MCQ
The equilibrium constant for the reaction
${H_2}(g) + {I_2}(g) \rightleftharpoons 2HI(g)$
is $32$ at a given temperature. The equilibrium concentrations of $I_2$ and $HI$ are $0.5 \times 10^{-3}\, M$ and $8 \times 10^{-3}\, M$ respectively. the equilibrium concentration of $H_2$ is
- A$1 \times {10^{ - 3}}\,M$
- B$0.5 \times {10^{ - 3}}\,M$
- C$2 \times {10^{ - 3}}\,M$
- ✓$4.0 \times {10^{ - 3}}\,M$
