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Question- Understanding the high-temperature behavior of nitrogen oxides is essential for controlling pollution generated in automobile engines. The decomposition of nitric oxide (NO) to N2 and O2 is second order with a rate constant of 0.0796 M^-1s^-1 at 737 degrees C and 0.0815 M ^-1s^1 at 947 degrees C.
Calculate the activation energy for the reaction.
Any help is greatly appreciated! Anyone can tell me how to solve it step by step so that I will be able to understand what is going on
At equilibrium the total pressure was 1.00 atm and the NOCl prssure was 0.27 atm. 2NOCl(g) &hArr 2NO(g) + Cl2(g) Calculate the partial pressure of NO and Cl2 in the system
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