Home
Class 12
CHEMISTRY
In a mixture of N(2) and H(2) in the rat...

In a mixture of `N_(2)` and `H_(2)` in the ratio `1:3` at `30` atm and `300^(@)C`, the `%` of `NH_(3)` at equilibrium is `17.8`. Calculate `K_(p)` for `N_(2)+3H_(2) hArr 2NH_(3)`.

Text Solution

Verified by Experts

Let, the initial moles of `N_2 and H_2` be 1 and 3 respectively (this assumption is valid as `K_p` will not depend on the exact number of moles of `N_2 and H_2` . One can even start with x and 3x )
`{:("",N_2(g),+,3H_2(g),hArr,2NH_3),("Initially",1,"",3,"",0),("At equilibrium",1-x,"",3-3x,"",2x):}`
Since % by volume of a gas is same as % by mole
`therefore (2x)/(4-2x)=0.178`
`therefore x=(4xx0.178)/((2+2xx0.178))=0.302`
`therefore` Mole fraction of `H_2` at equilibrium
`=(3-3x)/(4-2x)=0.6165`
Mole fraction of `N_2` at equilibrium =1-0.6165-0.178 = 0.2055
`therefore K_p=((x_(NH_2) xxP_(T))^2)/((X_(N_2)xxP_T)(X_(H_2)xxP_T)^3)=((0.178xx30)^2)/((0.2055xx30)(0.6165xx30)^3)`
`K_p=7.31 xx 10^(-4) atm^(-2)`
Promotional Banner

Similar Questions

Explore conceptually related problems

For N_(2)+3H_(3) hArr 2NH_(3)+"Heat"

N_(2)+3H_(2) to NH_(3)

N_(2)+3H_(2) to NH_(3)

2 mol of N_(2) is mixed with 6 mol of H_(2) in a closed vessel of one litre capacity. If 50% N_(2) is converted into NH_(3) at equilibrium, the value of K_(c) for the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g)

A mixture of N_2 and H_2 in the molar ratio of 1:3 reacts to give NH_3 developing an equilibrium pressure of 50 atm and 650 ^@C . NH_3 present at equilibrium at equilibrium is 25% by weight, calculate K_p for N_2(g) +3H_3(g) hArr 2NH_3(g)

A reaction mixture containing H_(2), N_(2) and NH_(3) has partial pressures 1 atm, 2 atm, and 3 atm. Respectively, at 725 K . If the value of K_(p) for the reaction, N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) is 4.28xx10^(-5) atm^(-2) at 725 K , in which direction the net reaction will go?

In a chemical reaction N_(2)+3H_(2) hArr 2NH_(3) , at equilibrium point

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 20 L reaction vessel at 500 K . At this temperature, the equilibrium constant K_(c ) for the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) is 1.7xx10^(2) . Is the reaction mixture at equilibrium? If not, what is the direction of the net reaction?

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 20 L reaction vessel at 500 K . At this temperature, the equilibrium constant K_(c ) for the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) is 1.7xx10^(2) . Is the reaction mixture at equilibrium? If not, what is the direction of the net reaction?

In a container of constant volume at a particular temparature N_(2) and H_(2) are mixed in the molar ratio of 9:13 . The following two equilibria are found o be coexisting in the container N_(2)(g)+3H_(2)(g)harr2NH_(3)(g) N_(2)(g)+2H_(2)(g)harr N_(2)H_(4)(g) The total equiibrium pressure is found to be 305 atm while partial pressure of NH_(3)(g) and H_(2)(g) are 0.5 atm and 1 atm respectivly. Calculate of equilibrium constants of the two reactions given above.