For the equation
`N_(2)O_(5)(g)=2NO_(2)(g)+(1//2)O_(2)(g)`, calculate the mole fraction of `N_(2)O_(5)(g)` decomposed at a constant volume and temperature, if the initial pressure is `600 mm Hg` and the pressure at any time is `960 mm Hg`. Assume ideal gas behaviour.

For the reaction N_(2)O_(5)(g) 2NO_(2)(g)+1//2O_(2)(g) Calculate the mole fraction of N_(2)O_(5)(g) decomposed at a constant volume and temperature, if the initial pressure is 600 mm Hg and the pressure at any time is 960 mm Hg . Assume ideal gas behaviour.

For the reaction, N_(2)O_(5)(g)=2" NO"_(2)(g)+0.5" O"_(2)(g) , calculate the mole fraction of N_(2)O_(5)(g) decomposed at a constant volume and temperature, if the initial pressure is 600 mm Hg and the pressure at any time is 960 mm Hg. Assume ideal gas behaviour.

For the reaction: N_(2)O_(5)(g)rarr2NO_(2)(g)+(1)/(2)O_(2)(g) Calculate the mole fraction of N_(2)O_(5)(g) decomposed at constant volume and temperature, if the initial pressure is 600 mm Hg and the pressure at any time is 960 mm Hg. Assume ideal behaviour

the rate constant of a reaction is 1.5xx10^(7) s^(-1) at 50^(@)C and 4.5 xx10 ^(7) s^(-1) at 100 ^(@)C. Evaluate the Arrhenius paraments A and E^(a) . (ii) for the reaction N_(2)O_(5)(g) to 2NO_(2)(g) + 1/2 O_(2)(g) calculate the mole fractions N_(2)O_(5)(g) decomposed at a constant valume and temperature , if the initial pressses os 600 mm Hg and the pressure at any time is 960 mm Hg Assume ideal gas behaviour.

For the reaction, N_(2)O_(5(g))hArr2NO_(2(g))+0.50_(2(g)) , Calculate the mole fraction of N_(2)O_(5(g)) decomposed at a constant volume and temperature, if the initial pressure is 600 mm Hg and the pressure at any time is 960 mm Hg . Assume ideal gas behaviour.

AB_(2) dissociates as AB_(2)(g) hArr AB(g)+B(g) . If the initial pressure is 500 mm of Hg and the total pressure at equilibrium is 700 mm of Hg. Calculate K_(p) for the reaction.

AB_(2) dissociates as AB_(2)(g) hArr AB(g)+B(g) . If the initial pressure is 500 mm of Hg and the total pressure at equilibrium is 700 mm of Hg. Calculate K_(p) for the reaction.