What are the units for the rate constant k in a reaction with the rate law: rate = k[a][b]?

Given the following data for the reaction A + B → products: | [A] (mol/L) | [B] (mol/L) | Initial Rate (mol/L·s) | |-------------|-------------|------------------------| | 0.10 | 0.10 | 0.020 | | 0.20 | 0.10 | 0.040 | | 0.10 | 0.20 | 0.040 | Assuming the rate law is rate = k[A][B], what is the value of the rate constant k (in L/mol·s)?

Considering the rate law, rate = k[a]^2[b], which of the following statements is correct?

Given the reaction a → b, if the rate constant k is 0.25 mol L^{-1} s^{-1} at 75 °C and the reaction is first order in a, what is the correct rate law for this reaction?

For the reaction x + 2 y → xy₂, if the reaction occurs in a single elementary step as proposed, what is the correct rate law?

What is the overall reaction order for the following rate law: rate = k[a][b][c]?

Using the information in the table below, determine the rate law for the reaction: a(g) + 3 b(g) → c(g) + 2 d(g). | Experiment | [a] (M) | [b] (M) | Initial Rate (M/s) | |------------|--------|--------|--------------------| | 1 | 0.10 | 0.10 | 0.020 | | 2 | 0.20 | 0.10 | 0.040 | | 3 | 0.10 | 0.20 | 0.080 | Which of the following is the correct rate law?

Using the information in the table below, what is the correct rate law for the reaction 2 A(g) + B(g) → C(g) + D(g)? | Experiment | [A] (M) | [B] (M) | Initial Rate (M/s) | |------------|--------|--------|--------------------| | 1 | 0.10 | 0.10 | 2.0 × 10^{-3} | | 2 | 0.20 | 0.10 | 4.0 × 10^{-3} | | 3 | 0.10 | 0.20 | 2.0 × 10^{-3} | Which of the following is the correct rate law?

Which of the following expressions correctly represents the rate constant, k, for a first-order reaction with respect to its half-life, t_{1/2}?