**Question:**If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 5.5 mol of NO₂ were collected, then what is the percent yield for the reaction?2 NO (g) + O₂ (g) → 2 NO₂ (g)**Explanation:**This question examines the concept of percent yield in chemical reactions. Percent yield is calculated using the formula:\[\text{Percent Yield} = \left(\frac{\text{Actual Yield}}{\text{Theoretical Yield}}\right) \times 100\%\]- **Theoretical Yield Calculation:** Using stoichiometry, 10.0 moles of O₂ could theoretically produce 20.0 moles of NO₂, considering the reaction 2 NO + O₂ → 2 NO₂.- **Actual Yield:** The actual amount of NO₂ collected is 5.5 moles. **Solution:**1. Calculate the theoretical yield of NO₂ based on O₂ as the limiting reactant.2. Use the percent yield formula to find the answer.**Calculator Interface:**The image has a calculator interface on the right side with numbers (1-9, 0), arithmetic symbols, and a 'percent' button, presumably to assist in carrying out the calculation electronically.

The given reaction is as follows: 2NO(g) + O2(g)------->2NO2(g) The moles of O2 reacting, = 10…

Answered: If 10.0 moles of O: are reacted with…

If 10.0 moles of O: are reacted with excess NO in the reaction below, and only 5.5 mol of NO2 were collected, then what is the percent yield for the reaction? 2 NO (g) + O2 (g)→2 NO2 (g)

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

Expert Solution

Step 1

The given reaction is as follows:

2NO(g) + O₂(g)------->2NO₂(g)

The moles of O₂ reacting, = 10 moles.

The moles of NO₂ formed = 5.5 moles.

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