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# Consider the reaction: A sample of pure NH4HS is placed in ## Problem 104P Chapter 15

Introductory Chemistry | 5th Edition

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Problem 104P

Consider the reaction: A sample of pure NH4HS is placed in a sealed 2.0-L container and heated to 550 K at which the equilibrium constant is 3.5 × 10‒3. Once the reaction reaches equilibrium, what mass of NH3 is in the container? (Assume that the sample of NH4HS was large enough that equilibrium could be achieved.)

Step-by-Step Solution:

Solution 104P:

Step 1: The equilibrium constant is

Keq = = [NH3][H2S]

Thus, we know that, NH4HS(s) is a solid, so that it is not included into the equilibrium constant.

Keq= 3.5 × 10‒3.

[NH3][H2S] =  3.5 × 10‒3.

From equation, 1 mol NH4HS(s) produces 1.0 mol of NH3(g) and (H2S each.

Thus,

[NH3] = [H2S]

Therefore.

Keq =  [NH3][H2S] =  [NH3]2 [NH3]2 = 3.5 × 10‒3. [NH3] = = 0.059 M

Step 2:

The moles of  NH3 is = 2.0 L x 0.059 mol/ 1.0 L

= 0.118 mol

Step 3 of 3

##### ISBN: 9780321910295

Since the solution to 104P from 15 chapter was answered, more than 252 students have viewed the full step-by-step answer. This full solution covers the following key subjects: Equilibrium, reaction, sample, container, large. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. The full step-by-step solution to problem: 104P from chapter: 15 was answered by Patricia, our top Chemistry solution expert on 05/06/17, 06:45PM. Introductory Chemistry was written by Patricia and is associated to the ISBN: 9780321910295. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. The answer to “Consider the reaction: A sample of pure NH4HS is placed in a sealed 2.0-L container and heated to 550 K at which the equilibrium constant is 3.5 × 10?3. Once the reaction reaches equilibrium, what mass of NH3 is in the container? (Assume that the sample of NH4HS was large enough that equilibrium could be achieved.)” is broken down into a number of easy to follow steps, and 56 words.

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