Home
Class 11
CHEMISTRY
A 550 K, the K(c) for the following rea...

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

A

`2xx10^(-4)`

B

`10^(-4)`

C

`2xx10^(4)`

D

`10^4`

Text Solution

Verified by Experts

The correct Answer is:
A
`K_c=([Z])/([X][Y])implies1/2[Y]=[X]=1/2[Z]=a` (say)
`:. [Z] = 2a, [Y] = 2a, [X] = a`
`10^4 = (2a)/(a.2a) implies a =10^(-4)`
`[Z] = 2a = 2 xx10^(-4)`
Promotional Banner

Similar Questions

Explore conceptually related problems

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 ?

At 600^(@)C,K_(P) for the following reaction is 1 atm. X(g) rarr Y(g) + Z(g) At equilibrium, 50% of X (g) is dissociated. The total pressure of the equilibrium system is p atm. What is the partial pressure (in atm) of at equilibrium ?

At 500 K, equlibrium constant, K_(c) for the following reaction is 5. 1//2 H_(2)(g)+ 1//2(g)hArr HI (g) What would be the equilibrium constant K_(c) for the reaction 2hi(g)hArrH_(2)(g)+l_(2)(g)

1 mol of nitrogen is mixed with 3 mol of hydrogen in a 4 L container. If 0.25% of nitrogen is converted to ammonia by the following reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) then calculate the equilibrium constant K_(c) in concentration units. What will be the value of K_(c) for the following equilibrium? 1/2 N_(2)(g)+3/2 H_(2)(g) hArr NH_(3)(g)