   Chapter 13, Problem 74QAP ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
5 views

# Small quantities of hydrogen gas can be prepared in the laboratory by the addition of aqueous hydrochloric acid to metallic zinc.msp;  Zn ( s ) + 2HCl ( a q )   ZnCl 2 ( a q ) + H 2 ( g ) pically, the hydrogen gas is bubbled through water for collection and becomes saturated with water vapor. Suppose 24 0.  mL of hydrogen gas is collected at 3 0   ° C and has a total pressure of 1 .0 32 mm by this process. What is the partial pressure of hydrogen gas in the sample? How many moles of hydrogen gas are present in the sample? How many grams of zincmust have reacted to produce this quantity of hydrogen? (The vapor pressure of water is 32 torr at 3 0   ° C .)

Interpretation Introduction

Interpretation:

The partial pressure of H2 and number of moles of H2 in the mixture should be calculated. Amount of zinc needed to produce that quantity of hydrogen should be calculated.

Concept Introduction:

According to Dalton’s law of partial pressure, if a container contains mixture of gases, the sum of partial pressures of all the gases present in the container is equal to the total pressure exerted on the wall of the container.

Thus, for three gases namely A, B and C with partial pressure PA, PB and PC the total pressure will be:

PT=PA+PB+PC

Where PT is the total pressure and PA, PB, PC are partial pressures of gases A, B and C The Ideal gas law;

PV = nRT

Where, P = Pressure of the ideal gas (atm)

V = Volume of the ideal gas (L)

n = number of moles of ideal gas present (mol)

R = Universal gas constant (L atm/K)

T = Temperature in Kelvin (K).

Explanation

According to the Dalton’s Law of partial pressure

PT=PO2+PH2O

1 torr = 0.00131579 atm

32 torr =32 torr× 0.00131579 atm1 torr = 0.042 atm 1.032 atm = PH2+0.042 atm PH2=0.990 atm

PV = nRT

0.990 atm×0

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