Chapter 21, Problem 26PS

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# Compare the mass of H2 expected from the reaction of steam (H2O) per mole of methane, petroleum, and coal. (Assume complete reaction in each case. Use CH2 and CH as representative formulas for petroleum and coal, respectively.)

Interpretation Introduction

Interpretation:

To compare the mass of H2(g) expected from the reaction of steam per mole of methane, petroleum and coal.

Concept introduction:

The formula for methane is CH4 and coal is C. Petroleum is a hydrocarbon with a general formula of CnH2n+2.

All of them reacts with steam to produce carbon monoxide and water. 1 mole of these substances produce different moles of hydrogen. The conservation of mass should be followed for any chemical reaction.

Explanation

The mass of H2(g) expected from the reaction of steam per mole of methane, petroleum and coal is calculated below.

Given:

The balanced chemical equation for the reaction of coal with steam is,

Â Â Â Â C(s)+H2O(g)â†’CO(g)+H2(g)

One mole of coal is reacting with one mole of steam to produce one mole of hydrogen.

The mass of C is 12Â g/mol.

The mass of H2O(g) is 18Â g/mol.

The mass of CO is 28Â g/mol.

Thus, the total mass of product formed should be equal to the sum of mass of coal and steam according to the law of conservation of mass which is 30Â g.

The mass of hydrogen formed can be calculated by subtracting the mass of CO formed during the reaction.

Hence, the mass of hydrogen expected is 2Â g.

The balanced chemical equation for the reaction of methane with steam is,

Â Â Â Â CH4(g)+H2O(g)â†’CO(g)+3H2(g)

One mole of methane is reacting with one mole of steam to produce three moles of hydrogen.

The mass of CH4 is 16Â g/mol.

The mass of H2O(g) is 18Â g/mol

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