Question

Biochemistry and Differential Equations: (25 pts) and Given the following simple reaction mechanism: A + B ->C Where the forward rate constant for this reaction at 25C is known to be 1.6 * 1044 V initial concentrations are as follows: [A]o = 7.5 uM Blo= 3.5 M [C]m = 0 If the reaction is run at 250 for 10 seconds, what will the concentration of [C] be? o. What if the temperature is increased to 45C?

Answer 1

(a) A + B C Initial 7.5 35 - Final 7.5-2 3.5-2 a for 2nd order reaction with two different reactant at different concentrations , kt = t in (B3/13% [B],-(Al. (A]/[A]. kt l = . 1/3.5-1/3-5 17.5-117.5 r (3.5-7.5 um 3.5- y 2.143 -1 1-6X100 M5 = X10S ( 7.5-% 4 MM -4 X1D-5 MX 16 X10 My xD 3.5-3 X 2.142) 7.5-8 I - - 0.064 - -0.004 e 0.938 3.5-8 x 2.143 = 7.5-2 :. 3.5-7 . 0.4377 7.5-1 3.2828 - 0.4377% 3-5-X - 0.3863 um :: ze = 3.5-3-2828 1- 0.4377 .:|[C] = 0.3863 UM

(6) Increase in temp will increase the rate constant value and rate of geaction will be more , hence [C] will be greater at 45°C affer 10 second. k= A e taIRT [k&TI By knowing the value of activation energy Ea, the increas increase in sate can be coleslated by following equation, In the )