At 400 K oxalic acid decomposes according to the reaction: H2C2O4( g )CO2( g )+H

Question

At 400 K oxalic acid decomposes according to the reaction:
H2C2O4(g)CO2(g)+HCOOH(g)
In three separate experiments, the intial pressure of oxalic acid and final total pressure after 20,000 s is measured.

Find the rate law of the reaction.

At 400  oxalic acid decomposes according to the reaction:

In three separate experiments, the intial pressure of oxalic acid and final total pressure after 20,000  is measured.

Find the rate law of the reaction.

Explanation / Answer

given data points suggests that Ptotal/Pat t=0 = 96.8/65.4= 1.465 from 1st data point

from 2nd data point, Ptotal/P at t=0 = 135/92.1= 1.465, for the 3rd data point, Ptotal/P at t=0 is = 163/111=1.465

so the all the data points sasity the equal ratio and hence the reaction is 1st order for 1st order reaction given

H2C2O4(g)CO2(g)+HCOOH(g)

let Po= initial pressure and change= x

hence pressrue at any time , H2C2O4= Po-x, CO2= x and HCOOH=x

hence total presure = Po-x+x+x= Po+x= 1.465Po

x=0.465Po , Po-x =0.535Po

hecne the integrated expression for -dP/dt= K becomes

ln(P/Po)= -Kt

P=0.465P0, Po=Po=initial presure , t= 20000sec

K=- ln(0.465)/20000= 3.82*10-5/sec

hence the rate expression beomes rate= 3.82*10-5PH2C2O4. ( B is correct)

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.