Solution Found!
Answer: The thermal decomposition of phosphine (PH3) into
Chapter 13, Problem 26P(choose chapter or problem)
The thermal decomposition of phosphine (\(\mathrm{PH}_{3}\)) into phosphorus and molecular hydrogen is a first-order reaction:
\(4 \mathrm{PH}_{3}(g) \rightarrow \mathrm{P}_{4}(g)+6 \mathrm{H}_{2}(g)\)
The half-life of the reaction is 35.0 s at 680°C. Calculate (a) the first-order rate constant for the reaction and (b) the time required for 95 percent of the phosphine to decompose.
Questions & Answers
QUESTION:
The thermal decomposition of phosphine (\(\mathrm{PH}_{3}\)) into phosphorus and molecular hydrogen is a first-order reaction:
\(4 \mathrm{PH}_{3}(g) \rightarrow \mathrm{P}_{4}(g)+6 \mathrm{H}_{2}(g)\)
The half-life of the reaction is 35.0 s at 680°C. Calculate (a) the first-order rate constant for the reaction and (b) the time required for 95 percent of the phosphine to decompose.
ANSWER:Step 1 of 3
Given:
Half life of the reaction = 35 s
The relation between rate constant and half life of 1st order reaction is given below.
