For the reaction `2NO_(2)rarr2NO+O_(2)`, rate expressed as :

For the reaction , 2NO_(2) rarr 2NO+ O_(2) rate is expressed as :

For the reaction 2SO_(3) to 2SO_(2) +O_(2) rate is expressed as ,

The rate of the reaction 2SO_(2) +O_(2) rarr 2SO_(3) may be expressed as : -(d[O_(2)])/(dt)= 2.5 xx10^(-4) "mol L"^(-1) "sec"^(-1) The rate of reaction when expressed in terms of SO_(3) will be :

For the reaction 2NO(g)+O_(2)(g)rarr2NO_(2)(g) , the rate law is r=k[NO]^(2)[O_(2)] . The reaction is carried out in a V L closed container . If the container had a volume equal to one-fourth of V L , then what would the reaction - rate be ?

For the reaction 2H_(2)+O_(2)rarr 2H_(2)O , the rate law expression is , r = k[H_(2)]^(n) . When the concentration of H_(2) is doubled, the rate of reaction found to be quadrupled. The value of n is

For the reaction : 2O_(3) rarr 3O_(2) the rate of reaction is correctly given by the expression

For the reaction, 2NO_((g) + O_(2(g) rarr 2NO_(2(g) the rate law is given as. Rate =k [NO]^2[O_2] The order of the reaction with respect to O_2 is _______

For the reaction : 2N_(2)O_(5) rarr 4NO_(2) +O_(2) , the rate of reaction in terms of O_(2) is d[O_(2)] /dt. In terms of N_(2)O_(5) , it will be :

For the reaction : 2N_(2)O_(5) rarr 4NO_(2) +O_(2) , the rate of reaction in terms of O_(2) is d[O_(2)] /dt. In terms of N_(2)O_(5) , it will be :

For the reaction, ltBrgt 2NO_(2)(g)rarr2NO(g)+O_(2)(g) at a certain temperature, the initial rate of decomposition of NO_(2) is 0.0036 mol L^(-1)s^(-1) . What is the initial rate of formation of O_(2)(g) in mol. L^(-1).s^(-1) ?