For a reaction: `2NO_(g) + 2H_(2(g) rarr N_(2(g)) + 2H_2O_(g)` the rate law is` rate = k[NO]_2 [H_2]`. What is the overall order with respect to NO and `H_2O`? What is the overall order?

The elementary reaction O_3(g) + O(g) rarr 2 O_2(g) is

The order of the reaction 2NO_(g)+O_(2(g))rarr 2NO_(2(g)) having Rate = k[NO_2]^2[O_2] is

For a reaction, 2NO_(2(g)) rarr 2NO_(g)+O_(2(g)) , the reaction is found to be second order with respect to NO_2 . Write its rate law. Also find its overall order and its molecularity.

Write the expression for: 2 N_2O(g)rarr 4 NO_2(g) + O_2(g) ?

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

A complex reaction takes place in two steps. NO_(g) + O_(3(g)) rarr NO_(3(g))+O_(g) NO_(3(g))+O_(g) rarr NO_(2(g))+ O_(2(g)) The predicted rate law is: rate = k[NO][O_3] Identify the rate determing step. Write overall reaction. Which is the reaction intermediate? Why?

DeltaH for the reaction 2H_(g) rarr H_2(g) will be

For the rection 2NOBr(g) rarr 2NO_2(g)+Br(g) , the rate law is rate = k[NOBr]^2 . If the rate of reaction is 6.5x10^(-6)mole L^(-1) s the concentration of NOBr is 2xx10^(-3) mole L^(-1) . What be the rate constant for the reaction?