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Solved: Consider the reaction: A sample of pure NH4HS is placed in a sealed 2.0-L

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 104P Chapter 15

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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Problem 104P

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 of 3

Chapter 15, Problem 104P is Solved
Step 3 of 3

Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

Since the solution to 104P from 15 chapter was answered, more than 400 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 2046 solutions. The full step-by-step solution to problem: 104P from chapter: 15 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. Introductory Chemistry was written by 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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Solved: Consider the reaction: A sample of pure NH4HS is placed in a sealed 2.0-L