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the rate constant of a reaction is 1.5x...

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.

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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.

The rate constant of a reaction is 1.5 xx 10^(7)s^(-1) at 50^(@)C and 4.5 xx 10^(7) s^(-1) at 100^(@)C . Evaluate the Arrhenius parameters A and E_(a) .

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 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))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.

For a reaction, 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g) rate of reaction is:

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