1) Methanol can be produced by the following reaction:(adsbygoogle = window.adsbygoogle || []).push({});

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.

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# Homework Help: Reaction Rate and Activation Energy

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