K equilbrium

Consider the following graph:

When equilibrium is reached, the rate of the forward reaction is

• 0.00 mol/min

• 0.25mol/min

• 1.0 mol/min

• 3.0 mol/min

Consider the following equilibrium:

2NO_{2 (g) <->} N₂O_{4 (g)} + energy

The equilibrium will shift to the left as a result of

• adding a catalyst.

• increasing the volume.

• removing some N₂O₄.

• decreasing the temperature.

Consider the following equilibrium:

N_{2 (g)} + 3H_{2 (g) <->} 2NH_{3 (g)} + energy

Certain conditions provide less than 10% yield of NH3 at equilibrium. Which of the following describes this equilibrium?

• A

• B

• C

• D

Which of the following best describes the relationship between K_eq and temperature

for an endothermic reaction?

• A

• B

• C

• D

Consider the following equilibrium:

2NO_{2(g) <->} N₂O_4(g)

A 1.00 L flask contains 0.030 mol NO₂ and 0.040 mol N₂O₄ at equilibrium.

The value of K_eq is

• 0.023

• 0.67

• 1.3

• 44

Tags

NGSS.HS-PS1-6

Consider the following reaction:

2H_2(g) + O_{2(g) <->} 2H₂O_(l)

What is the equilibrium constant expression for the reaction?

• A

• B

• C

• D

Consider the following equilibrium:

2NOBr_{(g) <->} 2NO_(g) + Br_2(g) K_eq = 6.4 X 10^-2

At equilibrium, a 1.00 L flask contains 0.030 mol NOBr and 0.030 mol NO.

How many mol Br₂ are present?

• 1.9 X 10^-3 mol

• 6.4 X10^-2 mol

• 3.0 X10^-2 mol

• 4.7 X10^-1 mol

Tags

NGSS.HS-PS1-7

Consider the following equilibrium:

2NO_(g) + O_2(g) <-> 2NO_{2 (g)} + energy

When the volume of the container is increased, the equilibrium shifts to the

• left and K_eq decreases.

• right and K_eq increases.

• left and Keq remains constant.

• right and Keq remains constant.

Consider the following reaction:

2Hg_(g) + O_2(g) <-> 2HgO_(s)

The equilibrium constant expression for the reaction is

• A

• B

• C

• D

The value of Keq changes when

• a catalyst is added.

• the temperature changes.

• the surface area changes.

• the concentration of reactants changes.