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Ethene is converted to ethane by the reaction C 2 H 4 ( g ) + H 2 ( g ) → Catalyst C 2 H 6 ( g ) C 2 H 4 flows into a catalytic reactor at 25.0 atm and 300.°C with a flow rate of 1000. L/min. Hydrogen at 25.0 atm and 300.°C flows into the reactor at a flow rate of 1500. L/min. If 15.0 kg C 2 H 6 is collected per minute, what is the percent yield of the reaction?

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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Chapter
Section
BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 8, Problem 76E
Textbook Problem
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Ethene is converted to ethane by the reaction

C 2 H 4 ( g ) +   H 2 ( g ) Catalyst   C 2 H 6 ( g )

C2H4 flows into a catalytic reactor at 25.0 atm and 300.°C with a flow rate of 1000. L/min. Hydrogen at 25.0 atm and 300.°C flows into the reactor at a flow rate of 1500. L/min. If 15.0 kg C2H6 is collected per minute, what is the percent yield of the reaction?

Interpretation Introduction

Interpretation: The percent yield of the given reaction is to be determined if the actual yield of C2H6 is 15g and volumes of C2H4 and H2 are given as 1000L/min and 1500L/min respectively.

Concept introduction:

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

Numberofmoles=Pressure×VolumeR×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,

Number of moles×Molecularmass in grams=producedmass

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

Explanation of Solution

Explanation

The volume of C2H4 in the given reaction is given as 1000L/min .

The volume of H2 in the given reaction is given as 1500L/min .

The equation for finding number of moles of a substance, According to ideal gas equation,

Numberofmoles=Pressure×VolumeR×Temperature

The pressure, temperature and R-value are constant for both C2H4 and H2 in the given reaction.

Hence,

The pressure is taken as P .

The temperature is taken as T .

The value of R is taken as R .

Therefore,

In a minute,

The number of moles of C2H4 in the given reaction is,

nC2H4=1000PRTmol

The number of moles of H2 in the given reaction is,

nH2=1500PRTmol

The number of moles of C2H4 gas is 1000PRTmol/min .

The number of moles of H2 gas is 1500PRTmol/min .

The balance equation of given reaction is,

C2H4+H2C2H6

The 1 mole of C2H4 is reacting with 1 mole of H2 to produce 1 mole of C2H6 .

That means, the C2H4 and H2 are in 1:1 ratio.

Therefore,

In a minute,

The 1500PRTmolofH2 requires1500PRTmolofC2H4 .

The given number of moles of C2H4 gas is 1000PRTmol/min only.

Hence, C2H4 is the limiting reagent in the given reaction.

The balance equation of given reaction is,

C2H4+H2C2H6

The 1 mole of C2H4 is reacting with 1 mole of H2 to produce 1 mole of C2H6

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Chemistry: An Atoms First Approach
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