did i do this correct? Given the balanced reaction, initial GRAMS of each reactant and product, and the molar masses of each species complete the remainder of the change and final rows, in GRAMS.**NOTE:** Report all masses with ONE DECIMAL PLACE and be sure to include + and - signs with numerical values with NO SPACES.\[ 2 \, \text{C}_2\text{H}_6 \, (\text{g}) + 7 \, \text{O}_2 \, (\text{g}) \rightarrow 4 \, \text{CO}_2 \, (\text{g}) + 6 \, \text{H}_2\text{O} \, (\text{g}) \]| | \(\text{C}_2\text{H}_6\) | \(\text{O}_2\) | \(\text{CO}_2\) | \(\text{H}_2\text{O}\) ||---------------------------|--------------------------|----------------|----------------|------------------|| **(MM = 30.07 g/mol)** | **(MM = 32.00 g/mol)** | **(MM = 44.01 g/mol)** | **(MM = 18.02 g/mol)** || **Initial Grams** | 10.0 | 10.0 | 0.0 | 0.0 || **Change Grams** | -2.68 | -10 | 7.85 | 4.82 || **Final Grams** | 7.32 | 0 | 7.85 | 4.82 |This table provides information on the initial, change, and final masses of each species involved in the reaction. The molar masses (MM) are given for each compound to aid in calculating the changes in mass. The initial grams represent the starting amounts of each reactant, while the change grams show whether there is a gain or loss during the reaction. The final grams reflect the amounts present after the reaction is complete.

The stoichiometry of the balanced chemical equation states that two moles of C2H6 react with seven…

Given the balanced reaction, initial GRAMS of each reactant and product, and the molar masses of each species complete the remainder of the change and final rows, in GRAMS. NOTE: Report all masses with ONE DECIMAL PLACE and be sure to include + and- signs with numerical values with NO SPACES. 2 C2H6 (g) + 7 02 (g) ---> 4 CO2 (g) + 6 H,0 (g) C2H6 O2 H2O CO2 (MM = 30.07 (MM = 32.00 (MM = 18.02 (MM - 44.01 g/mol) g/mol) g/mol) g/mol) Initial Grams 10.0 10.0 0.0 0.0 -10 7.85 4.82 Change Grams -2.68 Final Grams 7.32 7.85 4.82

Given the balanced reaction, initial GRAMS of each reactant and product, and the molar masses of each species complete the remainder of the change and final rows, in GRAMS. NOTE: Report all masses with ONE DECIMAL PLACE and be sure to include + and- signs with numerical values with NO SPACES. 2 C2H6 (g) + 7 02 (g) ---> 4 CO2 (g) + 6 H,0 (g) C2H6 O2 H2O CO2 (MM = 30.07 (MM = 32.00 (MM = 18.02 (MM - 44.01 g/mol) g/mol) g/mol) g/mol) Initial Grams 10.0 10.0 0.0 0.0 -10 7.85 4.82 Change Grams -2.68 Final Grams 7.32 7.85 4.82

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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Question

did i do this correct?

Given the balanced reaction, initial GRAMS of each reactant and product, and the molar masses of each species complete the remainder of the change and final rows, in GRAMS.

**NOTE:** Report all masses with ONE DECIMAL PLACE and be sure to include + and - signs with numerical values with NO SPACES.

\[ 2 \, \text{C}_2\text{H}_6 \, (\text{g}) + 7 \, \text{O}_2 \, (\text{g}) \rightarrow 4 \, \text{CO}_2 \, (\text{g}) + 6 \, \text{H}_2\text{O} \, (\text{g}) \]

| | \(\text{C}_2\text{H}_6\) | \(\text{O}_2\) | \(\text{CO}_2\) | \(\text{H}_2\text{O}\) |
|---------------------------|--------------------------|----------------|----------------|------------------|
| **(MM = 30.07 g/mol)** | **(MM = 32.00 g/mol)** | **(MM = 44.01 g/mol)** | **(MM = 18.02 g/mol)** |
| **Initial Grams** | 10.0 | 10.0 | 0.0 | 0.0 |
| **Change Grams** | -2.68 | -10 | 7.85 | 4.82 |
| **Final Grams** | 7.32 | 0 | 7.85 | 4.82 |

This table provides information on the initial, change, and final masses of each species involved in the reaction. The molar masses (MM) are given for each compound to aid in calculating the changes in mass. The initial grams represent the starting amounts of each reactant, while the change grams show whether there is a gain or loss during the reaction. The final grams reflect the amounts present after the reaction is complete.

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