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Exam 17: Equilibrium: the Extent of Chemical Reactions

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Question 21

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Hydrogen bromide will dissociate into hydrogen and bromine gases. What effect will a temperature increase of 50 $\degree$ C have on this system at equilibrium?

A) The partial pressure of hydrogen bromide will increase.
B) The partial pressure of hydrogen will increase.
C) The partial pressure of hydrogen bromide and bromine will increase.
D) There will be no effect on the partial pressure of any of the gases.
E) Need to know the initial pressure, volume and temperature before any of the above predictions can be made.

F) B) and E)
G) C) and D)

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Question 22

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A chemical reaction will reach equilibrium when the limiting reactant is used up.

A) True
B) False

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Question 23

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Write the mass-action expression, Q_c, for the following chemical reaction.

The reaction system is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of carbon disulfide is reduced?

Ethane can be formed by reacting acetylene with hydrogen. Under which reaction conditions would you expect to have the greatest equilibrium yield of ethane?

The following reaction is at equilibrium in a closed container. Which, if any, of the following actions will lead to an increase in the pressure of H₂O present at equilibrium?

Once a reaction system reaches equilibrium, the concentrations of reactions and products no longer change.

10.0 mL of a 0.100 mol L¯¹ solution of a metal ion M²⁺ is mixed with 10.0 mL of a 0.100 mol l¯¹ solution of a substance L. The following equilibrium is established: At equilibrium, the concentration of L is found to be 0.0100 mol L¯¹. What is the equilibrium concentration of ML₂²⁺, in mol L¯¹?

A mixture of 0.600 mol of bromine and 1.600 mol of iodine is placed into a rigid 1.000-L container at 350 $\degree$ C. When the mixture has come to equilibrium, the concentration of iodine monobromide is 1.190 M. What is the equilibrium constant for this reaction at 350 $\degree$ C?

Magnesium carbonate dissociates to magnesium oxide and carbon dioxide at elevated temperatures. A reaction vessel contains these compounds in equilibrium at 300 $\degree$ C. What will happen if the volume of the container is reduced by 25% at 300 $\degree$ C?

Write the expressions for K_c and K_p for the reaction

The following reaction is at equilibrium at a pressure of 1 atm, in a closed container. Which, if any, of the following actions will decrease the concentration of CO₂ gas present at equilibrium?

If Q > K, more products need to be formed as the reaction proceeds to equilibrium.

The following reaction, in CCl₄ solvent, has been studied at 25 $\degree$ C. The equilibrium constant K_c is known to be 0.141. If the initial concentration of chlorine is 0.0300 M and of bromine monochloride is 0.0200 M, what is the equilibrium concentration of bromine?

Changing the amount of a solid reactant or product in an equilibrium reaction will not affect the amounts of the other reactants and products present at equilibrium.

Consider the equilibrium: A(s) B(s) + C(g), $\Delta$ H $\degree$ _rxn > 0 Predict and explain how or whether the following actions would affect this equilibrium. A) adding more solid A B) lowering the temperature C) increasing the pressure on the system by reducing its volume D) adding helium gas to increase the total pressure

When a reaction system reaches equilibrium, the forward and reverse reactions stop.

If all the reactants and products in an equilibrium reaction are in the gas phase, then K_p = K_c.

Compounds A, B, and C react according to the following equation. At 100 $\degree$ C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of K_c for this reaction?

The reaction of nitrogen with oxygen to form nitrogen monxide can be represented by the following equation. At 2000 $\degree$ C, the equilibrium constant, K_c, has a value of 4.10 * 10¯⁴. What is the value of K_p?