The rate constant for the first-order decomposition at 45 °C of dinitrogen pentoxide, N2O5, dissolved in chloroform, CHCl3, is 6.2 × 10−4 min−1.2N2 O5 ⟶ 4NO2 + O2What is the rate of the reaction when [N2O5] = 0.40 M?

A certain first-order reaction has a rate constant of 2.50×10−3 s^−1. How long will it take for the reactant concentration to drop to 1/8 of its initial value?

A certain first-order reaction has a rate constant of 1.60×10−3 s−1. How long will it take for the reactant concentration to drop to 18 of its initial value?

The reaction described by H, (g) + L,(g) 2 HI(g) has an experimentally determined rate law of rate = k [H2] [I2] Some proposed mechanisms for this reaction are: Mechanism A k1 (1) H,(g) + L,(g) → 2 HI(g) (one-step reaction) Mechanism B k1 =2 I(g) k_1 (1) L(g) ; (fast, equilibrium) k2 (2) H, (g) + 2 I(g) 2 HI(g) (slow) Mechanism C k1 = 2 I(g) (fast, equilibrium) (1) k2 (2) I(g) + H, (g) HI(g) + H(g) (slow) (3) H(g) + I(g) → HI(g) (fast) Question Sourc

After 48 seconds, 10.% of reactant has reacted. If the reaction is a 1st order reaction, the special rate constant k = _.

Dinitrogen pentoxide, N2O5, decomposes by a first order reaction with an activation energy of 110 kJ/mol. At 65 °C, the rate constant is k = 5.2 x 10-3 s-1.