   # Sulfurous acid is unstable in aqueous solution and gradually decomposes to water and sulfur dioxide gas (which explains the choking with associated with sulfurous acid solutions). :math&gt; H 2 SO 3 ( a q ) → H 2 O ( l ) + SO 2 ( s ) 4.25 g of sulfurous acid undergoes this reaction, what mass of sulfur dioxide is released? ### Introductory Chemistry: A Foundati...

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

#### Solutions

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

9th Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781337399425
Chapter 9, Problem 33QAP
Textbook Problem
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## Sulfurous acid is unstable in aqueous solution and gradually decomposes to water and sulfur dioxide gas (which explains the choking with associated with sulfurous acid solutions).:math> H 2 SO 3 ( a q ) → H 2 O ( l ) + SO 2 ( s ) 4.25 g of sulfurous acid undergoes this reaction, what mass of sulfur dioxide is released?

Interpretation Introduction

Interpretation:

The mass of sulphur dioxide released from 4.25 g of sulphurous acid should be calculated.

Concept Introduction:

The balanced chemical reaction is as follows:

H2SO3(aq)H2O(l)+SO2(g)

From the balanced chemical reaction, 1 mol of sulfurous acid gives 1 mole of sulphur dioxide. The mass of sulphur dioxide produced can be calculated from its number of moles that can be calculated from number of moles of sulfurous acid.

### Explanation of Solution

Calculate the number of moles of sulfurous acid as follows;

n=mM

Here, molar mass of sulfurous acid is 82.07 g/mol thus,

n=4.25 g82.07 g/mol=0.0518 mol

From the balanced chemical reaction, 1 mol of sulfurous acid gives 1 mol of sulphur dioxide thus, 0.0518 mol gives 0

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