Asked by Steve

The decopostion of formic acid follows first-order kinetics.

HCO2H(g)==>CO2(g) + H2(g)

The half-life for the reaction at 550 degrees Celsius is 24 seconds. How many seconds does it take for the formic acid concentration to decrease by 75%?

Answered by DrBob222
Calculate k = 0.693/t(1/2) = 0.693/24
Then ln(No/N) = kt
No = 100 to start (any number will do)
N = reduced by 75% so N = 25?
Plug in N, No, and k, solve for t.
Post your work if you get stuck.
Answered by Brandon
Where does the 0.693 come from?
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