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# What minimum volume of hydrogen gas (at STP) is required ISBN: 9780321910295 34

## Solution for problem 114P Chapter 18

Introductory Chemistry | 5th Edition

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Problem 114P

What minimum volume of hydrogen gas (at STP) is required to fully hydrogenate 15.5 kg of propyne?

Step-by-Step Solution:

Step 1</p>

The balanced chemical equation for the hydrogenation of propyne is Step 2</p>Explanation:

Like with any stoichiometry problem, the key tool you have at your disposal is the mole ratio.

However, an interesting thing takes place when you're dealing with gases that are under the same conditions for pressure and temperature. In such cases, the mole ratio becomes the volume ratio.

The idea is that, since you're dealing with two ideal gases, you can use the ideal gas law equation to write

P⋅V1=n1⋅RT → for ethyne;

P⋅V2=n2⋅RT → for hydrogen.

The pressure and the temperature are the same for both gases, since the reaction presumably takes place at STP.

If you divided these two equations, you'll get

P⋅V1/P⋅V2=n1⋅RT/n2⋅RT

This is equivalent to

n1/n2=V1/V2.

The mole ratio is equivalent to the volume ratio.

Step 3 of 4

Step 4 of 4

##### ISBN: 9780321910295

Since the solution to 114P from 18 chapter was answered, more than 295 students have viewed the full step-by-step answer. The answer to “What minimum volume of hydrogen gas (at STP) is required to fully hydrogenate 15.5 kg of propyne?” is broken down into a number of easy to follow steps, and 17 words. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The full step-by-step solution to problem: 114P from chapter: 18 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. This full solution covers the following key subjects: fully, gas, hydrogen, hydrogenate, minimum. This expansive textbook survival guide covers 19 chapters, and 2045 solutions.

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