   Chapter 9, Problem 82AP ### 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

# One step in the commercial production of sulfuric acid, H 2 SO 4 , involves the conversion of sulfur dioxide, SO 2 , into sulfur trioxide, SO 3 .msp;  2 SO 2 ( g ) + O 2 ( g ) → 2 SO 3 ( g ) 150 kg of SO 2 reacts completely, what mass of msp;  SO 3 should result?

Interpretation Introduction

Interpretation:

The mass of SO3 formed should be calculated.

Concept Introduction:

The commercial production of sulphuric acid, H2SO4 involves the following step in which sulphur dioxide, SO2 is converted into sulphur trioxide, SO3 as follows:

2SO2(g)+O2(g)2SO3(g)

The mass of SO3 can be calculated by calculating the number of moles of SO3 formed in the reaction.

Explanation

The chemical reaction is as follows:

2SO2(g)+O2(g)2SO3(g)

From the above balanced chemical reaction, 2 mole of SO2 on reaction with oxygen gives 2 moles of SO3.

Thus, 1 mol of SO2 gives 1 mol of SO3. The mass of SO2 is given 150 kg, number of moles of SO2 can be calculated as follows:

n=mM

Here, m is mass and M is molar mass.

Molar mass of SO2 is 64.066 g/mol, number of moles will be:

n=150 kg(1000 g1 kg)64.066 g/mol=2341

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