Brun

Nitric oxide (NO) can be removed from gas-fired power-plant emissions by reaction with methane as follows: CH4(g) + 4NO(g) --> 2N2(g) + CO2(g) + 2H2O(g) Complete the equation relating the rates for each of the following: a) the rate of appearance of N2 to...

Posted by Brunette on Sunday, October 14, 2012 at 10:42pm. Values of the rate constant for the decomposition of N2O5 at four different temperatures are as follows: T(K) k(s^-1) 658....2.14*10^5 673....3.23*10^5 688....4.81*10^5 703....7.03*10^5 The activa...

calculate the value of the equilibrium constant K for this reaction A+B <--> C from the following information 3C <--> D Kc= 7.1*10^-4 D <--> 3A + 3B Kc= 2.9*10^-2

The equilibrium constant Kp for the following equilibrium is 33 at 298 K. What is the value of Kc at this same equilibrium at 298 K

At 860.0 deg celsius, the equilibrium constant Kp for the synthesis of ammonia (below) is 3.35 * 10^-5. What is the value of Kc? N2(g) + 3H2(g) <--> 2NH3(g)

Oh! Thank you! I forgot to pick a second temperature.

they are saying that the d[CO2] for the d[CO2]/dT is wrong but I'm not sure why.