1) Methanol can be produced by the following reaction: CO (g) + 2H2 (g) --> CH30H (g) How is the rate of disappearance of hydrogen gas related to the rate of appearance of methanol? -delta[H2]/delta t = ? a. + delta [H2]/delta t b. + 1delta[CH3OH]/2delta t c. + 2 delta [CH3OH]/delta t d. none of the above Is it d because the rates are supposed to be determined experimentally? 2) The first order isomerization of cyclopropane -> propene has a rate constant of 0.00026 1/sec at 435 Celsius with an activation energy of 264 kJ/mol. What is the temperature at which the rate constant is 0.00447 1/sec? Calculate your answer in kelvins. k2 = 0.00447 1/s k1 = 0.00026 1/s T1 = 435 C = 708.15 K E_a = 264 kJ/mol = 2640 J/mol ln (k2/k1) = (-E_a/R)*[(1-T2) - (1/T1)]???? 1/T2 = [-ln (k2/k1)/(-E_a/R)] + (1/T1) 1/T2 = -ln(0.00447/.00026)/[-2640 J/mol/(8.314)] + (1/708.15 K) =0.0096133567 + (1/708.15 K) = 0.011025 1/0.011025 = 90.69 K = 90.7 K??? Is the correct final answer and method? Thank you.