The date below are for the reaction of NO and `Cl_2` to form NOCl at 295K.

Calculate the rate constant.

The date below are for the reaction of NO and Cl_2 to form NOCl at 295K. Write the rate expression?

The date below are for the reaction of NO and Cl_2 to form NOCl at 295K. Determine the reaction rate when the concentrations of Cl_2 and NO are 0.2M and 0.4M respectively?

The date below are for the reaction of NO and Cl_2 to form NOCl at 295K. What is the order w.r.t. NO of Cl_2 in the reaction.

Write the reactions of F_2 and Cl_2 with water.

For the reaction: 2A + B rarr A_2B the rate = k[A][B]^2 with k = 2.0xx10^-6 mol^-2 L^2 s^-1 . Calculate the initial rate of the reaction when [A] = 0.1 mol L^-1 , [b] = 0.2 mol L^-1 . Calculate the rate of reaction after [A] is reduced to 0.06 mol L^-1 .

Nitrogen pentoxide decomposes according to equation 2N_2O_5(g) rarr 4NO_2(g) + O_2(g) The first order reaction was allowed to proceed at 40^@C and the data below were collected . Calculate the rate constant, include units with you answer.

In a first order reaction, the concentration of the reactant is reduced from 0.6moll^(-1) to 0.2moll^(-1) in 5 minutes. Calculate the rate constant of the reaction.

Time required to decompose SO_2Cl_2 to half of its initial amount is 60 minutes. If the decomposition is a first order reaction, calculate the rate constant of the reaction.

For the conversion of 1 mole of SO_2(g) to SO_3(g) the heat of reaction at constant volume ( Delta U^@ ) at 298K is -97.027 KJ Calculate the enthalpy change ( Delta H^@ )

The rate of reaction triples when temperature change from 20^@C to 50^@C . Calculate the energy of activation. (R = 8.314 Jmol^-1K^-1)