   Chapter 20, Problem 19PS

Chapter
Section
Textbook Problem

Hydrogen can be produced using the reaction of steam (H2O) with various hydrocarbons. Compare the mass of H2 expected from the reaction of steam with 100. g each of methane, petroleum, and coal. (Assume complete reaction in each case. Use CH2 and C as the representative formulas for petroleum and coal, respectively.)

Interpretation Introduction

Interpretation:

The mass of hydrogen H2 produced from the reaction of steam with the given substances should be determined.

Concept introduction:

• Numberofmole=GivenmassofthesubstanceMolarmass
• The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol) .
• For chemical reaction balanced chemical reaction equation established in accordance with the Law of conservation of mass.
• Stoichiometric factor is a relationship between reactant and product which is obtained from the balanced chemical equation for a particular reaction.
Explanation

Hydrogen can be produced using the reaction of steam with various hydrocarbons.

Here hydrogen is produced by the reaction of steam with 100g each of methane, petroleum and coal.

The mass of hydrogen H2 produced from the reaction of steam with these can be calculated as follows,

• From methane

Balanced equation for the reaction of steam with methane is,

H2O(g)+CH4(g)3H2(g)+CO(g)

The amount of methane in moles needed for complete the reaction with steam is,

100g16g/mol=6.25molCH4

Using the stoichiometric factor calculating the mass of hydrogen produced,

6.25molCH4×3molH21molCH4×2.02g/molH2=37.9g

The mass of hydrogen produced from methane is 37.9g.

• From petroleum,

Balanced equation for the reaction of steam with petroleum is,

H2O(g)+CH2(l)2H2(g)+CO(g)

The amount of petroleum in moles needed for complete the reaction with steam is,

100g14g/mol=7

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