The decomposition of phosphine,PH₃,follows first-order kinetics.
4 PH₃(g) $\to$ P₄(g) + 6 H₂(g)
The half-life for the reaction at 550 ^$\circ$C is 81.3 seconds.What percentage of phosphine remains after 195 seconds?

Question

The decomposition of phosphine,PH₃,follows first-order kinetics.
4 PH₃(g)

\to

P₄(g) + 6 H₂(g)
The half-life for the reaction at 550 ^$\circ$C is 81.3 seconds.What percentage of phosphine remains after 195 seconds?

Quizplus · Accepted Answer

The percentage of phosphine remaining can be calculated using the first-order kinetics formula: $ \text{Remaining} = 100 \times (0.5)^{t/t_{1/2}} $. Here, $ t = 195 $ seconds and $ t_{1/2} = 81.3 $ seconds. Thus, $ \text{Remaining} = 100 \times (0.5)^{195/81.3} \approx 19\% $.

The Decomposition of Phosphine,PH3,follows First-Order Kinetics →\to→ P4(g)+ 6 H2(g) the Half-Life for the Reaction at 550

The Decomposition of Phosphine,PH₃,follows First-Order Kinetics $\to$ P₄(g)+ 6 H₂(g)
the Half-Life for the Reaction at 550