At 550 K, the Kc for the following reaction is `10^(4) mol^(-1)L . X(g) + Y(g) rarr Z(g)` At equilibrium, it was observed that `[X] = 1/2[Y] = 1/2[Z]` . What is the value of `[Z]("in "mol^(-1)L)`at equilibrium ?

Options

A. `2 xx 10^(-4)`
B. `10^(-4)`
C. `2 xx 10^4`
D. `10^4`

Answer

A

Explanation

`X_((g)) + Y_((g)) `therefore K_c = ([Z])/([X][Y]) = 10^4`
`= ([Z])/(1/2 [Z][Z]) = 10^4 = 1/2 [Z] = 1/(10^4)`
`implies [Z] = 2 xx 10^(-4) M`