Home
Class 11
CHEMISTRY
N(2(g)) + O(2(g)) + 180.6 kJ to 2NO((g))...

`N_(2(g)) + O_(2(g)) + 180.6 kJ to 2NO_((g))`, calculate (a) heat of reaction, (b) heat of formation of nitric oxide and (c) heat required to form one litre of nitric oxide at `25^@C`. 

Text Solution

Verified by Experts

Thermochemical equation, `N _(2 (g)) + O _(2(g)) to 2 NO _((g )), Delta H =+ 180.6 kJ.` The heat of the given reaction `=Delta H = + 180.6 kJ` Since 2 mole of nitric acid is formed in the reaction, the heat of formation of nitric oxide, `Delta H _(f ) = (Delta H)/(2) = (180.6)/(2) = 90.3 kJ mol ^(-1)`
At `25^(@)C` and 1 atm one mole of a gas occupies 24.4 litres.
Heat required to form 24.4 litre of NO = 90.3 kJ .
Heat required to form one litre of NO `= (90.3)/(24.4) = 3.7 kJ lit ^(-1)`
Promotional Banner

Similar Questions

Explore conceptually related problems

N_(2(g)) + 2O_(2(g)) rarr 2NO_(2) + xkJ, 2NO_((g)) + O_(2(g)) rarr 2NO_(2(g)) + ykJ . The enthalpy of formation of NO is

N_(2(g))+O_(2(g))+"Heat"rarr 2NO_((g)) What information do you get from the above equation ? Comment.

Comment on C_((s))+O_(2(g)) to CO_(2(g))+Heat equation.

10 g of a metal carbonate on heating given 5.6 g of its oxide. The equivalent amont metale 5x. What is x.

N_2(g)+O_2(g)+181kJ leftrightarrow 2NO(g) Write the Le Chatelier's conditions for shifting the equilibrium towards the formation of nitric acid.

For the reaction, N_(2(g)) + 3H_(2(g)) rarr 2NH_(3(g)) . Heat of reaction at constant volume exceeds the heat of reaction at constant pressure by the value of xRT. The value of x is______