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Following data are obtained for the reac...

Following data are obtained for the reaction:
`N_(2)O_(5) rarr 2NO_(2) + .^(1//2) O_(2)`
`|{:(t//s,0,300,600),([N_(2)O_(5)]//mol L^(-1),1.6 xx 10^(-2),0.8 xx 10^(-2),0.4 xx 10^(-2)):}|`
(a) Show that it follows first order reaction
(b) Calculate the half-life
(Given log 2 = 0.3010 log 4 = 0.6021]

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For the reaction N_(2)O_(5) rarr 2NO_(2) + (1)/(2) O_(2) , the rate of disappearance of N_(2)O_(5) is 6.25 xx 10^(-3) "mol L"^(-1) s^(-1) . The rate of formation of NO_(2) and O_(2) will be respectively.

The rate constant for the reaction 2N_(2)O_(5) rarr 4NO_(2)+O_(2) is 3.0 xx 10^(-5) s^(-1) . If the rate is 2.40 xx 10^(-5) mol L^(-1) s^(-1) , then the concentration of N_(2)O_(5) (in mol L^(-1) ) is

The rate constant for the reaction, 2N_(2)O_(5) rarr 4NO_(2) + O_(2) is 3.0 xx 10^(-5) s^(-1) . If the rate is 2.40 xx 10^(-5) mol L^(-1) s^(-1) , then the initial concentration of N_(2)O_(5) (in mol L^(-1) ) is

The rate constant for the reaction: 2N_(2)O_(5) rarr 4NO_(2)+O_(2) is 3.0xx10^(-5) sec^(-1) . If the rate is 2.40xx10^(-5) M sec^(-1) , then the concentration of N_(2)O_(5) (in M) is:

Rate constant for the reaction 2N_(2)O_(5) to 4NO_(2) + O_(2) is 4.98 xx 10^(-4) s^(-1) . Find the order of reaction?

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