This is a Mixed question/ It is worth 2 points/You have unlimited attempts/There

Question

This is a Mixed question/ It is worth 2 points/You have unlimited attempts/There is no attempt penalty 08 Question 2 points) a See page 646 Hydrogen peroxide (H202) decomposes into water and oxygen: H2O2(1)- H2O(l)-jo2(g) The data in the table below were collected for the decomposition of H202 at a constant temperature. If possible, determine the reaction order in H202 of the decomposition of H202 and calculate the value of the rate constant at the temperature of the experiments Concentration of Hydrogen Peroxide as a Function of Time Time (s) 0 100 200 500 1000 1500 [H202l (M) 0.500 0.460 0424 0.330 0.218 0.144 1st attem JESTIONSCOMPLETED

Explanation / Answer

Such type of question can be done by hit and trial method only.

For example let us,assume

1. Zero order reaction

If it is zero order

then, co - ct=kt

co= initial conc. ct= final conc. K=equillibrium constant t=time

If it follows zero order then k should be same

for ex. 1. 0.5-0.460/100= 0.0004

2, 0.460-0.424/100= 0.00036

As,K is not same it is not zero order

2. First order

ln(i/f)=kt

i= initial conc f=final conc

checking

1. ln(0.5/0.46)=k(100)

k=8.33*10-4

2. ln(0.424/0.330)=k(300)

k=  8.33*10-4

Hence,as k=constant,we cansay that this is first order kinetics

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