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Standard XII

Chemistry

Oxides of Nitrogen

Two moles of ...

Question

Two moles of gas $A_{2}$ are mixed with two moles of gas $B_{2}$ in a flask of volume 1 lit. If at equilibrium 0.5 moles of $A_{2}$ are obtained. Then find out $K_{p}$ for reaction.
$A_{2} (g)_{+} B_{2} (g) ⇌ 2 A B (g)$

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Solution

The correct option is D 36
$K_{p}$ is the equilibrium constant calculated from the partial pressures of a reaction equation. It is used to express the relationship between product pressures and reactant pressures. It is a unitless number, although it relates the pressures.
$K p =$ $\frac{(1.5 \times 2)^{2}}{(0.5 \times 0.5)} = 36$
Hence, the answer is 36.

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Two moles of gas A2 are mixed with two moles of gas B2 in a flask of volume 1 lit. If at equilibrium 0.5 moles of A2 are obtained. Then find out Kp for reaction.A2(g)+B2(g)⇌2AB(g)

Two moles of gas $A_{2}$ are mixed with two moles of gas $B_{2}$ in a flask of volume 1 lit. If at equilibrium 0.5 moles of $A_{2}$ are obtained. Then find out $K_{p}$ for reaction.
$A_{2} (g)_{+} B_{2} (g) ⇌ 2 A B (g)$