\( N _{2}O_{5}\rightarrow2NO_{2}+\frac{1}{2}O_{2}\). The pressure of \(O_{2}\) at "10" minutes and completion of the reaction are 600mm" and "800mm" Hg respectively.What is the half life of the reaction in minutes?

The following reaction was carried out at 44^(@)C : N_(2)O_(5)rarr2NO_(2)+_(1//2)O_(2) The concentration of NO_(2) is 6.0xx10^(-3) M afte minutes of the start of reaction . Calculate the rat of production of NO_(2) over the first ten minutes of the reaction

For the decomposition, N_(2)O_(5)(g) rarr N_(2)O_(4)(g) + 1//2O_(2)(g) , the initial pressure of N_(2)O_(5) is 114 mm and after 20 sec , the pressure of reaction mixture becomes 133 mm . Calculate the rate of reaction in terms of : (a) change in pressure sec^(-1) and (b) change in molarity sec^(-1) . Given that reaction is carried out at 127^(@)C .

For the decomposition of dinitrogen pentoxide at 200^(@)C , N_(2)O_(5)(g)toN_(2)O_(4)(g)+(1)/(2)O_(2)(g) , if the intial pressure is 14 mm and after 25 minutes of the reaction, total pressure of the gassous mixture is 133 mm, calculate the average rate of reaction in (a) atm min^(-1)" "(b)" mol "L^(-1)s^(-1) .

The reaction , 2N_(2)O_(5)rarr 4NO_(2)+O_(2) is first order and takes 24 minutes for 75% decomposition of N_(2)O_(5) at the end of 1 hour after the start of the reaction find the amount of oxide is left.

The decomposition of N_(2)O_(5) at an initial pressure of 380 mm and 50^(@)C is 50% complete in 56 minutes and 71% complete in 100 minutes. What is the order of reaction? How much of N_(2)O_(5) will decomposes in 100 minutes at 50^(@)C but at an initial pressure of 500 mm ?

PQ_(2) dissociates as PQ_2 (g)hArrPQ(g)+Q(g) The initial pressure of PQ_2 is 600 mm Hg. At equilibrium, the total pressure is 800mm Hg. Calculate the value of K_p .