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Get Full Access to Introductory Chemistry - 5 Edition - Chapter 11 - Problem 114p
Get Full Access to Introductory Chemistry - 5 Edition - Chapter 11 - Problem 114p

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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

ISBN: 9780321910295 34

## Solution for problem 114P Chapter 11

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

Step 3 of 4

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