chem ch. 10 continued

The equilibrium constant for the reaction shown below is Kc=0.0091. If the equilibrium concentrations of A and B are 0.031 M and 0.0823 M, respectively, what is the equilibrium concentration of C? 3A(aq)⇌3B(aq)+2C(aq)

.022 M

At equilibrium for the reaction in aqueous medium below, the concentrations of A, B, C, and D are 0.011 M, 0.0067 M, 0.0124 M, and 0.0062 M, respectively. What is the equilibrium constant? A+2B⇌3C+D

.024

Consider the reaction below. At equilibrium, the concentration of A is 0.0502 M and the concentration of B is 0.057 M. If the equilibrium constant is Kc=3.8038, what is the equilibrium concentration of C? 2A(aq)+B(aq)⇌3C(aq)

.082

For the following equilibrium: 2A⇌B+C If equilibrium concentrations are [A]=0.95 M, [B]=0.45 M, and [C]=1.8 M, what is the equilibrium constant?

.90

Calculate the value of the equilibrium constant, Kc , for the system shown, if 0.1908 moles of CO2, 0.0908 moles of H2, 0.0092 moles of CO, and 0.0092 moles of H2O vapor were present in a 2.00 L reaction vessel at equilibrium. CO2 g+H2 g⇌CO g+H2O g

0.0049

Consider the reaction below. At equilibrium, the concentration of A is 0.0333 M and the concentration of B is 0.0831 M. If the equilibrium constant is Kc=10.9499, what is the equilibrium concentration of C? 2A(aq)+3B(aq)⇌3C(aq)

0.0191 M

The equilibrium constant for the reaction shown below is Kc=0.529. If the equilibrium concentrations of B and C are 0.0798 M and 0.0553 M, respectively, what is the equilibrium concentration of A? 2A(aq)⇌2B(aq)+C(aq)

0.0258 M

Consider the reaction below. At equilibrium, the concentration of A is 0.0242 M and the concentration of B is 0.0767 M. If the equilibrium constant is Kc=0.0266, what is the equilibrium concentration of C? 3A(g)⇌3B(g)+2C(g)

0.029 M

The equilibrium concentrations of A and B for the reaction below are 0.0055 M and 0.0272 M, respectively. If the equilibrium constant is Kc=0.4708, what is the equilibrium concentration of C? 2A(g)⇌B(g)+3C(g)

0.081 M

The equilibrium constant for the reaction below is 4.0. What is the equilibrium concentration of H2O when a mixture that is 1.4M in H2O, 1.6M in CO, and 1.6M in H2 are mixed to make 1.0L of solution? C(s)+H2O(g)⇌CO(g)+H2(g) Report your answer with two significant figures.

1.0 M

For the following equilibrium: A+2B⇌C If initial concentrations are [A]=0.50 M, [B]=0.75 M, and [C]=1.2 M, and at equilibrium [C]=1.0 M, what is the equilibrium constant?

1.1

The equilibrium constant for the reaction below is 1.0. What is the equilibrium concentration of H2 when a mixture that is 1.2M in C, 1.2M in H2O, 2.1M in CO, and 2.1M in H2 are mixed to make 1.0L of solution? C(s)+H2O(g)⇌CO(g)+H2(g)

1.4

Consider the following chemical reaction to answer the question that follows. Na2CO3+CaCl2⇌2NaCl+CaCO3 The initial concentrations of CaCl2 and Na2CO3 in a solution are both equal to 0.34 M. After the reaction reaches equilibrium, the concentration of Na2CO3 is 0.05 M. What is the expression for the change in concentration of NaCl?

2x

What is the coefficient for O2 in the balanced version of the following chemical equation: C2H4+O2→CO2+H2O

3

Hydrogen gas and gaseous iodine will react to form hydrogen iodide, as described by the following chemical equation. H2(g)+I2(g)↽−−⇀2HI(g)Kc(400∘C)=50.0 Assume that all of the HI(g) is removed from a vessel containing this reaction, and equilibrium is re-established. What will be the new equilibrium concentration of HI if the equilibrium concentrations of H2 and I2 are both equal to 0.450M?

3.18

For the following equilibrium: 3A+B↽−−⇀2C If equilibrium concentrations are [A]=1.1 M and [B]=1.4 M, and Kc=11.3, what is the equilibrium concentration of C?

4.6 M

Initially, a mixture of 0.100 M NO,0.050 M H2,0.100 M H2O was allowed to reach equilibrium (initially there was no N2). At equilibrium the concentration of NO was found to be 0.062 M. Determine the value of the equilibrium constant, Kc, for the reaction: 2NO+2H2↔N2+2H2O

6.5×102

At a certain temperature, the equilibrium constant for the reaction below is 4.55×10−2. Calculate the equilibrium concentration of hydrogen if the equilibrium concentrations of nitrogen and ammonia are 3.98 M and 7.32 M, respectively. N2+3H2⇋2NH3

6.66 M

An equilibrium constant is described by which of the following?

An equilibrium constant is the value of the reaction quotient for a system at equilibrium.

If we plug equilibrium concentrations into the reaction quotient expression, we should be able to calculate:

Kc

Given the reaction below, what is the equilibrium expression? 2CO2(g)+2H2O(g)⇌C2H4(g)+3O2(g)

Kc=[C2H4][O2]^3 --------------- [CO2]^2[H2O]^2

What will be the equilibrium expression for the following equilibrium: C4H8→2C2H4

Kc=[C2H4]^2 ------------- [C4H8]

Question Write the equilibrium expression for the following reaction: 2Fe2O3(s)+3C(s)⇌4Fe(s)+3CO2(g)

Kc=[CO2]3

Find the equilibrium expression for the reversible reaction below. 2NO(g)+Cl2(g)⇌2NOCl(g)

Kc=[NOCl]^2 ----- [NO]^2[Cl2]

What is the chemical equilibrium that would generate the following equilibrium constant expression: Kc=[SO3]^2 ------------- [O2][SO2]^2

O2+2SO2→2SO3

Which of the following is NOT true regarding a system in equilibrium?

Only the concentration of the reactants is constant.

Acetic acid, CH3CO2H, reacts with ethanol, C2H5OH, to form ethyl acetate, CH3CO2C2H5 and water. CH3CO2H+C2H5OH↽−−⇀CH3CO2C2H5+H2O The equilibrium constant for this reaction with dioxane as a solvent is 4.0. What are the equilibrium concentrations when a mixture that is 0.15 M in CH3CO2H,0.15 M in C2H5OH,0.40 M in CH3CO2C2H5, and 0.40 M in H2O are mixed in enough dioxane to make 1.0 L of solution?

[CH3CO2H] = 0.18 M, [C2H5OH] = 0.18 M, [CH3CO2C2H5] = 0.37 M, [H2O] = 0.37 M

Under certain conditions, the equilibrium constant for the following equation is 6.0. H2+I2↽−−⇀2HI What are the equilibrium concentrations of H2,l2, and HI if the initial concentration of HI was 4.0 M and the initial concentrations of both H2 and l2 are zero?

[H2]=0.90 M,[I2]=0.90 M,[HI]=2.2 M

The equilibrium constant is equal to the reaction quotient when the system is:

at equilibrium

In an ICE chart, the C stands for:

change

When calculating changes in concentration, the algebraic terms calculated from the stoichiometry of the equilibrium equation will go into which row of an ICE chart?

change

If K is followed by a subscript c, that means it is evaluated using:

concentrations

To calculate changes in concentration for a system not at equilibrium, we must first:

determine the direction the equilibrium will move

If Q is less than K, in which direction will the equilibrium proceed?

forward

As a reaction proceeds in the forward direction, K will:

increase

Which of the following concentrations appear in the numerator of the equilibrium constant expression?

product

Once we have initial concentrations listed in the ICE chart, the next step is to calculate:

relative changes in concentration

Question If Q is greater than K, in which direction will the equilibrium proceed?

reverse

The Kc for a system will vary depending on the:

temperature of the system

It can be difficult to differentiate a system at equilibrium from a system containing a:

very slow chemical reaction