When gasoline burns in an automobile engine, nitric oxide is formed from oxygen and nitrogen. Nitric oxide is a major air pollutant. High temperatures, such as those found in a combustion engine, are needed for the following reaction:

$$\mathrm { N } _ { 2 } ( g ) + \mathrm { O } _ { 2 } ( g ) \Longleftrightarrow 2 \mathrm { NO } ( g )$$

. K for the reaction is 0.01 at

$$2000 ^ { \circ } \mathrm { C }$$

. If 4.0 mol of

$$N_2$$

, 0.1 mol of

$$O_2$$

, and 0.08 mol of NO are placed in a 1.0-L vessel at

$$2000 ^ { \circ } \mathrm { C }$$

, predict which reaction will be favored.

An equilibrium mixture at a specific temperature is found to consist of

$$1.2 \times 10 ^ { - 3 } \mathrm { mol } / \mathrm { L } \mathrm { Cl }, 3.8 \times 10 ^ { - 4 } \mathrm { mol } / \mathrm { L } \mathrm { O } _ { 2 } , 5.8 \times 10 ^ { - 2 } \mathrm { mol } / \mathrm { L } \mathrm { H } _ { 2 } \mathrm { O }$$

, and

$$5.8 \times 10 ^ { - 2 } \mathrm { mol } / \mathrm { L } \mathrm { Cl } _ { 2 }$$

according to the following:

$$4 \mathrm { HCl } ( g ) + \mathrm { O } _ { 2 } ( g ) \Longleftrightarrow 2 \mathrm { H } _ { 2 } \mathrm { O } ( g ) + 2 \mathrm { Cl } _ { 2 } ( g )$$

In general, which reaction is favored (forward or reverse) if the value of K at a specified temperature is a. very small? b. very large?

Describe and explain how the concentrations of A, B, C, and D change from the time when A and B are first combined to the point at which equilibrium is established for the reaction A+B

$$\Longleftrightarrow \mathrm { C } + \mathrm { D }$$

.

A solution of AgI contains

$$2.7 \times 10 ^ { - 10 } \mathrm { mol } / \mathrm { L } \mathrm { Ag } ^ { + }$$

. What is the maximum

$$I ^ { - }$$

concentration that can exist in this solution?

Let s equal the solubility, in mol/L, of

$$AB_2$$

. In terms of s, what is the molar concentration of A? of B? What is the

$$K _ { \mathrm { sp } }$$

of

$$AB_2$$

?