Home
Class 11
CHEMISTRY
At 1000 K , a sample of pure NO(2) gases...

At 1000 K , a sample of pure `NO_(2)` gases decomposes as :
`2NO_(2)(g)hArr2NO(g)+O_(2)(g)`
The equilibrium constant `K_(P)` is 156.25 atm .Analysis showns that the partial pressure of `O_(2)` is 0.25 atm at equilibrium .The parital pressure o f`NO_(2)` at equilibrium is :

A

`0.01`

B

`0.02`

C

`0.04`

D

none of these

Text Solution

Verified by Experts

The correct Answer is:
b
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM

    NARENDRA AWASTHI|Exercise Level 1 (Q.93 To Q.122)|1 Videos

  • CHEMICAL EQUILIBRIUM

    NARENDRA AWASTHI|Exercise Level 2|1 Videos

  • ATOMIC STUCTURE

    NARENDRA AWASTHI|Exercise level 2|1 Videos

  • DILUTE SOLUTION

    NARENDRA AWASTHI|Exercise Level 3 - Match The Column|1 Videos

Similar Questions

Explore conceptually related problems

For the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) the equilibrium constant K_(p) changes with

NH_(4)HS(s)hArrNH_(3)(g)+H_(2)S(g) The equilibrium pressure at 25^(@)C is 0.660 atm . What is K_(p) for the reaction?

N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) For the reaction intially the mole ratio was 1:3 of N_(2):H_(2) .At equilibrium 50% of each has reacted .If the equilibrium pressure is P, the parial pressure of NH_(3) at equilibrium is :

In the equilibrium 2SO_(2)(g)+O_(2)(g)hArr2SO_(3)(g) , the partial pressure of SO_(2),O_(2) and SO_(3) are 0.662,0.10 and 0.331 atm respectively . What should be the partial pressure of Oxygen so that the equilibrium concentrations of SO_(3) are equal ?

For the reaction 2NO_(2)(g)+(1)/(2)O_(2)(g)hArrN_(2)O_(5)(g) if the equilibrium constant is K_(p) , then the equilibrium constant for the reaction 2N_(2)O_(5)(g)hArr4NO_(2)(g)+O_(2)(g) would be :

When N_(2)O_(5) is heated at certain temperature, it dissociates as N_(2)O_(5)(g)hArrN_(2)O_(3)(g)+O_(2)(g),K_(c)=2.5 At the same time N_(2)O_(3) also decomposes as : N_(2)O_(3)(g)hArrN_(2)O(g)+O_(2)(g). "If initially" 4.0 moles of N_(2)O_(5) "are taken in" 1.0 litre flask and alowed to dissociate. Concentration of O_(2) at equilibrium is 2.5 M. "Equilibrium concentratio of " N_(2)O_(5) is :

N_(2)O_(3) is an unstable oxide of nitrogen and it decomposes into NO (g) and NO_(2)(g) where NO_(2)(g) is further dimerise dimerise into N_(2)O_(4) as N_(2)O_(3)(g)hArrNO_(2)(g)+NO(g)" ",K_(p_(1)=2.5 bar 2NO_(2)(g)hArrN_(2)O_(4)(g)" ": K_(P2) A flask is initially filled with pure N_(2)O_(3)(g) having pressure 2 bar and equilibria was established. At equilibrium partial pressure of NO (g) was found to be 1.5 ber. The equilibrium partial pressure of N_(2)O_(3)(g) is :

A sample of HI (g) is placed in a flask at a pressure of 0.2 atm. At equilibrium the partial pressure of HI (g) is 0.04 atm. What is K_(p) for the given equilibrium ? 2HI(g) hArr H_(2)(g) + I_(2)(g)

Calculate partial pressure of B at equilibrium in the following equilibrium A(s) iff B(g) +2C(g), " " K_(P)=32 atm^(3) .

5 moles of SO_(2) and 5 moles of O_(2) are allowed to react .At equilibrium , it was foumnd that 60% of SO_(2) is used up .If the pressure of the equilibrium mixture is one aatmosphere, the parital pressure of O_(2) is :