Home
Class 11
CHEMISTRY
1 mol of A and 0.5 mole of B were enclos...

1 mol of A and 0.5 mole of B were enclosed in a three litres vessel. The following equilibrium was established under suitable conditions.
`A+2B hArrC`
At equilibrium, the amount of B was found to be 0.3 mol. The equilibrium constant `K_C` at the experimental temperature will be

A

`11.1`

B

`1.11`

C

`0.01 `

D

`2.50`

Text Solution

Verified by Experts

The correct Answer is:
A
`{:(A,+,2B,hArr,C),(1,,0.5,,0),(1–0.1 ,,0.5–0.2 ,,0.1),(0.9,, 0.3 ,,0.1),((0.9)/3,,(0.3)/3,,(0.1)/3):}`
`K=([C])/([A][B]^2)=([0.1//3])/(([0.9//3][0.3//3])^(2))`
`=11.11`
Promotional Banner

Similar Questions

Explore conceptually related problems

1 moles of NO_2 and 2 moles of CO are enclosed in a one litre vessel to attain the following equilibrium NO_2 +CO hArr NO+ CO_2 . It was estimated that at the equilibrium , 25% of initial amount of CO is consumed. The equilibrium constant K_p is

In the reaction, A + B hArr2C , at equilibrium, the concentration of A and B is 0.20 mol L^(-1) each and that of C was found to be 0.60 mol L^(-1) . The equilibrium constant of the reaction is

One mole of SO_(3) was placed in a litre reaction vessel at a certain temperature. The following equilibrium was established 2SO_(3)(g)hArr 2SO_(2)(g)+O_(2)(g) At equilibrium 0.6 moles of SO_(2) were formed. The equilibrium constant of the reaction will be

When 3.00 mole of A and 1.00 mole of B are mixed in a 1,00 litre vessel , the following reaction takes place A(g) +B(g) hArr 2C(g) the equilibrium mixture contains 0.5 mole of C. What is the value of equilibrium constant for the reaction ?

4 mole of Sl_(2)Cl_(4)(g) is introduced innto a 10L vessel. The following equilibrium was established S_(2)Cl_(4)(g)hArr2SCl_(2)(g) at equilibrium 0.2 mol of S_(2)Cl_(4) was present in the vessel. The value of equilibrium constant is.

A+B rarr C+D Initially moles of A and B are equal. At equilibrium, moles of C are three times of A. The equilibrium constant of the reaction will be

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) hArr Z(g) at 300 K. If the moles of Z at equilibrium is 0.5 then what is equilibrium constant K_C ?

For the reaction, A(g)+2B(g)hArr2C(g) one mole of A and 1.5 mol of B are taken in a 2.0 L vessel. At equilibrium, the concentration of C was found to be 0.35 M. The equilibrium constant (K_(c)) of the reaction would be

In the reversible reaction A + B hArr C + D, the concentration of each C and D at equilobrium was 0.8 mole/litre, then the equilibrium constant K_(c) will be