Home
Class 12
CHEMISTRY
Calculate partial pressure of B at equil...

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

A

2

B

3

C

17

D

5.8

Text Solution

Verified by Experts

The correct Answer is:
A
Promotional Banner

Similar Questions

Explore conceptually related problems

At 25^(@)C and 1 atm pressure, the partial pressure in equilibrium mixture of N_(2)O_(4) and NO_(2) , are 0.7 and 0.3 atm , respectively. Calculate the partial pressures of these gases when they are in equilibrium at 25^(@)C and a total pressure of 10 atm .

Calculate the partial pressure of carbon monoxide from the following data’s CaCO_(3)(s) overset(Delta)to CaO(s) + CO_(2)(g), K_(p) = 8 xx 10^(-2) CO_(2)(g) + C(s) rarr 2CO(g), K_(p) = 2

The partial pressures of N_(2)O_(4) "and" NO_(2) "at" 40^(@)C for the following equilibrium N_(2)O_(4)(g)hArr2NO_(2)(g) are 0.1 "atm and" 0.3 atm respectively. Find K_(P) for the reaction.

A vessel at 1000K contains CO_(2)(g) at 2 atm pressure. When graphite is added the following equilibrium is established. CO_(2)(g)+C(s) hArr 2CO(g) the toal pressure at equilibrium is 3 atm. The value of K_(p) is

Calculate K_(P) for the reaction A(g) iff B(s)+2C(g), K_(C)=0.2 at 305 K.

The value of K_(c) for the following equilibrium is CaCO_(3(s))hArrCaO_((s))+CO_(2(g)) . Given K_(p)=167 bar at 1073 K.

A sample of HI(g) is placed in 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)

A sample of HI(g) is placed in 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)

The equilibrium constant, K_(p) for the reaction 2SO_(2)(g)+O_(2)(g)hArr2SO_(3)(g) is 44.0atm^(-1) "at" 1000 K . What would be the partial pressure of O_(2) if at equilibrium the amound of SO_(2) and SO_(3) is the same?

For a gaseous reaction aA(g)+bB(g)hArrcC(g)+dD(g) equilibrium constants K_(c),K_(p) and K_(x) are represented by the following reation K_(c)=([C]^(c)[D]^(d))/([A]^(a)[B]^(b)),K_(p)=(Pc^(c).P_(D)^(d))/P_(A)^(a) and Kx=(x_(C)^(c).x_(D)^(d))/(x_(A)^(a).x_(B)^(b) where [A] represents molar concentrationof A,p_(A) represents partial pressure of A and P represents total pressure, x_(A) represents mole fraction of For the following equilibrium relation betwen K_(c) and K_(c) (in terms of mole fraction) is PCl_(3)(g)+Cl_(2)(g)hArrPCl_(5)(g)