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. 4 NH,(g) + 50,(g)-4 NO(g) + 6 H,0(g) a. Calculate the average rate of reaction with respect to NH,. b. Calculate the average rate at which H,0 is being formed. c. Calculate the average rate at which O, is being consumed. (answer + units for NH) (answer + units for H,0) (answer + units for O)

Consider the following reactions: + O2(e) + O2(8) + 2H* → 2NO(8) → 2MgO(s) I. II. N2e) Mg(s) (aq) > Ca2+ Increasing the surface area will increase the reaction rate in: II. CaCO3(s) + H2Ou + CO2(8) (aq) А. Il only В. I and III only C. Il and III only D. I, II, and III

When given a chemical equation, how may I find the rate expression, concentration, average reaction rate, mols, and mass?

b. On the same diagram, draw a dashed line to indicate the changes that result from the addition of the catalyst. Explain the role of the catalyst in changing the rate of the reaction. 11. Given the following initial rate data: каза гази Rate (mole/Los) 1,350 12 TI T2 13,500 T3 54,000 a. What is the rate expression for the reaction? b. What is the value for k and its units? [A] .20 .50 .50 [B] .30 .60 1.2 c. What would happen to the rate if both the concentrations of A and B were doubled? 12. Consider a reaction of the form 2A + BC. The data for this reaction is given below: Initial rate of formation of C M/s Initial [A] Initial [B]

Arrange the following reactions in order of increasing rate (slowest to fastest) i. CzsHs2 (s) + 38 O2 (8) → 5 CO2 (g) + 26 H20 () ii. Ag* (aq) + I'(aq) > Agl (s) iii. H2 (g) + % O2 (8) → H20 a. i, ii, ii b. iii, ii, i c. ii, i, ii d. ii, i, iii e. ii, ii, i

The rate of a certain reaction was studied at various temperatures. The table shows temperature (7) and rate constant (k) data collected during the experiments. Plot the data to answer the questions. What is the value of the activation energy, Ea, for this reaction? E₂ = What is the value of the pre-exponential factor (sometimes called the frequency factor), A, for this reaction? A = kJ. mol-¹ $ $1 T(K) 400 420 440 460 480 500 520 540 560 580 k (s-¹) 0.000369 0.00200 0.00928 0.0377 0.136 0.445 1.33 3.64 9.31 22.3

The rate constant for the first-order decomposition of N2O5(g) to NO2(g) and O2(g) is 7.48 × 10-3 s-1 at a given temperature. Initially, the system only contains N2O5 at an initial pressure of 0.100 atm. a. Write a balanced chemical equation for this reaction. b. Find the total pressure after 100 s of the reaction.

1c

8. a) Starting from the rate law for the second order reaction below, derive the relationship between half- life, rate constant, and initial concentration. 2A → B 8. b) Draw the potential energy diagrams (qualitatively) for the following reaction mechanisms. Assume that all intermediates are higher energy than their respective reactant states, and that the product state is lower in energy than the reactant state. Mechanism 1: 03 + NO → 02 + NO3 (slow) 0 + 03 → 2 02 (fast) NO3 + NO → 2 NO2 (fast) Mechanism 2: 03 2 02 +0 (fast) NO + 0 → NO2 (slow) Mechanism 3: 03 + NO → 02 + NO2 (slow)