# College Chemistry (DrBob222)

The decomposition of HCO2H follows first-order kinetics.

HCO2H(g) CO2(g) + H2(g)

The half-life for the reaction at a certain temperature is 44 seconds. How many seconds are needed for the formic acid concentration to decrease by 73%?

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1. k = 0.693/t1/2

ln(No/N) = kt
No = any convenient number but I would use 100 to represent 100%. Then if it decreases by 73% that leaves 27% so
N = 27
k from above
t = ? Solve for t in seconds if you use half life in seconds.

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2. Thank you! You are legendary!

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