   Chapter 4, Problem 24PS

Chapter
Section
Textbook Problem

Methanol, CH3OH, can be prepared from carbon monoxide and hydrogen.CO(g) + 2 H2(g) → CH3OH(l)What mass of hydrogen is required to produce 1.0 L of CH3OH (d = 0.791 g/mL) if this reaction has a 74% yield under certain conditions?

Interpretation Introduction

Interpretation:

It should be determine that the mass of H2 required to produce 1.0L of CH3OH if the reaction has 74% yield.

Concept introduction:

• The relation between the number of moles and mass of the substance is ,

Numberofmole=MassingramMolarmass

Massingramofthesubstance=Numberofmole×Molarmass

• 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 written in accordance with the Law of conservation of mass.
• Law of conservation of mass states that for a reaction total mass of the reactant and product must be equal.
• Stoichiometric factor is a relationship between reactant and product which is obtained from the balanced chemical equation for a particular reaction.
• Amountof substance=Concentrationofsubstance×volumeofthesubstance
• Mass=Density×Volume
• Theoretical yield is the maximum product yield that can be expected on the masses of the reactants and the reaction stoichiometry.
• Mass percent of elements of a compound is the ratio of mass of element to the mass of whole compound and multiplied with hundred.
Explanation

Balanced chemical equation for the given reaction is,

CO(g)+2H2(g)CH3OH(l)

From the balanced chemical equation it is clear that CH3OH and H2 react in a 1:2ratio.

The mass of CH3OH involved in this reaction is 791g it is obtained by using the equation Mass=Density×Volume

From the mass percent of reaction actual mass of CH3OH involved in this reaction can be calculated as follows,

791g is 74% of the theoretical yield of the reaction.

So,

74%×Theoreticalyield=791g

Theoreticalyield=791g0

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