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When 12 g of methanol (CH3OH) was treated with excess MnO4, 14 g of formic acid (HCOOH) was obtained. Calculate the percent yield. Note: This equation cannot be balanced as is because other things more complicated are happening. Use the reaction as it is shown below: 3CH3OH + 4MNO4 3HCOOH + 4MNO2

When 12 g of methanol (CH3OH) was treated with excess MnO4, 14 g of formic acid (HCOOH) was obtained. Calculate the percent yield. Note: This equation cannot be balanced as is because other things more complicated are happening. Use the reaction as it is shown below: 3CH3OH + 4MNO4 3HCOOH + 4MNO2

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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When 12 g of methanol (CH₃OH) was treated with excess MnO₄⁻, 14 g of formic acid (HCOOH) was obtained. Calculate the percent yield. Note: This equation cannot be balanced as is because other things more complicated are happening. Use the reaction as it is shown below: \[3\text{CH}_3\text{OH} + 4\text{MnO}_4^- \rightarrow 3\text{HCOOH} + 4\text{MnO}_2\] - ( ) 100% - ( ) 92% - ( ) 70% - ( ) 82% - ( ) 55% - ( ) 32.61% - ( ) none of these are correct
Transcribed Image Text:When 12 g of methanol (CH₃OH) was treated with excess MnO₄⁻, 14 g of formic acid (HCOOH) was obtained. Calculate the percent yield. Note: This equation cannot be balanced as is because other things more complicated are happening. Use the reaction as it is shown below: \[3\text{CH}_3\text{OH} + 4\text{MnO}_4^- \rightarrow 3\text{HCOOH} + 4\text{MnO}_2\] - ( ) 100% - ( ) 92% - ( ) 70% - ( ) 82% - ( ) 55% - ( ) 32.61% - ( ) none of these are correct
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