   # Consider the reaction 4PH 3 ( g ) → P 4 ( g ) +6H 2 ( g ) If, in a certain experiment, over a specific time period, 0.0048 mole of PH 3 is consumed in a 2.0-L container each second of reaction, what are the rates of production of P 4 and H 2 in this experiment? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 11, Problem 23E
Textbook Problem
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## Consider the reaction 4PH 3 ( g )   →   P 4 ( g ) +6H 2 ( g ) If, in a certain experiment, over a specific time period, 0.0048 mole of PH3 is consumed in a 2.0-L container each second of reaction, what are the rates of production of P4 and H2 in this experiment?

Interpretation Introduction

Interpretation: A reaction in which a stated amount of PH3 is consumed to produce P4 and H2 is given. The rates of production of P4 and H2 are to be calculated.

Concept introduction: The rate of a reaction is defined as the decrease in the concentration of a reactant or the increase in the concentration of the product per unit time.

### Explanation of Solution

To determine: The rates of production of P4 .

Given

The stated reaction is,

4PH3(g)P4(g)+6H2(g)

The moles of PH3 consumed are 0.0048mole .

The volume of container is 2.0L .

0.0048mole are consumed in a 2.0L container each second.

According to the given reaction,

4mol of PH3 form P4 =1mol

1mol of PH3 form P4 =(14)mol

0.0048mole of PH3 form P4 =(1×0.00484)mol=0.0012mol

0.0012mol of PH3 are formed in one second in a 2L container.

Therefore, the rate of formation of PH3 per litre =(0.00122)mol/Ls=6.0×10-4mol/Ls_

To determine: The rates of production of H2

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