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Q.

2 mole of X and 1 mole of Y are allowed to react in a 2 litre container. When equilibrium is reached. the following reaction occurs $2 X (g) + Y (g) ⇌ Z (g) at 300 K$ If the moles of Z at equilibrium is 0.5 then what is equilibrium constant $K_{C}$ ?

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answer is 4.

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Detailed Solution

When X reacts with Y the reaction takes place as,

$\begin{array}{lccc} 2 X (g) + Y (g) ⇌ Z (g) \\ t = 0 & 2 & 1 & - \\ At eq. & 2 - 2 x 1 - x & x \end{array}$

$K_{c} = \frac{\frac{0.5}{2}}{{(\frac{1}{2})}^{2} \times (\frac{1}{2^{2}})} = 4$

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2 mole of X and 1 mole of Y are allowed to react in a 2 litre container. When equilibrium is reached. the following reaction occurs 2X(g)+Y(g)⇌Z(g) at 300K If the moles of Z at equilibrium is 0.5 then what is equilibrium constant KC?