Home
Class 12
CHEMISTRY
1mole NH(3) gas is introduced in a 4 lit...

`1`mole `NH_(3)` gas is introduced in a `4 litre` vessel containing `5gram` of He and heated at `400K` temperature. `NH_(3)` is `40%` dissociated and following equilubrium is established `:-`
`NH_(3)hArr(1)/(2)N_(2)+(3)/(2)H_(2)`
Find total pressure at equilibrium `:-`

A

`2.87atm`

B

`21.76atm`

C

`2.17atm`

D

`28.7atm`

Text Solution

Verified by Experts

The correct Answer is:
B
PV=nRT
`P(4)=2.65xx0.0821xx400`
`n_(He)=(5)/(4)=1.25`
`n(NH_(3)+H_(2)+N_(2))=1.4`
Promotional Banner

Similar Questions

Explore conceptually related problems

Some solid NH_(4)HS is placed in flask containing 0.5 atm of NH_(3) . What would be the pressure of NH_(3) and H_(2)S when equilibrium is reached. NH_(4)HS(g) hArr NH_(3)(g)+H_(2)S(g), K_(p)=0.11

N_2 and H_2 are taken in 1:3 molar ratio in a closed vessel to attained the following equilibrium , N_2(g)+3H_2(g) hArr 2NH_3(g) Find K_p for reaction at total pressure of 2P if P_(N_2) at equilibrium is P/3 :

The equilibrium constant for the reaction N_(2)+3H_(2)hArr2NH_(3) "is" 70 at a certain temperature. Hence, equilibrium constant for the reaction NH_(3)hArr(1)/(2)N_(2)+(3)/(2)H_(2) of the same temperature will be approximately

Some acid NH_(4)HS is placed in flask containing 0.5 atm of NH_(3) . What would be pressures of NH_(3) and H_(2)S when equilibrium is reached? NH_(4)HS_((s))hArrNH_(3(g))+H_(2)S_((g)) , K_(p)=0.11

One mole of N_(2) (g) is mixed with 2 moles of H_(2)(g) in a 4 litre vessel If 50% of N_(2) (g) is converted to NH_(3) (g) by the following reaction : N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) What will the value of K_(c) for the following equilibrium ? NH_(3)(g)hArr(1)/(2)N_(2)(g)+(3)/(2)H_(2)(g)