Need assistance on the formula of how to answer this **Part F**Calculate the grams of NO that would be produced.Express your answer with the appropriate units.\[ m(\text{NO}) = \, \text{Value} \, \text{Units} \][Submit] [Request Answer]---**Part G**Determine the limiting reactant, given 31.0 g of each reactant, in the following reaction:\[ \text{C}_2\text{H}_6\text{O}(l) + 3\text{O}_2(g) \rightarrow 2\text{CO}_2(g) + 3\text{H}_2\text{O}(g) \]---**Explanation:**The given equation calculates the moles of \(\text{HNO}_3\) formed:- \[31.0 \, \text{g} \, \text{H}_2\text{O} \times \frac{1 \, \text{mol} \, \text{H}_2\text{O}}{18.015 \, \text{g}} \times \frac{2 \, \text{mol} \, \text{HNO}_3}{1 \, \text{mol} \, \text{H}_2\text{O}} = 3.44 \, \text{mol} \, \text{HNO}_3\]Since the number of moles produced by NO\(_2\) is less, it is identified as the limiting reagent. Determine the limiting reactant, given 31.0 g of each reactant, in the following reaction:\[3NO_2(g) + H_2O(l) \rightarrow 2HNO_3(aq) + NO(g)\]Options for the limiting reactant:- NO- HNO₃- NO₂- H₂O---Correct Answer Explanation:To find the limiting reactant, use the 31.0 g of each reactant and calculate the amount of product formed by each reactant. The limiting reactant is the one that forms the least amount of product, as it will run out first. Either product can be used for this comparison. In this example, \(HNO_3\) is used.1. **Calculation for \(NO_2\):**\[\text{moles of } HNO_3 \text{ formed} = 31.0 \, \cancel{g \, NO_2} \times \frac{1 \, \cancel{mol \, NO_2}}{46.00 \, \cancel{g \, NO_2}} \times \frac{2 \, mol \, HNO_3}{3 \, \cancel{mol \, NO_2}} = 0.449 \, mol \, HNO_3\]2. **Calculation for \(H_2O\):**\[\text{moles of } HNO_3 \text{ formed} = 31.0 \, \cancel{g \, H_2O} \times \frac{1 \, \cancel{mol \, H_2O}}{18.015 \, \cancel{g \, H_2O}} \times \frac{2 \, mol \, HNO_3}{1 \, \cancel{mol \, H_2O}} = 3.44 \, mol \, HNO_3\]Since the number of moles produced by \(NO_2\) is less, \(NO_2\) must be the limiting reagent.

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Answered: Calculate the grams of NO that would be…

Calculate the grams of NO that would be produced. Express your answer with the appropriate units.

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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