In calculating the percent yield in the picture, what must we assume about the amount of carbon present? 3. Carbon tetrachloride (CC14) can be produced using the following reaction. If 34.535 grams ofchlorine (Cl2) produced 28.550 g of CC14, what is the percent yield of this reaction?C(s) + 2 Cl2(g) CCI4(1)

Given: The reaction given is as follows: C(s) + 2Cl2(g) → CCl4(l) Also, given that 34.535 grams of…

Answered: 3. Carbon tetrachloride (CCI4) can be…

Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Chapter1: Introduction

Section: Chapter Questions

Problem 1.1P

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In calculating the percent yield in the picture, what must we assume about the amount of carbon present?

3. Carbon tetrachloride (CC14) can be produced using the following reaction. If 34.535 grams of
chlorine (Cl2) produced 28.550 g of CC14, what is the percent yield of this reaction?
C(s) + 2 Cl2(g) CCI4(1)

Expert Solution

Step 1

Given:

The reaction given is as follows:

$C (s) + 2 {Cl}_{2} (g) \to {CCl}_{4} (l)$

Also, given that 34.535 grams of Chlorine (Cl₂) reacts in the reaction to produce 28.550 gm of CCl₄.

Molecular weight of Chlorine (Cl₂) = 70.9 gm/mol

Molecular weight of CCl₄ = 153.8 g/mol

Note: Since the carbon is present in solid form, it should not be used in stoichiometric calculations. Also, the carbon content is not mentioned in the question.

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