What is the equilibrium equation for the following reaction? FeS(s)+ 2 H3O+ (aq)⇌ Fe2+(aq)+ H2S (aq)+ 2 H2O (l)

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

Nitric oxide reacts with oxygen to form nitrogen dioxide: 2 NO(g)+ O2(g)⇌ 2 NO2(g) What is Kc for the forward reaction if the equilibrium concentration of NO is 0.200 M,O2 is 0.100 M,and NO2 is 0.250 M at 25°C?

A) 8)00 × 10-2 B) 6)41 × 10-2 C) 12.5 D) 15.6 A) 8)00 × 10-2 B) 6)41 × 10-2 C) 12.5 D) 15.6

An equilibrium mixture of CO,O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0100 M O2.At this temperature,Kc equals 1.4 × 102 for the reaction: 2 CO(g)+ O2(g)⇌ 2 CO2(g). What is the equilibrium concentration of CO?

A) 7)1 × 10- 7 M B) 8)4 × 10- 4 M C) 1)4 × 10-2 M D) 1)2 × 10-1 M A) 7)1 × 10- 7 M B) 8)4 × 10- 4 M C) 1)4 × 10-2 M D) 1)2 × 10-1 M

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl5(g)⇌ PCl3(g)+ Cl2(g) At 250° 0.125 M PCl5 is added to the flask.If Kc = 1.80,what are the equilibrium concentrations of each gas?

A) [PCl5] = 0.0 0765 M,[PCl3] = 0.117 M,and [Cl2] = 0.117 M B) [PCl5] = 0.0625 M,[PCl3] = 0.335 M,and [Cl2] = 0.335 M C) [PCl5] = 1.80 M,[PCl3] = 1.80 M,and [Cl2] = 1.80 M D) [PCl5] = 3.96 M,[PCl3] = 3.83 M,and [Cl2] = 3.83 M A) [PCl5] = 0.0 0765 M,[PCl3] = 0.117 M,and [Cl2] = 0.117 M B) [PCl5] = 0.0625 M,[PCl3] = 0.335 M,and [Cl2] = 0.335 M C) [PCl5] = 1.80 M,[PCl3] = 1.80 M,and [Cl2] = 1.80 M D) [PCl5] = 3.96 M,[PCl3] = 3.83 M,and [Cl2] = 3.83 M

Oxalic acid can donate two protons to water in successive reactions: (1)H2C2O4(aq)+ H2O(l)⇌ H3O+(aq)+ HC2O4-(aq) (2)HC2O4-(aq)+ H2O(l)⇌ H3O+(aq)+ C2O42-(aq) If Kc1 = 5.9 × 10-2 and Kc2 = 6.4 × 10-5 at 25°C,what is the value of Kc for reaction (3)? (3)H2C2O4(aq)+ 2 H2O(l)⇌ 2 H3O+(aq)+ C2O42-(aq)

A) 3)8 × 10-6 B) 1)1 × 10-3 C) 5)9 × 10-2 D) 9)2 × 102 A) 3)8 × 10-6 B) 1)1 × 10-3 C) 5)9 × 10-2 D) 9)2 × 102

The reaction below virtually goes to completion because cyanide ion forms very stable complexes with Ni2+ ion: [Ni(H2O)6]2+(aq)+ 4 CN-(aq)→ [Ni(CN)4]2-(aq)+ 6 H2O(l) At the same time,incorporation of 14C labelled cyanide ion (14CN-)is very rapid: [Ni(CN)4]2-(aq)+ 4 14CN-(aq)= [Ni(14CN)4]2-(aq)+ 4 CN-(aq) Which statement below is correct with regard to stability and rate of reaction?

A) Equilibrium is static. B) Stable species can react rapidly. C) Stable species do not react rapidly. D) Unstable species react rapidly. A) Equilibrium is static. B) Stable species can react rapidly. C) Stable species do not react rapidly. D) Unstable species react rapidly.

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 largest 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

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO2(g)+ O2(g)⇌ 2 SO3(g). If initial concentrations are [SO2] = 6.00 M,[O2] = 0.45 M,and [SO3] = 9.00 M,the system is

A) at equilibrium. B) not at equilibrium and will remain in an unequilibrated state. C) not at equilibrium and will shift to the left to achieve an equilibrium state. D) not at equilibrium and will shift to the right to achieve an equilibrium state. A) at equilibrium. B) not at equilibrium and will remain in an unequilibrated state. C) not at equilibrium and will shift to the left to achieve an equilibrium state. D) not at equilibrium and will shift to the right to achieve an equilibrium state.

Exam 13: Chemical Equilibrium

What is the equilibrium constant,K_c,for the reaction: 2 Hg(l)+ O₂(g)⇌ 2 HgO(s) If the amounts of reactants and products at equilibrium are: 1.00 g of HgO(s),2.00 mL of Hg(l),and 1.60 M O₂(g)? (The molar mass and density of HgO(s)is 217 g/mol,and 1.10 g/cm³.The molar mass and density of Hg(l)is 201 g/mol,and 13.6 g/mL. )

(Multiple Choice)

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Question 101

If K_c = 0.900,and K_p = 538 for a hypothetical reaction,which of the equations below could represent the reaction at 25°C?

(Multiple Choice)

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Question 102

What is the equilibrium equation for the following reaction? FeS(s)+ 2 H₃O⁺ (aq)⇌ Fe²⁺(aq)+ H₂S (aq)+ 2 H₂O (l)

(Multiple Choice)

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Question 103

Shown below is a concentration vs.time plot for the reaction A ⇌ 2B.For this reaction the value of the equilibrium constant is

(Multiple Choice)

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Question 104

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

(Short Answer)

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Question 105

Gaseous hydrogen bromide decomposes at elevated temperatures according to the following equation: 2 HBr(g)⇌ H₂(g)+ Br₂(g). At a certain temperature a 2.00 L flask is initially filled only with 0.600 mol of HBr.What is the value of K_c at that temperature if the flask contains 0.104 mol of H₂ at equilibrium?

(Multiple Choice)

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Question 106

Nitric oxide reacts with oxygen to form nitrogen dioxide: 2 NO(g)+ O₂(g)⇌ 2 NO₂(g) What is K_c for the forward reaction if the equilibrium concentration of NO is 0.200 M,O₂ is 0.100 M,and NO₂ is 0.250 M at 25°C?

(Multiple Choice)

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Question 107

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

(Short Answer)

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Question 108

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0100 M O₂.At this temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g)+ O₂(g)⇌ 2 CO₂(g). What is the equilibrium concentration of CO?

(Multiple Choice)

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Question 109

The following pictures represent mixtures of cis-C₂H₂X₂ molecules and trans-C₂H₂X₂molecules,which interconvert according to the equation cis-C₂H₂X₂ ⇌ trans-C₂H₂X₂.If mixture (1)is at equilibrium,which of the other mixtures are also at equilibrium?

(Multiple Choice)

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Question 110

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl₅(g)⇌ PCl₃(g)+ Cl₂(g) At 250° 0.125 M PCl₅ is added to the flask.If K_c = 1.80,what are the equilibrium concentrations of each gas?

(Multiple Choice)

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Question 111

The esterification of acetic acid and ethanol is given by the reaction below: C₂H₅OH(aq)+ CH₃COOH(aq)⇌ CH₃COOC₂H₅(aq)+ H₂O(l) When 1.00 mol of ethanol was mixed with 2.00 mol of acid in a 1.00 L flask,0.86 mol of ester was formed at room temperature.What is the value of the equilibrium constant,K_c?

(Multiple Choice)

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Question 112

Shown below is a concentration vs.time plot for the reaction A ⇌ 2B.For this reaction the value of the equilibrium constant is

(Multiple Choice)

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Question 113

What is the equilibrium equation for the dissociation of formic acid in water? HCOOH (aq)+ H₂O (l)⇌ H₃O⁺ (aq)+ HCOO^- (aq)

(Multiple Choice)

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Question 114

The reaction CaCO₃(s)⇌ CaO(s)+ O₂(g)is endothermic 298 K.The effect of adding a catalyst 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 115

Oxalic acid can donate two protons to water in successive reactions: (1)H₂C₂O₄(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ HC₂O₄^-(aq) (2)HC₂O₄^-(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ C₂O₄^2-(aq) If K_c1 = 5.9 × 10^-2 and K_c2 = 6.4 × 10^-5 at 25°C,what is the value of K_c for reaction (3)? (3)H₂C₂O₄(aq)+ 2 H₂O(l)⇌ 2 H₃O⁺(aq)+ C₂O₄^2-(aq)

(Multiple Choice)

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Question 116

The reaction below virtually goes to completion because cyanide ion forms very stable complexes with Ni²⁺ ion: [Ni(H₂O)₆]²⁺(aq)+ 4 CN^-(aq)→ [Ni(CN)₄]^2-(aq)+ 6 H₂O(l) At the same time,incorporation of ¹⁴C labelled cyanide ion (¹⁴CN^-)is very rapid: [Ni(CN)₄]^2-(aq)+ 4 ¹⁴CN^-(aq)= [Ni(¹⁴CN)₄]^2-(aq)+ 4 CN^-(aq) Which statement below is correct with regard to stability and rate of reaction?

(Multiple Choice)

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Question 117

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 largest equilibrium constant?

(Multiple Choice)

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Question 118

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g). If initial concentrations are [SO₂] = 6.00 M,[O₂] = 0.45 M,and [SO₃] = 9.00 M,the system is

(Multiple Choice)

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Question 119

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.

(Short Answer)

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Question 120

Showing 101 - 120 of 166

If K_c = 0.900,and K_p = 538 for a hypothetical reaction,which of the equations below could represent the reaction at 25°C?

What is the equilibrium equation for the following reaction? FeS(s)+ 2 H₃O⁺ (aq)⇌ Fe²⁺(aq)+ H₂S (aq)+ 2 H₂O (l)

Shown below is a concentration vs.time plot for the reaction A ⇌ 2B.For this reaction the value of the equilibrium constant is

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

Nitric oxide reacts with oxygen to form nitrogen dioxide: 2 NO(g)+ O₂(g)⇌ 2 NO₂(g) What is K_c for the forward reaction if the equilibrium concentration of NO is 0.200 M,O₂ is 0.100 M,and NO₂ is 0.250 M at 25°C?

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

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0100 M O₂.At this temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g)+ O₂(g)⇌ 2 CO₂(g). What is the equilibrium concentration of CO?

The following pictures represent mixtures of cis-C₂H₂X₂ molecules and trans-C₂H₂X₂molecules,which interconvert according to the equation cis-C₂H₂X₂ ⇌ trans-C₂H₂X₂.If mixture (1)is at equilibrium,which of the other mixtures are also at equilibrium?

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl₅(g)⇌ PCl₃(g)+ Cl₂(g) At 250° 0.125 M PCl₅ is added to the flask.If K_c = 1.80,what are the equilibrium concentrations of each gas?

Shown below is a concentration vs.time plot for the reaction A ⇌ 2B.For this reaction the value of the equilibrium constant is

What is the equilibrium equation for the dissociation of formic acid in water? HCOOH (aq)+ H₂O (l)⇌ H₃O⁺ (aq)+ HCOO^- (aq)

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

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 largest equilibrium constant?

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g). If initial concentrations are [SO₂] = 6.00 M,[O₂] = 0.45 M,and [SO₃] = 9.00 M,the system is

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.

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Exam 13: Chemical Equilibrium

If Kc = 0.900,and Kp = 538 for a hypothetical reaction,which of the equations below could represent the reaction at 25°C?

What is the equilibrium equation for the following reaction? FeS(s)+ 2 H3O+ (aq)⇌ Fe2+(aq)+ H2S (aq)+ 2 H2O (l)

Shown below is a concentration vs.time plot for the reaction A ⇌ 2B.For this reaction the value of the equilibrium constant is

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

Nitric oxide reacts with oxygen to form nitrogen dioxide: 2 NO(g)+ O2(g)⇌ 2 NO2(g) What is Kc for the forward reaction if the equilibrium concentration of NO is 0.200 M,O2 is 0.100 M,and NO2 is 0.250 M at 25°C?

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

An equilibrium mixture of CO,O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0100 M O2.At this temperature,Kc equals 1.4 × 102 for the reaction: 2 CO(g)+ O2(g)⇌ 2 CO2(g). What is the equilibrium concentration of CO?

The following pictures represent mixtures of cis-C2H2X2 molecules and trans-C2H2X2 molecules,which interconvert according to the equation cis-C2H2X2 ⇌ trans-C2H2X2.If mixture (1)is at equilibrium,which of the other mixtures are also at equilibrium?

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl5(g)⇌ PCl3(g)+ Cl2(g) At 250° 0.125 M PCl5 is added to the flask.If Kc = 1.80,what are the equilibrium concentrations of each gas?

Shown below is a concentration vs.time plot for the reaction A ⇌ 2B.For this reaction the value of the equilibrium constant is

What is the equilibrium equation for the dissociation of formic acid in water? HCOOH (aq)+ H2O (l)⇌ H3O+ (aq)+ HCOO- (aq)

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

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 largest equilibrium constant?

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO2(g)+ O2(g)⇌ 2 SO3(g). If initial concentrations are [SO2] = 6.00 M,[O2] = 0.45 M,and [SO3] = 9.00 M,the system is

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.

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Ionic Bonds and Some Main-Group Chemistry

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If K_c = 0.900,and K_p = 538 for a hypothetical reaction,which of the equations below could represent the reaction at 25°C?

What is the equilibrium equation for the following reaction? FeS(s)+ 2 H₃O⁺ (aq)⇌ Fe²⁺(aq)+ H₂S (aq)+ 2 H₂O (l)

Nitric oxide reacts with oxygen to form nitrogen dioxide: 2 NO(g)+ O₂(g)⇌ 2 NO₂(g) What is K_c for the forward reaction if the equilibrium concentration of NO is 0.200 M,O₂ is 0.100 M,and NO₂ is 0.250 M at 25°C?

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

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0100 M O₂.At this temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g)+ O₂(g)⇌ 2 CO₂(g). What is the equilibrium concentration of CO?

The following pictures represent mixtures of cis-C₂H₂X₂ molecules and trans-C₂H₂X₂molecules,which interconvert according to the equation cis-C₂H₂X₂ ⇌ trans-C₂H₂X₂.If mixture (1)is at equilibrium,which of the other mixtures are also at equilibrium?

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl₅(g)⇌ PCl₃(g)+ Cl₂(g) At 250° 0.125 M PCl₅ is added to the flask.If K_c = 1.80,what are the equilibrium concentrations of each gas?

What is the equilibrium equation for the dissociation of formic acid in water? HCOOH (aq)+ H₂O (l)⇌ H₃O⁺ (aq)+ HCOO^- (aq)

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

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 largest equilibrium constant?

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g). If initial concentrations are [SO₂] = 6.00 M,[O₂] = 0.45 M,and [SO₃] = 9.00 M,the system is

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.