In the laboratory, you are studying the first-order conversion of a reactant to

Question

In the laboratory, you are studying the first-order conversion of a reactant to products in a reaction vessel with a constant volume of . At 1:00 p.m., you start the reaction at 23 with 1.000 of . At 2:00 p.m., you find that 0.600 of remains, and you immediately increase the temperature of the reaction mixture to 28. At 3:00 p.m., you discover that 0.250 of is still present. You want to finish the reaction by 4:00 p.m. but need to continue it until only 0.020 of remains, so you decide to increase the temperature once again.

Part A)

What is the minimum temperature required to convert all but 0.020 mol of X to products by 4:00pm
T= ?

Explanation / Answer

40% (0.4 mol out of 1) was converted in 1 hr at 23C

58.33% (0.35 out of 0.6) mole was converted in 1 hr at 28C

28/23 = 58.33/40

Every 5 degrees C you increase the reaction rate by 18.33% (a factor of 1.458)

In order to get from 0.25 to 0.020 in 1 hr you need the rate to convert 92% of the remaining reactants in that time

58.33+18.33x = 92

x = 1.834

1.834*5 = 9.184C

Increase the temperature to 28+9.184 = 37.184C

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