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

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

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

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

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 :

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 ?

The half life period of the reaction : N_(2) O_(5) rarr 2NO_(2) +(1)/(2) O_(2) is 24 hrs at 30^(@) C . Starting with 10 g of N_(2) O_(5) how many grams of N_(2) O_(5) will remain after a period of 96 hours ?

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

Calculate Delta H^(theta) for the reaction : H_(2)O (l) rarr H_(2)(g) + (1)/(2) O_(2) (g) Given 2H_(2)(g) + O_(2)(g) rarr 2H_(2)O(l) Delta H = -571.6 kJ