In a gaseous reaction A_{2(g)} longrightarrow | vedclass

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(B) Given reaction: $A_{2(g)} \longrightarrow B_{(g)} + \frac{1}{2} C_{(g)}$Initial pressure at $t = 0$: $P_{A_2} = 100 	ext{ mm}$,$P_B = 0$,$P_C = 0

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(B) Given reaction: $A_{2(g)} \longrightarrow B_{(g)} + \frac{1}{2} C_{(g)}$Initial pressure at $t = 0$: $P_{A_2} = 100 	ext{ mm}$,$P_B = 0$,$P_C = 0$Pressure at $t = 5 	ext{ min}$: $P_{A_2} = 100 - x$,$P_B = x$,$P_C = \frac{1}{2} x$Total pressure $P_t = (100 - x) + x + \frac{1}{2} x = 100 + \frac{1}{2} x$Given $P_t = 120 	ext{ mm}$,so $100 + \frac{1}{2} x = 120$$\frac{1}{2} x = 20 \implies x = 40 	ext{ mm}$The rate of disappearance of $A_2$ is defined as the change in its partial pressure over time: $\frac{x}{t} = \frac{40 	ext{ mm}}{5 	ext{ min}} = 8 	ext{ mm min}^{-1}$.

In a gaseous reaction $A_{2(g)} \longrightarrow B_{(g)} + \frac{1}{2} C_{(g)}$,the increase in pressure from $100 \text{ mm}$ to $120 \text{ mm}$ is noticed in $5 \text{ min}$. The rate of disappearance of $A_2$ in $\text{mm min}^{-1}$ is

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