Home
Class 12
CHEMISTRY
28 g of N2 at 299.6 K having a pressure ...

28 g of `N_2` at 299.6 K having a pressure of 2.46 atm occupy

A

`K.E_((He))gtK.E_((Ar))`

B

Cannot be compared

C

`K.E_((He))=K.E_((Ar))`

D

`K.E_((He))gt1/2K.E_((Ar))`

Text Solution

Verified by Experts

Promotional Banner

Similar Questions

Explore conceptually related problems

K_p for the reaction N_2O_4 (g) hArr 2NO_2(g) is 0.66 at 46^@C . Calculate the part per cent dissociation of N_2O_4 at 46^@C and a total pressure of 0.5 atm. Also calculate the partial pressure of N_2O_4 and NO_2 at equilibrium .

For N_2+3H_2⇌2NH_3 , one mole of N_2 and three moles of H_2 are at pressure of 4 atm. Equilibrium pressure is found to be 3 atm. Hence, K_p is:

For the dissociation reaction N_(2)O_(4)(g)hArr2NO_(2)(g), the equilibrium constant K_(P) is 0.120 atm at 298 K and total pressure of system is 2 atm. Calculate the degree of dissociation of N_(2)O_(4) .

A vessel contains 28 g of N_(2) and 32 g of O_(2) at temperature T = 1800 K and pressure 2 atm . What would be the pressure when N_(2) dissociates 30% and O_(2) dissociates 50% and temperature remains constant ?

Hydrogen gas obtained by electrolysis of 18g of water is heated to 127^(@)C at a pressure of 2 atm . Calculate the volume it would occupy.

N_(2)O_(3) dissociates into NO and NO_(2) . At equilibrium pressure of 3 atm , all three gases were found to have equal number of moles in a vessel. In another vessel, equimolormixture of N_(2)O_(3), NO and NO_(2) are taken at the same temperature but at an initial pressure of 9 atm then find the partial pressure of NO_(2) (in atm ) at equilibrium in second vessel! N_(2)O_(3)(g) hArr NO(g) + NO_(2) (g)

28 g "of" N_2 gas is contained in a flask at a pressure of 10 atm and at a temperature of 57^@ C . It is found that due to leakage in the flask, the pressure is reduced to half and the temperature to 27^@ C . The quantity of N_(2) gas that leaked out is.

In a mixture of N_2 and CO_2 gases, the partial pressure of CO_(2) is 1.25 atm. The total pressure of the mixture is 5 atm. The mole fraction of N_(2) in the mixture is

Calculate the temperature at which 28 g of N_2 will occupy a volume of 10.0 litres at 2.46 atmospheres.

The value of K_P for the reactions N_2(g) +3H_2(g) hArr 2NH_3(g), " is " 4.28 xx 10 ^(-5) " at " 450 ^(@) C . A reaction mixture contains N_2,H_2 and NH_3 at partial pressures of 0.6 atm ,2.5 atm and 0.50 atm respectively . In which direction the reaction will proceed?