the decomposition of HCO2H follows first order kinetics. The half life for the r
ID: 963800 • Letter: T
Question
the decomposition of HCO2H follows first order kinetics. The half life for the reaction at a certain temperature is 34 seconds. How many seconds are needed for the formic acid concentration to decrease by 37% the decomposition of HCO2H follows first order kinetics. The half life for the reaction at a certain temperature is 34 seconds. How many seconds are needed for the formic acid concentration to decrease by 37% the decomposition of HCO2H follows first order kinetics. The half life for the reaction at a certain temperature is 34 seconds. How many seconds are needed for the formic acid concentration to decrease by 37%Explanation / Answer
find the rate constant using first order kinitics
k = 0.693 / t1/2
k = 0.693 / 34 = 0.0204 s-1
now use the first order rate equation
k = (2.303/t) log(a / a-x)
a = intial concentration 100%
a-x = 100-37 = 63% remains
0.0204 = (2.303 / t) log(100/67)
t = 2.303 x 0.174 / 0.0204
t = 19.63 s
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