Question

The rate of decomposition of hydrogen peroxide is first order in h2o2. at [h2o2] = 0.150 m, the decomposition rate was measured to be 4.83 × 10–6 m•s –1 . what is the rate constant for the reaction

Answer 1

The rate constant for the first-order decomposition of hydrogen peroxide at a concentration of 0.150 M and a decomposition rate of 4.83 × 10⁻⁶ M•s⁻¹ is calculated to be 3.22 × 10⁻⁵ s⁻¹.

Step-by-step explanation:

The rate of decomposition of hydrogen peroxide, which is first-order in H2O2, can be described using the rate law equation: rate = k [H2O2], where k is the rate constant, and [H2O2] is the concentration of hydrogen peroxide. Given that the rate of decomposition is 4.83 × 10⁻⁶ M•s⁻¹ at a concentration of 0.150 M, we can calculate the rate constant k by rearranging the rate law to k = rate / [H2O2]. Plugging in the numbers, k = (4.83 × 10⁻⁶ M•s⁻¹) / (0.150 M), which equals 3.22 × 10⁻⁵ s⁻¹.

Answer 2

If the decomposition of H2O2 is first order, then rate=k*[H2O2], and k=rate/[H2O2] In this case k=(4.83 x 10-6 M/s)/(0.15 M) k=3.22 x 10-5 s^-1