Dinitrogen pentoxide decomposes at 475K as: `N_2O_5(g) rarr N_2O_4(g) + 1/2 O_2(g)` If the initial pressure is 125 mm and after 30 minutes of the reaction, total pressure of the gaseous mixture is 148 mm, calculate the average rate of reaction in atm `mi n^(-1)`

Nitrogen pentoxide decomposes according to equation : 2N_2O_5(g) rarr 4NO_2(g) + O_2(g) This first order reaction was allowed to proceed at 40^@ C and the data below were collected : Calculate the rate constant. Include units with your answer.

Nitrogen pentoxide decomposes according to equation : 2N_2O_5(g) rarr 4NO_2(g) + O_2(g) This first order reaction was allowed to proceed at 40^@ C and the data below were collected : What will be the concentration of N_2O_5 after 100 minutes ?

For the first order reaction 2N_2O_5 (g) rarr 4 NO_2(g)+ O_2(g) which is incorrect:-

The following rate data were obtained for the reaction : 2NO(g) + O_2(g) rarr 2 NO_2 (g) Determine the rate law expression and order of the reaction.

Consider the following reaction for 2NO_2(g) + F_2(g) rarr 2NO_2F(g) . The expression for the rate of reaction in terms of the rate of change of Partial pressures of reactant and product is/are

The decomposition of N_2O_5 according to the equation, 2N_2O_5(g) harr 4NO_2(g) + O_2(g) is a first order reaction. After 30 min from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.5 mm of Hg and on complete decomposition, the total pressure is 584.5 mm of Hg. Calculate the rate constant of the reaction.

A gascous mixture contains 56 g N_2, 44 g CO_(2) and 16 g CH_(4) . The total pressure of mixture is 720 mm. What is partial pressure of CH_(4) ?

For the reaction O_(3(g)) + O_((g)) rarr 2O_(2(g)) , if the rate law expression is, rate = K[O_3] [O] , the molecularity and order of the reaction are respectively

For a reaction : 2NH_3(g) overset (Pt) rarr N_2(g)+3H_2(g) Rate =k . Write the order and molecularity of this reaction.