Home
Class 12
CHEMISTRY
At 1000 K, if the equilibrium constant K...

At 1000 K, if the equilibrium constant `K_(p)` for the reaction.
`2NOCl(g)hArr2NO(g)+Cl_(2)(g)`
is `4.157xx10^(-4)` bar, the `K_(c)` (in mol`L^(-1)`) is (R = 0.083 L bar `K^(-1)mol^(-1)`)

A

`4.16xx10^(-7)`

B

`4.16xx10^(-4)`

C

`5.0xx10^(-4)`

D

`5.0xx10^(-6)`

Text Solution

Verified by Experts

The correct Answer is:
D
`K_(p)=K_(c)(RT)^(Deltan)`
Where,
`K_(C)andK_(p)` = Equilibrium constants
R = Gas constant (0.083 L`"bar"^(-1)xx"mol"^(-1)`)
T = Temperature (1000K)
`Deltan` = Number of gaseous moles of product - Moles of reactant
`K_(c)=4.157xx10^(-4)`
`Deltan=3-2=1`
`K_(C)=K_(b)/(RT)=(4.157xx10^(-4))/(0.083xx1000)`
= `5.0xx10^(-6)`
Promotional Banner

Similar Questions

Explore conceptually related problems

At 1000 K, the equilibrium constant, K_(c) for the reaction 2NOCl(g) hArr 2NO(g) +Cl_(2)(g) is 4.0xx10^(-6) mol L^(-1) . The K_(p) (in bar) at the same temperature is (R=0.083" L bar K"^(-1) mol^(-4))

The equilibrium constant for the reaction: N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) at 725K is 6.0xx10^(-2) . At equilibrium [H_(2)]=0.25 "mol" L^(-1) and [NO_(3)]=0.06 "mol" L^(-1) Calculate the equilirbium concentration of N_(2) .

The value of K_(p) for the reaction 2H_(2)S(g) hArr 2H_(2)(g) +S_(2)(g) is 1.2 xx 10^(-2) at 1065^(circ)C . The value of K, for this reaction is

A mixture of 1.57 mol of N_(2) , 1.92 mol of H_(2) and 8.13 mol of NH_(3) is introduced into a 20L reaction vessel at 500K . At this temperature, the equilibrium constant, K_(c) for the reaction N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) is 1.7xx10^(2) . Is the reaction mixture at equilibrium ? If not, what is the direction of the net reaction ?

At 298 k, the equilibrium constant of the process 1.5O_2 (g) hArr O_3 (g) "is" 3xx10^(-29) . Standard free energy change (in K. J mol^(-1) ) of the process is approximately (R= 8.314 J mol^(-1) k^(-1), log 3 = 0.47)

18.4 g N_(2)O_(4) was placed in 1 L vessel at 400 K and allowed to attain the following equilibrium N_(2)O_(4)(g) hArr 2NO_(2)(g) . IF the total pressure at equilibrium was 10.64 bar, approximate K_(p) is (R = 0.083 L bar K^(-1) mol^(-1) ) (Assume N_(2)O_(4), NO_(2) as ideal gases)

For the reaction CO_((g)) + Cl_(2(g)) hArr COCl_(2(g)). The K_(p)//K_(c) is equal to