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A student carried out the following precipitation reaction: BaCl₂(aq) + Na₂CO3(aq) BaCO3(s) + 2NaCl(aq) After no more precipitate appeared to form, he filtered the barium carbonate solid and then immediately weighed it. Using this mass, he calculated the percent yield as 105%. Is this possible? Explain.

A student carried out the following precipitation reaction: BaCl₂(aq) + Na₂CO3(aq) BaCO3(s) + 2NaCl(aq) After no more precipitate appeared to form, he filtered the barium carbonate solid and then immediately weighed it. Using this mass, he calculated the percent yield as 105%. Is this possible? Explain.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A student carried out the following precipitation reaction: \[ \text{BaCl}_2(aq) + \text{Na}_2\text{CO}_3(aq) \longrightarrow \text{BaCO}_3(s) + 2\text{NaCl}(aq) \] After no more precipitate appeared to form, he filtered the barium carbonate solid and then immediately weighed it. Using this mass, he calculated the percent yield as 105%. Is this possible? Explain.
Transcribed Image Text:A student carried out the following precipitation reaction: \[ \text{BaCl}_2(aq) + \text{Na}_2\text{CO}_3(aq) \longrightarrow \text{BaCO}_3(s) + 2\text{NaCl}(aq) \] After no more precipitate appeared to form, he filtered the barium carbonate solid and then immediately weighed it. Using this mass, he calculated the percent yield as 105%. Is this possible? Explain.
Expert Solution
Introduction

Percent yield is defined as the ratio of actual yield to that of theoretical yield whole multiplied by 100. 

The percent yield shows the efficiency of any reaction. 

better the percent yield, more amount of product we will get. 

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