Fill in the coefficients you get from balancing the the reaction below using the half-reaction method. Be sure you simplify all the coefficients into the smallest whole number ratios for this final answer (i.e.- Standard Form). If the substance does not appear in the final equation put a "0" for the coefficient and don't forget to place a "1" in the spaces where the coefficient of 1 goes. If you leave the space blank it will be marked incorrect. (Reaction j) MnO4 (aq) + C6H5CH3(aq) + H20(1) + H*(aq) <> .----- C6H,CO2(aq) + Mn2*(aq) + H2O(1) + H*(aq)
Fill in the coefficients you get from balancing the the reaction below using the half-reaction method. Be sure you simplify all the coefficients into the smallest whole number ratios for this final answer (i.e.- Standard Form). If the substance does not appear in the final equation put a "0" for the coefficient and don't forget to place a "1" in the spaces where the coefficient of 1 goes. If you leave the space blank it will be marked incorrect. (Reaction j) MnO4 (aq) + C6H5CH3(aq) + H20(1) + H*(aq) <> .----- C6H,CO2(aq) + Mn2*(aq) + H2O(1) + H*(aq)
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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![Fill in the coefficients you get from balancing the reaction below using the half-reaction method. Be sure you simplify all the coefficients into the smallest whole number ratios for this final answer (i.e., Standard Form).
If the substance does not appear in the final equation put a "0" for the coefficient and don't forget to place a "1" in the spaces where the coefficient of 1 goes. If you leave the space blank it will be marked incorrect.
(Reaction j)
\[ \square \] \( \text{MnO}_4^-(\text{aq}) \) + \[ \square \] \( \text{C}_6\text{H}_5\text{CH}_3(\text{aq}) \) + \[ \square \] \( \text{H}_2\text{O}(\text{l}) \) + \[ \square \] \( \text{H}^+(\text{aq}) \rightarrow \)
\[ \square \] \( \text{C}_6\text{H}_6\text{CO}_2(\text{aq}) \) + \[ \square \] \( \text{Mn}^{2+}(\text{aq}) \) + \[ \square \] \( \text{H}_2\text{O}(\text{l}) \) + \[ \square \] \( \text{H}^+(\text{aq}) \)
Note: In the above reaction scheme, blank boxes indicate where students should fill in the appropriate coefficients to balance the reaction correctly.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2e28c3ed-054a-4ef0-ab65-829683c00322%2F8405ab23-1107-4163-8f85-026ce2e359e9%2Fctr3hi_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Fill in the coefficients you get from balancing the reaction below using the half-reaction method. Be sure you simplify all the coefficients into the smallest whole number ratios for this final answer (i.e., Standard Form).
If the substance does not appear in the final equation put a "0" for the coefficient and don't forget to place a "1" in the spaces where the coefficient of 1 goes. If you leave the space blank it will be marked incorrect.
(Reaction j)
\[ \square \] \( \text{MnO}_4^-(\text{aq}) \) + \[ \square \] \( \text{C}_6\text{H}_5\text{CH}_3(\text{aq}) \) + \[ \square \] \( \text{H}_2\text{O}(\text{l}) \) + \[ \square \] \( \text{H}^+(\text{aq}) \rightarrow \)
\[ \square \] \( \text{C}_6\text{H}_6\text{CO}_2(\text{aq}) \) + \[ \square \] \( \text{Mn}^{2+}(\text{aq}) \) + \[ \square \] \( \text{H}_2\text{O}(\text{l}) \) + \[ \square \] \( \text{H}^+(\text{aq}) \)
Note: In the above reaction scheme, blank boxes indicate where students should fill in the appropriate coefficients to balance the reaction correctly.
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