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Consider the reaction:P4(s) + 6H2(g) ? 4 PH3(g)(a) If 88.6 L of H2(g), measured at STP

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

Solution for problem 114P Chapter 11

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 114P

Consider the reaction:

\(P_{4}(s)+6\ \mathrm{H}_{2}(g) \rightarrow 4\ \mathrm{PH}_{3}(g)\)

(a) If 88.6 L of \({H}_{2}\)( g), measured at STP, is allowed to react with 158.3 g of \({P}_{4}\), what is the limiting reactant?

(b) If 48.3 L of \({P H}_{3}\), measured at STP, forms, what is the percent yield?

Equation Transcription:

Text Transcription:

P_4 (s) + 6 H_2 (g) right arrow 4 PH_3 (g)

Step-by-Step Solution:

Step 1 of 4

Given reaction:

(a) If 88.6 L of (g), measured at STP, is allowed to react with 158.3 g of , what is the limiting reactant?

To find the limiting reactant, we should know the moles of each reactant. So let’s find the number of moles of each reactant :

First, let’s find number of moles of  :

We know, at STP(Standard Temperature and Pressure), one mole of any gas occupies 22.4 L.

 

Moles of  =

                     = 3.955 moles.

Now, let’s find number of moles of  :

Molar mass of  = 123.89 g/mol.

 

moles of  =

                     = 1.277 moles.

Step 2 of 4

Chapter 11, Problem 114P is Solved
Step 3 of 4

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

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Consider the reaction:P4(s) + 6H2(g) ? 4 PH3(g)(a) If 88.6 L of H2(g), measured at STP