The enthalpy change (∆H) for the reaction
                
is -92.38 kJ at 298 K. what is the  at 298 K?

∆U^⊝ of combustion of methane is –X kJ mol^–1. The value of ∆H^⊝ is :

(i) = ∆U^⊝

(ii) > ∆U^⊝

(iii) < ∆U^⊝

(iv)  = 0

What do you understand by:
(i) Heat capacity of a substance
(ii) Heat capacity at constant volume
(iii) Heat capacity at constant pressure?

What do you understand by: (i) Specific heat capacity (ii) Molar heat capacity?

60.8 J of energy is required to change the temperature of 25.0 g of ethylene glycol (a compound used as an antifreeze in automobile engines) by 1.0 K. Calculate heat capacity of ethylene glycol.

169. Calculate the number of kJ of heat necessary to raise the temperature of 60.0g of aluminium from 35 to 55°C. Molar heat capacity of aluminium is 24 J mol^–1 K^–1.