Would like a detailed explanation with work on each problem so I can understand how to do these problems.

The activation energy for a exothermic reaction is 130,357J. The reaction is initially run at 284K. What temperature does the reaction need to be increased to in order to increase the rate constant by 100x ? Question 2 2 pts The decomposition of A2B5 (shown below) follows first order kinetics. If the half life at 27.90C is 799 s how long will it take for 34.9% of the A2B5 to decompose? 3A2B56AB2+B3 Question 3 2pts 0.0947 moles of NO2 gas is placed in a 500. ml flask which is then closed. At equilibrium, it is found that the flask contains 4.00103 moles of N2O4 gas. The equilibrium reaction is: 2NO2(g)N2O5(g). Using an ICE table, determine the equilibrium constant for this reaction. Question 4 2pts The pressure equilibrium constant for CO(g)+2H2(g) CH3OH is Kp=2.26104 at 298K. Calculate Kp1/2CH3OH1/2CO(g)+H2(g)