Question

You are monitoring the disappearance of ethanol vapor C2H5OH(g) in a closed, rigid chamber of volume 5 liters during the decomposition reaction

C2H5OH(g) --> CH3CHO(g) + H2(g) at T = 500 K.

The reaction is catalyzed by a copper surface.

If the activation energy for this reaction is 23 KJ/mol and the pressure is 113 torr, but at 450 seconds instead of 900 seconds, at what temperature should I run the reaction?

Answer 1

VILLA aoonenius daw According to kako ė Ea KE rareconstant , kot Arsenious factor Ea= activation Т- Te m() exhчуе. Energy, Ri universal lemperature. Gas constand. complete sin goos, at first reaction this condition temperature i T2 rade constant =ki Kiz ko e tra le cu we have to make the reaction to be completedin 450 seconds at this condition rate constant = kz, Temperature = Tz K2=ko e Ri (2) Ratea concentration of ethanol vanout = k [Ca Agon ] time ac is order of reaction, > (3) from (3) kal Time So Rial Į and kal and ko at Where to and ta of reactionat are time for complety temperatures Ti andi so that is not : : > (4) P IL considering (4) and (5) Las are same so ee CE ? en ( 2 ) = - El [ 1 ] {dne=1] t2 = 4650s, ti= 900s . Ea = 23 kJ/mol R = 8.314 Jhon Eq = 23,031 To = 500k ,Tz = ? substitating these values 400 in C 490) = - 23x10 Cose I -I 5500 1 / 2 = encuso a ] 8.314 5oo Ez -881314 -23x103 = 2.50557410649 -4 = 2.50557110 T2-500 500 Tz -4 60 x 2.5 0 5 5 3x 0 KT, , -5 6 : T2 [1 - 500x 2.50537x16 4 J -500 T2 = 500 1-500 x 2.5 OSS X10 9 Tz = 571.6lku 671.6lk So at 1571.61kl The The reaction should run. Scanned with CamScanner