For the reaction
`2H_(2)(g)+2NO(g) rarr N_(2)(g)+2H_(2)O(g)`
the observed rate expression is, rate `=k_(f)[NO]^(2)[H_(2)].` The rate experssion for the reverse reaction is :

For the reaction 2NO(g)+2H_(2)(g)toN_(2)(g)+2H_(2)O(g) . The rate law is rate =k[NO]^(2)[H_(2)] . What is the overall order of reaction.

For the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) , the rate of reaction is expressed as

For the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) , the rate of reaction is expressed as

Consider the reaction : 2H_(2)(g)+2NO(g)rarrN_(2)(g)+2H_(2)(g) The rate law for this reaction is : Rate = k[H_(2)][NO]^(2) Under what conditions could these steps represent mechanism? {:("Step 1:",2NO(g)hArrN_(2)O_(2)(g)),("Step 2:",N_(2)O_(2)+H_(2)rarrN_(2)O+H_(2)O),("Step 3:",N_(2)O+H_(2)rarrH_(2)O+N_(2)):}

Consider the reaction : 2H_(2)(g)+2NO(g)rarrN_(2)(g)+2H_(2)(g) The rate law for this reaction is : Rate = k[H_(2)][NO]^(2) Under what conditions could these steps represent mechanism? {:("Step 1:",2NO(g)hArrN_(2)O_(2)(g)),("Step 2:",N_(2)O_(2)+H_(2)rarrN_(2)O+H_(2)O),("Step 3:",N_(2)O+H_(2)rarrH_(2)O+N_(2)):}

For the reaction : 2NO_(2)(g)+F_(2)(g)rarr2NO_(2)F(g) the rate law is , rate =k[NO_(2)][F_(2)] . Write the differential rate equation for the reaction.

For the reaction , 2C_(2)H_(6)(g)+7O_(2)(g)rarr4CO_(2)(g)+6H_(2)O(l) , the rate of disappearnce of C_(2)H_(6)(g) :

For the reaction 3H_2(g) + N_2(g) rarr 2NH_3(g) . Compute and equate the reaction rates.