What is the rate law for the reaction A → B if the rate constant, k, is 0.25 m^-1 s^-1 at 75 °C?

According to this data, what is the order of the reaction in OH^-, to the nearest whole number?

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

Consider the following reaction: 2 Mg + O₂ → 2 MgO, rate=k[Mg][O₂]²

If a rate law is second order (reactant), doubling the reactant ________ the reaction rate.

Consider the tabulated data showing the initial rate of a reaction (A → products) at several different concentrations of A. What is the order of the reaction? Write a rate law for the reaction including the value of the rate constant, k.

[A] (M) Initial Rate (M/s)

0.050 0.100

0.075 0.225

0.090 0.324