Given the reaction below the following kinetic data is obtained. 2NO(g)+Cl2(g)2NOCl(g) Determine the values of m and n in the rate law, rate =k[NO]m[Cl2]n Once you have determined the rate law use those values of m and n to calculate the value of k. For the reaction below calculate Kc if [NO(g)]=2.0M,[H2O(g)]=0.5M[NH3(g)]=1.0 M and [O2(g)]=0.50M 4NH3(g)+5O2(g)4NO(g)+6H2O(g) 0.5 2 4 8 For the reaction A+BC with a rate law that is second order in B. , If the concentration of A doubles does the rate change? What is the reaction order in terms of A ? Which of the following expressions relates the equilibrium constants for the two reaction below? A+1/2BC2C2A+BK1K2 K2=(K1)2(K2)2=K1K2=1/(K1)2K2=1/K1