Chemistry and Chemical Reactivity (9th Edition)

Published by Cengage Learning
ISBN 10: 1133949649
ISBN 13: 978-1-13394-964-0

Chapter 14 Chemical Kinetics: The Rates of Chemical Reactions - Study Questions - Page 553f: 64


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Work Step by Step

a) From the rate law $r=k[PH_3]$, we deduce it's a first-order reaction, for which: $\ln(C/C_0)=-0.693/t_{1/2}\times t$ Decomposing 3/4 means that $C/C_0=0.25$ $\ln 0.25=-0.693/37.9\ s\times t$ $t=75.8\ s$ b) $\ln (C/C_0) = -0.693\times 60\ s/37.9\ s$ $(C/C_0)=0.334\ or\ 33.4\%$ The remaining fraction is 33.4% of the original.
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