To what temperature would the reaction below need to be heated to have a rate constant of 2.091e9 M-1s-1 if the rate constant was 1.0800e9 M-1s-1 at -78.00°C and the activation energy was 11.900 kJ/mol? NO(g) + O3(g) ↔ NO2(g) + O2(g)

For the formation of 1 mol of nitrosyl chloride at a given temperature, H = –44 kJ.NO(g) + ½ Cl2(g)  NOCl(g)The activation energy for this reaction is 59 kJ/mol. What is the activation energy for the reverse reaction? A) 59 kJ/molB) 15 kJ/molC) 103 kJ/molD) –44 kJ/molE) –103 kJ/mol

At a given temperature, the elementary reaction A↽−−⇀B,A↽−−⇀B, in the forward direction, is first order in AA with a rate constant of 0.0220 s−1.0.0220 s−1. The reverse reaction is first order in BB and the rate constant is 0.0840 s−1.0.0840 s−1. What is the value of the equilibrium constant for the reaction A↽−−⇀BA↽−−⇀B at this temperature? ?=K=     What is the value of the equilibrium constant for the reaction B↽−−⇀AB↽−−⇀A at this temperature? ?=

Which of the following reactions is impossible to occur as a single step? Cl2(g) --> 2 CI(g) OCI + H20(1) --> HOCI(aq) + OH NO(g) + Cl2(g) NOCI2(g) --> O 2 NO(g) + O2(g) 2 NO2(g) -->