Asked by saud
calculate the half-life of a first- order reaction if the concentration of the reactant is 0.0396 M at 12 seconds after the reaction starts and is 0.00579 M at 47 after the reaction starts. How long does it take for the reactant concentration to decrease to 0.00269 M
Answers
Answered by
DrBob222
ln(No/N) = kt
No = 0.0396
N = 0.00579
k = solve
t = 47-12 = 35 seconds.
Solve for k, then
k = 0.693/t<sub>1/2</sub> and solve for t<sub>1/2</sub>
Then
ln(No/N) = kt and plug in the new numbers to find time for the 0.00269M to be reached.
No = 0.0396
N = 0.00579
k = solve
t = 47-12 = 35 seconds.
Solve for k, then
k = 0.693/t<sub>1/2</sub> and solve for t<sub>1/2</sub>
Then
ln(No/N) = kt and plug in the new numbers to find time for the 0.00269M to be reached.
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