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If the rate constant for a reaction is 2.86s1 at 20C and the activation energy is 22.3kJ/mol, then what is the rate at 0C ? k= If the rate constant for a reaction is 2.86s1 at 20C and the activation energy is 36.2kJ/mol, then at what temperature will the rate constant be decreased to half its original value? T= For the elementary reaction: 2B+C products i) the molecularity would be: a) zero b) one c) two -d) three e) undefined ii) the rate law would be: a) rate =k[B][C] b) rate =k[B][C]2 c) rate =k[B]2[C] d) undefined The expression, rate =k[A]2[B]2, would suggest which of the following steps to be the rate determining step in the overall reaction? step1step2step3overall:A+BC+BD+A2A+2BCD+Eproductsproducts