Chapter 5, Problem 82E

Interpretation Introduction

Interpretation: The percent yield of the given reaction is to be determined if the actual yield of ${\text{C}}_{\text{2}}{\text{H}}_{\text{6}}$ is $15\text{g}$ and volumes of ${\text{C}}_2{\text{H}}_4$ and ${\text{H}}_2$ are given as $\text{1000}\text{L/min}$ and $1500\text{L/min}$ respectively.

Concept introduction:

• Number of moles of a substance, According to ideal gas equation,

$\text{Number}\text{of}\text{moles}\text{=}\frac{\text{Pressure}\times \text{Volume}}{\text{R}\text{×}\text{Temperature}}$

• Mole ratios between the reactant and a product of a reaction are depends upon the coefficients of reactant and product in a balanced chemical equation.

• Limiting reagent: limiting reagent is a reactant, which consumes completely in the chemical reaction. The quantity of the product depends on this limiting reagent, it can be determined with the help of balanced chemical equation for the reaction.

• mass of a substance from its number of moles is,

$\text{Number of moles}\text{×}\text{Molecular}\text{mass in grams}\text{=}\text{produced}\text{mass}$

• Percent yield of reaction is the ratio of mass of actual yield to the mass of theoretical yield.