**Hydrogen Gas Reduces NO to N₂ in the Reaction:**\[ 2H_2(g) + 2NO(g) \rightarrow 2H_2O(g) + N_2(g) \]The initial reaction rates of four mixtures of $ H_2 $ and $ NO $ were measured at 1500°C with the following results:| Experiment | $[H_2]_0 $ (M) | $[NO]_0 $ (M) | Initial Rate (M/s) ||------------|------------------|-----------------|--------------------|| 1 | 0.212 | 0.136 | 0.0393 || 2 | 0.212 | 0.272 | 0.0789 || 3 | 0.424 | 0.544 | 0.624 || 4 | 0.848 | 0.544 | 2.50 | ### Instructions for Calculating Rates**Answer these using the table:**#### Part 3- **Rate 3:** ______ molecules/(cm³·s)#### Part 4- **Rate 4:** ______ molecules/(cm³·s)**Note:** Use the provided table to fill in the blanks for the rates specified above.

Recall the given equation 2H2g + 2NOg⇔2H2Og + N2 Let order of reaction with respect to H2 is x and order of reaction with respect to NO is y So, rate law of this reaction is as follows Rate=KH2xNOy K is rate constant of this reaction. we have to find rate of this reactionSubstitute above expression with given values 0.0393 M/s=K0.212 Mx0.136 My .....(1)0.0789 M/s=K0.212 Mx0.272 My .....(2) 0.624 M/s=K0.424 Mx0.544 My .....(3) 2.5 M/s=K0.848 Mx0.544 My ......(4) Divide equation (2) by equation (1)0.0789 M/s0.0393 M/s=K0.212 Mx0.272 My K0.212 Mx0.136 My 2=2y Hence, y=1So, order of reaction with respect to NO is 1 Again divide equation (3) by equation (1)0.624 M/s0.0393 M/s=K0.424 Mx0.544 My K0.212 Mx0.136 My 15.9=2x4yAs, y=1, So,15.9=2x4 2x=3.98 x≈2So, order of reaction with respect to H2 is 2 Now find value of rate constant from equation (1) 0.0393 M/s=K0.212 M2×0.136 M1 K=6.43 M-2.s-1 Now find Rate 3 Rate=6.43 M-2.s-1×0.424 M2×0.544 M1 =0.629 M/s =0.629 molL.s =0.629 molL.s×6.022×1023 molecules1 mol×1 L1000 cm3 =3.789×1020 molecules/(cm3.s) Now find Rate 4 Rate=6.43 M-2.s-1×0.848 M2×0.544 M1 =2.515 M/s =2.515 molL.s =2.515 molL.s×6.022×1023 molecules1 mol×1 L1000 cm3 =1.515×1021 molecules/(cm3.s)

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Hydrogen gas reduces NO to N2 in the following reaction: 2H, (g) + 2NO(g) 2H,0(g) +N2 (g) The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results: Experiment [H2]o (M) [NO]o (M) Initial Rate (M/s) 1 0.212 0.136 0.0393 0.212 0.272 0.0789 3 0.424 0.544 0.624 4 0.848 0.544 2.50

Hydrogen gas reduces NO to N2 in the following reaction: 2H, (g) + 2NO(g) 2H,0(g) +N2 (g) The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results: Experiment [H2]o (M) [NO]o (M) Initial Rate (M/s) 1 0.212 0.136 0.0393 0.212 0.272 0.0789 3 0.424 0.544 0.624 4 0.848 0.544 2.50

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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Hydrogen gas reduces NO to N2 in the following reaction: 2H, (g) + 2NO(g) 2H,0(g) + N, (g) The initial reaction rates of four mixtures of H, and NO were measured at 1500°C with the following results: Experiment [H2]o (M) [NO]o (M) Initial Rate (M/s) 0.212 0.136 0.0393 2 0.212 0.272 0.0789 0.424 0.544 0.624 0.848 0.544 2.50 4.
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