Home
Class 11
CHEMISTRY
Calculate the total pressure developed i...

Calculate the total pressure developed in a vessel containing a mixture of three parts `H_(2)` and one part of `N_(2)` to give a mixture containing `10%` ammonia (by moles) at equilibrium at `450^(@)C`.
`K_(p)` for `N_(2)+3H_(2)rarr 2NH_(3)` is `1.6xx10^(-4) atm` units at `450^(@)C`

Text Solution

Verified by Experts

`{:(N_(2),+,3H_(2),hArr,2NH_(3)),(1-x,,3-3x,,2x):}`
Total "moles" `=4-2x`
`[NH_(3)]=(2x)/(4-2x)=10/100,rArr x=0.2/0.1=2/11`
`p_(N_(2))=((1-x))/(4-2x)P=(0.9P)/(4), p_(H_(2))=(3-3xP)/(4-2x)=(2.7P)/(4)`
`p_(NH_(3))=(2x)/(4-2x)P=0.1 P`
`:. K_(p)=((0.1 P)^(2))/((0.9P//4)(2.7P//4)^(3))rArr P^(2)~~903`,
`rArr P=30.03 "atm"`
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Concept Applicationexercise 7.1|53 Videos

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 7.2|40 Videos

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Subjective|15 Videos

  • CLASSIFICATION AND NOMENCLATURE OF ORGANIC COMPOUNDS

    CENGAGE CHEMISTRY ENGLISH|Exercise Analytical and Descriptive Type|3 Videos

Similar Questions

Explore conceptually related problems

K_(p) for the reaction N_(2)+3H_(2) hArr 2NH_(3) at 400^(@)C is 1.64xx10^(-4) atm^(-2) . Find K_(c) .

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) .

If partial pressure of N_2 in gaseous mixture containing equal mass of CO and N_2 is 0.5 atm then the total pressure of gaseous mixture is

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 gaseous mixture of H_(2) and NH_(3) gas contains 68 mass % of NH_(3) . The vapour density of the mixture is-

At 127°C and l atm pressure, a mixture of a gas contains 0.3 mole of N_(2) , 0.2 mole of O_(2) The volume of the mixture is

What is DeltaG^(ɵ) for the following reaction? 1/2 N_(2)(g)+3/2 H_(2)(g) hArr NH_(3)(g), K_(p)=4.42xx10^(4) at 25^(@)C

What is DeltaG^(ɵ) for the following reaction? 1/2 N_(2)(g)+3/2 H_(2)(g) hArr NH_(3)(g), K_(p)=4.42xx10^(4) at 25^(@)C

When a mixture of N_2 and H_2 in the volume ratio of 1:5 is allowed to react at 100 k and 10^3 atm pressure , 0.426 mole fraction of NH_3 is formed at equilibrium . The K_p for the reaction is

The total pressure exerted by the mixture of equal moles of two gases is 5xx10^(3)NM^(-2) in a container of volume 2 litres at 273K. Calculate the number of moles of the gases mixed.