Write the rate law of `2N_(2)O_(5(g))rarr 4NO_(2(g))+O_(2(g))` reaction.

Discuss the rate of the reaction 2N_(2)O_(5(g)) rarr 4NO_(2(g))+O_(2(g))

For a first order reaction involving decomposition of N_(2) O_(5) the following information is available : 2N_(2)O_(5)(g) rarr 4NO_(2) (g) +O_(2)(g) Rate =k [N_(2)O_(5)] N_(2)O_(5)(g) rarr 2NO_(2)(g) +1//2 O_(2) (g) Rate =k [N_(2)O_(5)) Which of the following expressions is true ?

Nitrogen pentoxide decomposes according to equation : 2N_(2)O_(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 : (a) Calculate the rate constant. Include units with your answer. (b) What will be the concentration of N_(2)O_(5) after 100 minutes ? (c ) Calculate the initial rate of reaction ?

For the reaction : 2 NH_(3)(g) rarr N_(2)(g) + 3 H_(2)(g)

In the reaction N_(2(g)) + O_(2(g)) to 2NO_((g)), DeltaH^@ reaction is + 179.9 kJmol^(-1) and DeltaS_("reaction")^@ = 66.09 JK^(-1)mol^(-1) . Calculate DeltaG^@ reaction at 300K.

The rate constant for the reaction : 2N_(2) O_(5) rarr 4NO_(2) +O_(2) is 3.0xx10^(-5) "sec"^(-1) . If the rate is 2.40xx10^(-5) mol "litre"^(-1) "sec"^(-1) then the concentration of N_(2)O_(5) (in mol "litre"^(-1) ) is :

Changes in enthalpy for the reaction : 2H_(2)O_(2)(g) rarr 2H_(2)O (l) + O_(2)(g) if heat of formation of H_(2)O_(2)(l) and H_(2)O(l) are -188 kJ mol^(-1) and -286 kJ mol^(-1) respectively is

For the reaction : C(s) + O_(2)(g) rarr CO_(2)(g)