Question:medium
The equilibrium constant for the equilibrium $PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$ at a particular temperature is $2 \times 10^{-2}$ mol L$^{-1}$. The number of moles of $PCl_5$ that must be taken in a one-litre flask at the same temperature to obtain a concentration of $0.20$ mol of chlorine at equilibrium is}
The equilibrium constant for the equilibrium $PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$ at a particular temperature is $2 \times 10^{-2}$ mol L$^{-1}$. The number of moles of $PCl_5$ that must be taken in a one-litre flask at the same temperature to obtain a concentration of $0.20$ mol of chlorine at equilibrium is}
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Always set up ICE table carefully. Mistakes usually happen in equilibrium expressions.
Updated On: May 8, 2026
- $2.2$
- $2.0$
- $1.8$
- $0.2$
- $0.1$
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The Correct Option is A
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