I don't understand how to work a problem.What is the percent yield for the reaction below if 119.3 g of chromium metal is formed when 61.3g of carbon reacts with excess Cr2O3? 3) Practice M 4 table (1 reactant)What is the percent yield for the reaction below if 119.3 g of Chromium metal is formed when 61.3 g of Carbonreacts with excess Cr2O3?O BALANCED? 2 Cr203 (s)3c(s)4 Cr(s)3 Co2 (g)->mass (g)Molar Mass (g/mol)52molCoefficient3ratioPercent yieldWhy is the 1st column blacked out?Why is the Last column blacked out?4) Practice M 4 table (2 reactants):What is the theoretical yield of BOTH products when 100.0 g of Cr2O3 reacts with 100.0 g of C?

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don't understand how to work a problem. What is the percent yield for the reaction below if 119.3 g of chromium metal is formed when 61.3g of carbon reacts with excess Cr2O3?

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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I don't understand how to work a problem.

What is the percent yield for the reaction below if 119.3 g of chromium metal is formed when 61.3g of carbon reacts with excess Cr2O3?

3) Practice M 4 table (1 reactant)
What is the percent yield for the reaction below if 119.3 g of Chromium metal is formed when 61.3 g of Carbon
reacts with excess Cr2O3?
O BALANCED? 2 Cr203 (s)
3c(s)
4 Cr(s)
3 Co2 (g)
->
mass (g)
Molar Mass (g/mol)
52
mol
Coefficient
3
ratio
Percent yield
Why is the 1st column blacked out?
Why is the Last column blacked out?
4) Practice M 4 table (2 reactants):
What is the theoretical yield of BOTH products when 100.0 g of Cr2O3 reacts with 100.0 g of C?

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