   Chapter 9, Problem 86AP ### 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
1 views

# When small quantities of elemental hydrogen gas are needed for laboratory work, the hydrogen is often generated by chemical reaction of a metal with acid. For example, tine reacts with hydrochloric acid, releasing gaseous elemental hydrogen::math> Zn ( s ) + 2 HCI ( a q ) → ZnCl 2 ( a q ) + H 2 ( g ) at mass of hydrogen gas is produced when 2.50 g of zinc is reacted with excess aqueous hydrochloride acid?

Interpretation Introduction

Interpretation:

The mass of hydrogen gas produced should be calculated.

Concept Introduction:

The reaction of zinc and hydrochloric acid to produced zinc chloride and hydrogen gas is as follows:

Zn(s)+2HCl(aq)Zn(Cl)2(aq)+H2(g)

The mass of hydrogen gas produced can be calculated from the number of moles of hydrogen gas produced. This can be calculated from the number of moles of Zn reacting in the reaction.

Explanation

Zn(s)+2HCl(aq)Zn(Cl)2(aq)+H2(g)

From the above balanced chemical reaction, 1 mole of Zn reacts with 2 moles of HCl to form 1 mole of ZnCl2 and 1 mol of H2.

The mass of Zn is given 2.50 g, number of moles of Zn can be calculated as follows:

n=mM

Here, m is mass and M is molar mass.

Molar mass of Zn is 65.38 g/mol, number of moles will be:

n=2

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