Multiple Choice
Given the rate law rate = [p]^2[g][o], what is the overall order of the reaction?
15. Chemical Kinetics
Rate Law
Back15. Chemical Kinetics
Rate Law
- Multiple ChoiceGiven the following elementary steps: Step 1: A + B → C + D (fast) Step 2: C + B → D (slow), what is the overall rate law for the reaction?
- Multiple ChoiceWhat are the units for the rate constant k in a reaction with the rate law: rate = k[a][b]?
- Multiple ChoiceConsidering the rate law for the reaction 2NO + O2 → 2NO2, which of the following could be a possible rate law expression?
- Multiple ChoiceWhich of the following statements about the rate constant (k) in a chemical reaction is true?
- Multiple ChoiceConsidering the rate law, rate = k[a]^2[b], which of the following statements is correct?
- Multiple ChoiceWhich of the following best describes the difference between the rate of a reaction and its rate constant?
- Multiple ChoiceBased on the given two-step mechanism for the formation of 2NO2(g) from NO(g) and O2(g), what is the rate law for the overall reaction?
- Multiple ChoiceWhat is the rate law for the elementary reaction 2 HCl → H2 + Cl2?
- Multiple ChoiceWhat is the rate law for the following elementary reaction: ClO(g) + O(g) → Cl(g) + O2(g)?1views
- Open Question
Consider the rate law. rate=𝑘[a]𝑥 determine the value of 𝑥 if the rate doubles when [a] is doubled.
- Multiple ChoiceUsing the data below (also from questions 6 and 7), determine the value of the rate constant for the reaction.
Data Table for Three Experiments Experiment Initial [NH4+] Initial [NO2] Initial rate (M/s) Experiment 1 0.24 M 0.10 M 7.2 × 10-6 M/s Experiment 2 0.12 M 0.10 M 3.6 × 10-6 M/s Experiment 3 0.12 M 0.15 M 5.4 × 10-6 M/s - Multiple ChoiceFor the reaction 2 NOCl (g) → 2 NO (g) + Cl2 (g),the experimental rate law is: rate = k[NOCl]2[NO]-1
Determine if the following mechanism is valid.
Step 1: NOCl (g) ⇌ NO (g) + Cl (g) (fast)
Step 2: NOCl (g) + Cl (g) → NO (g) + Cl2 (g) (slow)
- Multiple ChoiceThe following reaction is first order: C2H6 → 2 CH3. If the rate constant is equal to 5.5 × 10⁻⁴ s⁻¹ at 1000 K, how long will it take for 0.35 mol of C2H6 in a 1.00 L container to decrease to 0.10 mol in the same container?
- Multiple ChoiceWhich of the following correctly matches the integrated rate law for a simple second-order reaction (where the rate depends on the concentration of a single reactant A)?