Question 1

An increase in the number of moles of gas as the reaction goes from reactants to products in a gas-phase equilibrium results in ________

Accepted Answer

A) Kp F1F1F1S1F1F1F10 Kc. 
B) Kp F1F1F1S1F1F1F10 Kc. 
C) Kp F1F1F1S1F1F1F10 Kc. 
D) Kp F1F1F1S1F1F1F10 Kc F1F1F1S1F1F1F10 (RT )  F1F1F1S1F1F1F10. 
E) KpKc F1F1F1S1F1F1F10 (RT )  F1F1F1S1F1F1F10.

Question 2

A reaction is run under conditions in which the equilibrium constant is known to be 2.5. F1F1F1S1F1F1F10F1F1F1S1F1F1F1010². At equilibrium, the forward rate is determined to be 5.0 F1F1F1S1F1F1F10 10F1F1F1S1^F1F1F10⁴ mol LF1F1F1S1^F1F1F10¹ sF1F1F1S1^F1F1F10¹. What is the rate of the reverse reaction under these conditions?

Accepted Answer

The answer of A reaction is run under conditions in...

Question 3

The equilibrium constant for the formation of calcium carbonate from the ions in solution is 2.2 F1F1F1S1F1F1F10 108 according to the reaction:    What is the value of the equilibrium constant for the reverse of this reaction?

Accepted Answer

A) the same, 2.2 F1F1F1S1F1F1F10 108 
B) (F1F1F1S1F1F1F102.2 F1F1F1S1F1F1F10 108) 
C) 2.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 
D) 4.5 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F109 
E) 4.5 F1F1F1S1F1F1F10 109

Question 4

The reaction of bromine gas with chlorine gas, shown here, has a Kp value of 7.20. If a closed vessel was charged with the two reactants, each at an initial partial pressure of 0.500 atm, and the product also at 0.500 atm, what would be the equilibrium partial pressure of BrCl(g)? Br2(g) F1F1F1S1F1F1F10 Cl2(g)  2BrCl(g)

Accepted Answer

A) 0.500 atm 
B) 0.680 atm 
C) 0.859 atm 
D) 0.029 atm 
E) 0.987 atm

Question 5

Hydrofluoric acid is used in the preparation of numerous pharmaceuticals (e.g., Prozac) and industrial materials (e.g., Teflon). It can be produced by the reaction of hydrogen and fluorine gases. Starting with initial concentrations of 2.00 M for H2 and 2.00 M for F2, what would be the equilibrium concentration of HF? The equilibrium constant for the reaction Kc F1F1F1S1F1F1F10 115.

Accepted Answer

A) 0.85 M 
B) 1.69 M 
C) 2.85 M 
D) 3.37 M 
E) 4.00 M

Question 6

Water can decompose at an elevated temperature to give hydrogen and oxygen according to the equation below. At a particular temperature in a vessel containing water vapor and air, the partial pressures of H2O, H2, and O2 are 0.055 atm, 0.0065 atm, and 0.19 atm, respectively. What is the value of the reaction quotient, QP, for this reaction under these conditions? 2H2O(g)  2H2(g) F1F1F1S1F1F1F10 O2(g)

Accepted Answer

A) 0.023 
B) 1.5 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
C) 2.7 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 
D) 370 
E) 4.4 F1F1F1S1F1F1F10 104

Question 7

The sulfide ion, S²F1F1F1S1^F1F1F10, reacts with water as a weak base: S²F1F1F1S1^F1F1F10F1F1F1S1F1F1F10 H₂O SHF1F1F1S1^F1F1F10 F1F1F1S1F1F1F10 OHF1F1F1S1^F1F1F10K F1F1F1S1F1F1F10 1.0 If sodium sulfide were dissolved in water to make a solution of 0.50 M, what would be the resulting concentration of OHF1F1F1S1^F1F1F10?

Accepted Answer

The answer of The sulfide ion, S²F1F1F1S1^F1F1F10, reacts with water...

Question 8

Write the equilibrium expression for the reaction

Accepted Answer

A)   
B)   
C)   
D)   
E)

Question 9

Which of the following occurs when reactants are added to a chemical reaction in solution or the gas phase at equilibrium?

Accepted Answer

A) Q increases and the equilibrium shifts to produce more products. 
B) Q increases and the equilibrium shifts to produce more reactants. 
C) Q decreases and the equilibrium shifts to produce more products. 
D) Q decreases and the equilibrium shifts to produce more reactants. 
E) Q is unchanged by the addition of reactants.

Question 10

If the temperature of an endothermic reaction at equilibrium could be increased instantaneously, what would be the instantaneous effect on Q and K before equilibrium was again achieved?

Accepted Answer

A) Q would increase and K would stay the same. 
B) Q would decrease and K would stay the same. 
C) Q would stay the same and K would increase. 
D) Q would stay the same and K would decrease. 
E) Both Q and K would stay the same.

Question 11

Using the Reaction, Initial, Change, Equilibrium (RICE) table started for calculating equilibrium concentrations of the reaction shown, what is the expression for the equilibrium constant in terms of x? 2NOCl(g)  2NO(g) F1F1F1S1F1F1F10 Cl2(g)
R [NOCl] [NO] [Cl2]
I 0.20 M 0 M 0 M
C
E

Accepted Answer

A)   
B)   
C)   
D)   
E)

Question 12

The gas-phase equilibrium of the oxidation of sulfur dioxide, shown here, has an equilibrium constant, Kp, value of 4.17 F1F1F1S1F1F1F10 102 at 200F1F1F1S1F1F1F10C. If a closed vessel was filled with sulfur trioxide and the initial pressure of SO3 was 0.033 atm at 200F1F1F1S1F1F1F10C, what would be the final partial pressure of SO3? 2SO2(g) F1F1F1S1F1F1F10 O2(g)  2SO3(g)

Accepted Answer

A) more than 0.033 atm 
B) less than 0.033 atm 
C) 0.033 atm exactly 
D) There is no way to tell.

Question 13

The reaction of bromine gas with chlorine gas, shown below, has a Kp value of 0.127. If a closed vessel was charged with the reactant at an initial partial pressure of 0.500 atm, what would be the equilibrium partial pressure of Br2(g)? 2BrCl(g)  Br2(g) F1F1F1S1F1F1F10 Cl2(g)

Accepted Answer

A) 0.412 atm 
B) 0.196 atm 
C) 0.252 atm 
D) 0.304 atm 
E) 0.104 atm

Question 14

Sulfur dioxide emitted in the burning of coal is "scrubbed" from the effluent using ________

Accepted Answer

A) limestone (CaCO3). 
B) lime (CaO). 
C) calcium metal (Ca). 
D) calcium hydride (CaH2). 
E) calcium hydroxide [Ca(OH)2].

Question 15

In equilibrium expressions, the concentrations of pure solids and liquids ________

Accepted Answer

A) have the assigned value of one. 
B) have the assigned value of zero. 
C) have constant values, cS and cl. 
D) are determined from the density and molar mass. 
E) are treated as any other solute.

Question 16

If the reaction quotient Q is equal to the related equilibrium constant, K, ________

Accepted Answer

A) the reaction is at equilibrium. 
B) the reaction will continue to make more products. 
C) the reaction will consume products and make reactants. 
D) the reaction will release heat to achieve equilibrium. 
E) the value of K will increase until it is equal to Q.

Question 17

For the reaction of hydrogen and nitrogen gases at 30°C to form two moles of ammonia gas (NH₃), the value of K_P is 4.5 F1F1F1S1F1F1F10 10F1F1F1S1^F1F1F10¹². What is the equilibrium expression for K_c for the production of two moles of ammonia in terms of K_P and variables from the ideal gas law?

Accepted Answer

The answer of For the reaction of hydrogen and nitrogen...

Question 18

Gaseous hydrogen and iodine can be used to prepare HI in the following balanced chemical reaction. Calculate a value for the reaction quotient when [H2] F1F1F1S1F1F1F10 [I2] F1F1F1S1F1F1F10 4.67 F1F1F1S1F1F1F1010-3 M and [HI] F1F1F1S1F1F1F10 4.07 F1F1F1S1F1F1F10 10-2 M. H2(g) F1F1F1S1F1F1F10 I2(g)  2HI(g)

Accepted Answer

A) 1.32 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F102 
B) 1.87 F1F1F1S1F1F1F10 103 
C) 76.0 
D) 5.36 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
E) 1.77 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F101

Question 19

How would an increase in temperature affect the following equilibrium? H2O(l )  H2(g) F1F1F1S1F1F1F10  O2(g)  F1F1F1S1F1F1F10HF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 482.0 kJ/mol

Accepted Answer

A) More product would form and K would increase. 
B) More product would form but K would remain constant. 
C) K would be unaffected by a temperature change. 
D) More reactants would form but K would remain constant. 
E) More reactants would form and K would decrease.

Question 20

Equilibrium constants for gases can be expressed in terms of concentrations, Kc, or in terms of partial pressures, Kp. Which one of the following statements regarding Kc and Kp is correct?

Accepted Answer

A) Kc and Kp are equal when all stoichiometric coefficients in the balanced reaction equation equal one. 
B) Kc and Kp have the same values but different units. 
C) Kc and Kp are equal when the sum of the stoichiometric coefficients for the products equals the sum of the stoichiometric coefficients for the reactants. 
D) Kc and Kp can never be equal. 
E) Kc and Kp are equal when the conditions are standard (P F1F1F1S1F1F1F10 1 atm, T F1F1F1S1F1F1F10 298 K).

Exam 14: Chemical Equilibrium: How Much Product Does a Reaction Really Make

An increase in the number of moles of gas as the reaction goes from reactants to products in a gas-phase equilibrium results in ________

A reaction is run under conditions in which the equilibrium constant is known to be 2.5. 10². At equilibrium, the forward rate is determined to be 5.0  10^⁴ mol L^¹ s^¹. What is the rate of the reverse reaction under these conditions?

The equilibrium constant for the formation of calcium carbonate from the ions in solution is 2.2  10⁸ according to the reaction: What is the value of the equilibrium constant for the reverse of this reaction?

The sulfide ion, S²^, reacts with water as a weak base: S²^ H₂O SH^  OH^K  1.0 If sodium sulfide were dissolved in water to make a solution of 0.50 M, what would be the resulting concentration of OH^?

Write the equilibrium expression for the reaction

Which of the following occurs when reactants are added to a chemical reaction in solution or the gas phase at equilibrium?

If the temperature of an endothermic reaction at equilibrium could be increased instantaneously, what would be the instantaneous effect on Q and K before equilibrium was again achieved?

Using the Reaction, Initial, Change, Equilibrium (RICE) table started for calculating equilibrium concentrations of the reaction shown, what is the expression for the equilibrium constant in terms of x? 2NOCl(g) 2NO(g)  Cl₂(g) R [NOCl] [NO] [Cl₂] I 0.20 M 0 M 0 M C E

The reaction of bromine gas with chlorine gas, shown below, has a K_p value of 0.127. If a closed vessel was charged with the reactant at an initial partial pressure of 0.500 atm, what would be the equilibrium partial pressure of Br₂(g) ? 2BrCl(g) Br₂(g)  Cl₂(g)

Sulfur dioxide emitted in the burning of coal is "scrubbed" from the effluent using ________

In equilibrium expressions, the concentrations of pure solids and liquids ________

If the reaction quotient Q is equal to the related equilibrium constant, K, ________

For the reaction of hydrogen and nitrogen gases at 30°C to form two moles of ammonia gas (NH₃), the value of K_P is 4.5  10^¹². What is the equilibrium expression for K_c for the production of two moles of ammonia in terms of K_P and variables from the ideal gas law?

Gaseous hydrogen and iodine can be used to prepare HI in the following balanced chemical reaction. Calculate a value for the reaction quotient when [H₂]  [I₂]  4.67 10^-³ M and [HI]  4.07  10^-²M. H₂(g)  I₂(g) 2HI(g)

How would an increase in temperature affect the following equilibrium? H₂O(l ) H₂(g)  O₂(g) H^  482.0 kJ/mol

Equilibrium constants for gases can be expressed in terms of concentrations, K_c, or in terms of partial pressures, K_p. Which one of the following statements regarding K_c and K_p is correct?

Exam 14: Chemical Equilibrium: How Much Product Does a Reaction Really Make

An increase in the number of moles of gas as the reaction goes from reactants to products in a gas-phase equilibrium results in ________

A reaction is run under conditions in which the equilibrium constant is known to be 2.5. 102. At equilibrium, the forward rate is determined to be 5.0  104 mol L1 s1. What is the rate of the reverse reaction under these conditions?

The equilibrium constant for the formation of calcium carbonate from the ions in solution is 2.2  108 according to the reaction: What is the value of the equilibrium constant for the reverse of this reaction?

The sulfide ion, S2, reacts with water as a weak base: S2 H2O SH  OH K  1.0 If sodium sulfide were dissolved in water to make a solution of 0.50 M, what would be the resulting concentration of OH?

Write the equilibrium expression for the reaction

Which of the following occurs when reactants are added to a chemical reaction in solution or the gas phase at equilibrium?

If the temperature of an endothermic reaction at equilibrium could be increased instantaneously, what would be the instantaneous effect on Q and K before equilibrium was again achieved?

Using the Reaction, Initial, Change, Equilibrium (RICE) table started for calculating equilibrium concentrations of the reaction shown, what is the expression for the equilibrium constant in terms of x? 2NOCl(g) 2NO(g)  Cl2(g) R [NOCl] [NO] [Cl2] I 0.20 M 0 M 0 M C E

The reaction of bromine gas with chlorine gas, shown below, has a Kp value of 0.127. If a closed vessel was charged with the reactant at an initial partial pressure of 0.500 atm, what would be the equilibrium partial pressure of Br2(g) ? 2BrCl(g) Br2(g)  Cl2(g)

Sulfur dioxide emitted in the burning of coal is "scrubbed" from the effluent using ________

In equilibrium expressions, the concentrations of pure solids and liquids ________

If the reaction quotient Q is equal to the related equilibrium constant, K, ________

For the reaction of hydrogen and nitrogen gases at 30°C to form two moles of ammonia gas (NH3), the value of KP is 4.5  1012. What is the equilibrium expression for Kc for the production of two moles of ammonia in terms of KP and variables from the ideal gas law?

Gaseous hydrogen and iodine can be used to prepare HI in the following balanced chemical reaction. Calculate a value for the reaction quotient when [H2]  [I2]  4.67 10-3 M and [HI]  4.07  10-2 M. H2(g)  I2(g) 2HI(g)

How would an increase in temperature affect the following equilibrium? H2O(l ) H2(g)  O2(g) H  482.0 kJ/mol

Equilibrium constants for gases can be expressed in terms of concentrations, Kc, or in terms of partial pressures, Kp. Which one of the following statements regarding Kc and Kp is correct?

A reaction is run under conditions in which the equilibrium constant is known to be 2.5. 10². At equilibrium, the forward rate is determined to be 5.0  10^⁴ mol L^¹ s^¹. What is the rate of the reverse reaction under these conditions?

The equilibrium constant for the formation of calcium carbonate from the ions in solution is 2.2  10⁸ according to the reaction: What is the value of the equilibrium constant for the reverse of this reaction?

The sulfide ion, S²^, reacts with water as a weak base: S²^ H₂O SH^  OH^K  1.0 If sodium sulfide were dissolved in water to make a solution of 0.50 M, what would be the resulting concentration of OH^?

Using the Reaction, Initial, Change, Equilibrium (RICE) table started for calculating equilibrium concentrations of the reaction shown, what is the expression for the equilibrium constant in terms of x? 2NOCl(g) 2NO(g)  Cl₂(g) R [NOCl] [NO] [Cl₂] I 0.20 M 0 M 0 M C E

The reaction of bromine gas with chlorine gas, shown below, has a K_p value of 0.127. If a closed vessel was charged with the reactant at an initial partial pressure of 0.500 atm, what would be the equilibrium partial pressure of Br₂(g) ? 2BrCl(g) Br₂(g)  Cl₂(g)

For the reaction of hydrogen and nitrogen gases at 30°C to form two moles of ammonia gas (NH₃), the value of K_P is 4.5  10^¹². What is the equilibrium expression for K_c for the production of two moles of ammonia in terms of K_P and variables from the ideal gas law?

Gaseous hydrogen and iodine can be used to prepare HI in the following balanced chemical reaction. Calculate a value for the reaction quotient when [H₂]  [I₂]  4.67 10^-³ M and [HI]  4.07  10^-²M. H₂(g)  I₂(g) 2HI(g)

How would an increase in temperature affect the following equilibrium? H₂O(l ) H₂(g)  O₂(g) H^  482.0 kJ/mol

Equilibrium constants for gases can be expressed in terms of concentrations, K_c, or in terms of partial pressures, K_p. Which one of the following statements regarding K_c and K_p is correct?