By what factor does increasing the temperature of a reaction from T = 273 K to T = 283 K increase the rate of reaction? Assume the activation energy (E) of this reaction is 164,500 J and that the pre-exponential constant (A) is 2.1 x 10° s-1. Express your answer to one decimal place.

Given the following values of the enthalpy (DH) and activation energy (Ea) of four different reactions, identify an exothermic reaction that would exhibit the fastest rate at 298 K. (Assume that all reactants have the same initial concentration and the same Arrhenius frequency factor A in k = Ae-Ea/RT).   (A) DH = +45 kJ/mol;    Ea = 75 kJ/mol;             (B) DH = +35 kJ/mol;    Ea = 65 kJ/mol; (C) DH = -35 kJ/mol;     Ea = 75 kJ/mol; (D) DH = -45 kJ/mol;    Ea = 65 kJ/mol;

Consider the following elementary reaction: H,(9) +2NO(g) → N,0(g) +H,O(g) Suppose we let k, stand for the rate constant of this reaction, and k_, stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of H,O in terms of k, k_1, and the equilibrium concentrations of H, NO, and N,O. [H,0]= 0 %3D

The rate constant for a first-order reaction is 1.6  10–2s–1at 668 K and 5.1  10–2 s–1at 916 K. What is the activation energy? (R = 8.31 J/(mol · K))