Asked by Ana
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%?
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%?
Answers
Answered by
DrBob222
k = 0.693/t<sub>1/2</sub>
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.
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.
Answered by
Ana
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