5. For the reaction below, initially 3.5 mol of NH¸ are placed in a 4.0 L reaction chamber. After 3.0 minutes only 1.6 moles of NH, remain. SHOW ALL YOUR WORK. Rates should be in M/s 4 NH₂(g) + 5 0₂(g) → 4 NO(g) + 6 H₂0(g) a. Calculate the average rate of reaction with respect to NH ₂. b. Calculate the average rate at which H₂O is being formed. c. Calculate the average rate at which 0, is being consumed.

5. For the reaction below, initially 3.5 mol of NH¸ are placed in a 4.0 L reaction chamber. After 3.0 minutes only 1.6 moles of NH, remain. SHOW ALL YOUR WORK. Rates should be in M/s 4 NH₂(g) + 5 0₂(g) → 4 NO(g) + 6 H₂0(g) a. Calculate the average rate of reaction with respect to NH ₂. b. Calculate the average rate at which H₂O is being formed. c. Calculate the average rate at which 0, is being consumed.

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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The rate of the reaction NO₂(g) + CO(g) was determined in three experiments at 225°C. The results are given in the following table: 5th attempt Part 1 Rate law = NO(g) + CO₂(g) Part 2 Do not include spaces or multiplication signs in your answer. Determine the rate law for this reaction. Do not include states of matter or spaces in your answer. +. log. cos. d Experiment [NO2]o (M) [CO]o (M) Initial Rate -A[NO2]/At (M/s) 0.263 0.826 1.44x10-5 0.263 0.413 1.44x10-5 0.526 0.413 5.76x10-5 Part 3 1 2 3 Calculate the value of the rate constant at 225°C. M¹s-1 Calculate the rate of appearance of CO₂ when [NO₂] = [CO] = 0.550 M. x 10 M/s → See Periodic Table See Hint
7. For the set of elementary steps shown. Cl2 → 2 Cl (slow) a. Write the overall reaction equation. Cl+ C;H10 → HCI+C;H9 (fast) b. Identify the intermediates. C;H, + Cl → C,H,Cl (fast) c. Write the rate law for the overall reaction. 8. For the set of elementary steps shown. Step 1: H2(g) + IC1(g) → HI(g) + HCl(g) (slow) a. Write the overall reaction equation. Step 2: HI(g) + IC1(g) HCI(g) + I2(g) (fast) b. Identify the intermediates. c. Write the rate law for the overall reaction. 9. For the set of elementary steps shown... a. Write the overall reaction equation. Step 1: NO2 + F2 → NO,F + F (slow) Step 2: NO2 +F NO,F (fast) b. Identify the intermediates. c. Write the rate law for the overall reaction.
For the following reaction: N2 (g) + 3 H2 (g) → 2 NH3 (g) a. Give the relative rates of the above reaction based on the stoichiometry. b. Determine the rate of formation of NH3, if the rate of loss of H2 is 7.78 x 10-1 M/s.
A: Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3- --> 4 Zn2+ + N2O(g) + 5 H2O(l) What is the rate of Zn2+ formation if its concentration rises from 0.00 to 0.069 M in 2 minutes and 12 seconds? Group of answer choices 0.031 M/s 2.1 x 10-3 M/s 1.3 x 10-4 M/s 5.2 x 10-4 M/s B: Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3- --> 4 Zn2+ + N2O(g) + 5 H2O(l) If the rate of H+ disappearance is 0.0250 M/min, what is the rate of Zn2+ appearance? Group of answer choices 0.0100 M/min 0.00100 M/min 0.0250 M/min 0.0625 M/min
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5.00 mL 4.50 M acetone + 10.0 mL 1.15 M HCl + 10.0 mL 0.00200 M I2 + 25.0 mL H2O A student found that it took 146 seconds for the color of the I to disappear. a. What was the rate of the reaction? Hint: First find the initial concentration of Iz in the reaction mixture, [I2]o. Then use the equation Rate At t M/s b. Write the rate equation. (Abbreviate acetone to ace, H* ion to H", and iodine to I2. Represent the order of reaction with respect to acetone as m, the order of reaction with respect to iodine as n, and the order of reaction with respect to H* as p). c. Select all the unknown variables in the equation in part (b). Rate O[Ace] (Previous Next
1. A dimer is formed in the solution reaction of 2A → A2. The rate law is -ra = kCg where k is 0.015 M s. What is the half-life of A when the initial concentration is 0.05 M?
How would you find the rate law for this question?
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1. For an irreversible reaction A products, the graph of 1/[A] as a function of time is linear. What is the reaction order in A? a. Zeroth-order b. First-order c. Second-order d. The order in A cannot be determined based on the information given. 2. A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step 1: H₂(g) + 2 NO (g) → N₂O (g) + H₂O (g) Step 2: N₂O (g) + H₂ (g) → N2 (g) + H₂O (g) What is the molecularity of Step 2? a. unimolecular b. bimolecular c. termolecular d. zero molecular (spontaneous) e. More information is needed to answer this question. 3. Which one of the following will change the value of an equilibrium constant? a. changing temperature b. adding other substances that do not react with any of the species involved in the equilibrium c. varying the initial concentrations of reactants d. varying the initial concentrations of products e. changing the volume of the reaction vessel