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From the following data show that the decomposition of H_(2)O_(2) is a reaction of first order. Also calculate the value of the rate constant. |
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Answer» Solution :Let us substitute the values in the rate EQUATION for FIRST order reaction and calculate the value of rate constant(k) `k=2.303/tlog(a/(a-x)) = (2.303)/tlogV_(0)/V_(t)` CASE I. `V_(0) = 22.8 mL, V_(t) = 13.8 mL, t=10 min` `k=(2.303)/(10 min) log(22.8)/(13.8) = (2.303)/(10 min) (log 22.8 - log13.8)` `=(2.303)/(10 min) (1.358-1.140) = (2.303 XX 0.128)/(10 min) = 0.0502 min^(-1)` Case II. `V_(0) =22.8 mL, V_(t)=8.3, t=20min` `therefore k=(2.303)/(20 min)(1.388 - 0.919) = (2.303 xx 0.439)/(20 min) = 0.0505 min^(-1)` Since, the value of k comes out to be almost constant, the reaction is of first order. |
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