Chapter 17: Q42P (page 777)

Gaseous ammonia was introduced into a sealed container and heated to a certain temperature:
$2 {NH}_{3 (g)} ֏ N_{2 (g)} + 3 H_{2 (g)}$
At equilibrium, $[{NH}_{3}] = 0.0225 M, [N_{2}] = 0.114 M, and [H_{2}] = 0.342 M$ . Calculate Kc for the reaction at this temperature.

Short Answer

Expert verified

The value of the equilibrium constant $(K_{c})$ for the reaction at a certain temperature is 9.01.

Step by step solution

Step 1:Write the equilibrium constant

The equilibrium constant $(K_{c})$ is the constant that depends on the concentrations of reactants and products.

For a general chemical reaction,

aA + bB ֏ cC + dD

The equilibrium constant $(K_{c})$ is given as,

$K_{c} = \frac{{[C]}^{c} {[D]}^{d}}{{[A]}^{a} {[B]}^{b}}$

Here, a, b, c, and dare the stoichiometric coefficients.

Step2:Calculate Kc

Consider the following reaction;

2 {NH}_{3 (g)} ֏ N_{2 (g)} + 3 H_{2 (g)}

The equilibrium constant $(K_{c})$ for this reaction is given as,

$K_{c} = \frac{[N_{2}] {[H_{2}]}^{3}}{{[{NH}_{3}]}^{2}}$

From the given data,

$[{NH}_{3}] = 0.0225 M [N_{2}] = 0.114 M [H_{2}] = 0.342 M$

Substitute the concentration of $N_{2}, H_{2}, and {NH}_{3}$ to calculate the equilibrium constant $(K_{c})$ as follows:

role="math" localid="1654923012345" $K_{c} = \frac{[N_{2}] {[H_{2}]}^{3}}{{[{NH}_{3}]}^{2}} = \frac{(0.114) {(0.342)}^{3}}{{(0.0225)}^{2}} = \frac{0.00456}{0.000506} = 9.01$

Thus, the value of the equilibrium constant $(K_{c})$ for the reaction at a certain temperature is 9.01.

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Gaseous ammonia was introduced into a sealed container and heated to a certain temperature:
$2 {NH}_{3 (g)} ֏ N_{2 (g)} + 3 H_{2 (g)}$
At equilibrium, $[{NH}_{3}] = 0.0225 M, [N_{2}] = 0.114 M, and [H_{2}] = 0.342 M$ . Calculate Kc for the reaction at this temperature.

Short Answer

Step by step solution

Step 1:Write the equilibrium constant

Step2:Calculate Kc

One App. One Place for Learning.

Most popular questions from this chapter

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Gaseous ammonia was introduced into a sealed container and heated to a certain temperature:2NH3(g)֏N2(g)+3H2(g)At equilibrium, [NH3]=0.0225M,[N2]=0.114M,and[H2]=0.342M. Calculate Kc for the reaction at this temperature.

Short Answer

Step by step solution

Step 1:Write the equilibrium constant

Step2:Calculate Kc

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Chemical Analysis

Kinetics

Organic Chemistry

Ionic and Molecular Compounds

Nuclear Chemistry

Study anywhere. Anytime. Across all devices.

Gaseous ammonia was introduced into a sealed container and heated to a certain temperature:
$2 {NH}_{3 (g)} ֏ N_{2 (g)} + 3 H_{2 (g)}$
At equilibrium, $[{NH}_{3}] = 0.0225 M, [N_{2}] = 0.114 M, and [H_{2}] = 0.342 M$ . Calculate Kc for the reaction at this temperature.