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Question 93

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

(Short Answer)

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Question 94

At a certain temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g)+ O₂(g)⇌ 2 CO₂(g). If a 2.50-L flask contains 0.400 mol of CO₂ and 0.100 mol of O₂ at equilibrium,how many moles of CO are also present in the flask?

(Multiple Choice)

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Question 95

Which equilibrium below is homogeneous?

(Multiple Choice)

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Question 96

A reaction reaches dynamic equilibrium at a given temperature when

(Multiple Choice)

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Question 97

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the reaction: PCl₅(g)⇌ PCl₃(g)+ Cl₂(g) At 250°C,0.250 M PCl₅ is added to a flask.If K_c = 1.80,what are the equilibrium concentrations of each gas?

(Multiple Choice)

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Question 98

Write the equilibrium equation for the reverse reaction: 2 CH₄(g)+ 3 O₂(g)⇌ 2 CO(g)+ 4 H₂O(g)

(Multiple Choice)

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Question 99

Given the reaction: 2 HI ⇌ H₂ + I₂.If K_c^' for the reverse reaction is 1.85 × 10^-2 at 425°C,what is K_c for the forward reaction at the same temperature?

(Multiple Choice)

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Question 100

Showing 81 - 100 of 166

Exam 13: Chemical Equilibrium

The following pictures represent the equilibrium state for four different reactions of the type A2 + X2 ⇌ 2 AX (X = B,C,D,E).A atoms are unshaded.X atoms are shaded. -Which reaction has the smallest equilibrium constant?

Write the equilibrium equation for the reverse reaction: 2 CH4 (g)+ 3 O2 (g)⇌ 2 CO (g)+ 4 H2O (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 Kc is the equilibrium constant for a forward reaction,2 A⇌ B,what is Kc´ for the reaction 4 A⇌ 2B?

Which statement is true for a reaction with Kc equal to 2.43 × 10-12?

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

The equilibrium constant Kc for the reaction HF(aq)+ H2O(l)⇌ H3O+(aq)+F-(aq)is 3.5 × 10-4.What is the equilibrium concentration of H3O+ if the initial concentration of HF is 1.0 M?

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?

The pink and blue species below form a violet colored mixture at equilibrium: [Co(H2O)6]2+ (aq)+ 4 Cl- (aq)⇌ [CoCl4]2- (aq)+ 6 H2O (l) (pink)(blue) If the concentration of [Co(H2O)6]2+ is increased,what happens to the solution?

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

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)

If Kc = 2.0 x 1033 at 25°C,for the following reaction: H2(g)+ Cl2(g)⇌ 2 HCl(g),then find Kp at the same temperature.

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

At a certain temperature,Kc equals 1.4 × 102 for the reaction: 2 CO(g)+ O2(g)⇌ 2 CO2(g). If a 2.50-L flask contains 0.400 mol of CO2 and 0.100 mol of O2 at equilibrium,how many moles of CO are also present in the flask?

Which equilibrium below is homogeneous?

A reaction reaches dynamic equilibrium at a given temperature when

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the reaction: PCl5(g)⇌ PCl3(g)+ Cl2(g) At 250°C,0.250 M PCl5 is added to a flask.If Kc = 1.80,what are the equilibrium concentrations of each gas?

Write the equilibrium equation for the reverse reaction: 2 CH4(g)+ 3 O2(g)⇌ 2 CO(g)+ 4 H2O(g)

Given the reaction: 2 HI ⇌ H2 + I2.If Kc' for the reverse reaction is 1.85 × 10-2 at 425°C,what is Kc for the forward reaction at the same temperature?

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The following pictures represent the equilibrium state for four different reactions of the type A₂ + X₂ ⇌ 2 AX (X = B,C,D,E).A atoms are unshaded.X atoms are shaded. -Which reaction has the smallest equilibrium constant?

Write the equilibrium equation for the reverse reaction: 2 CH₄ (g)+ 3 O₂ (g)⇌ 2 CO (g)+ 4 H₂O (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 K_c is the equilibrium constant for a forward reaction,2 A⇌ B,what is K_c´ for the reaction 4 A⇌ 2B?

Which statement is true for a reaction with K_c equal to 2.43 × 10^-12?

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 equilibrium constant K_cfor the reaction HF(aq)+ H₂O(l)⇌ H₃O⁺(aq)+F^-(aq)is 3.5 × 10^-4.What is the equilibrium concentration of H₃O⁺ if the initial concentration of HF is 1.0 M?

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?

The pink and blue species below form a violet colored mixture at equilibrium: [Co(H₂O)₆]²⁺ (aq)+ 4 Cl^- (aq)⇌ [CoCl₄]^2- (aq)+ 6 H₂O (l) (pink)(blue) If the concentration of [Co(H₂O)₆]²⁺ is increased,what happens to the solution?

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

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)

If K_c = 2.0 x 10³³ at 25°C,for the following reaction: H₂(g)+ Cl₂(g)⇌ 2 HCl(g),then find K_p at the same temperature.

At a certain temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g)+ O₂(g)⇌ 2 CO₂(g). If a 2.50-L flask contains 0.400 mol of CO₂ and 0.100 mol of O₂ at equilibrium,how many moles of CO are also present in the flask?

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the reaction: PCl₅(g)⇌ PCl₃(g)+ Cl₂(g) At 250°C,0.250 M PCl₅ is added to a flask.If K_c = 1.80,what are the equilibrium concentrations of each gas?

Write the equilibrium equation for the reverse reaction: 2 CH₄(g)+ 3 O₂(g)⇌ 2 CO(g)+ 4 H₂O(g)

Given the reaction: 2 HI ⇌ H₂ + I₂.If K_c^' for the reverse reaction is 1.85 × 10^-2 at 425°C,what is K_c for the forward reaction at the same temperature?