What will be the amount of heat evolved by burning 10 L of methane under standard conditions?
`-76.2, -398.8 and -241.6" kJ mol"^(-1)` resepctively

Calculate the entropy change in surroundings when 1.00 mole of H_2O(l) is formed under standard conditions. Delta_fH^@ = -286 kJ mol^(-1)

A gas mixture of 3.67L of ethylene and methane on complete combustion at 25^(@)C produces 6.11 L of CO_(2) . Find out the heat evolved on buring 1L of the gas mixture. The heats of combustion of ethylene and methane are -1423 and -891kJ mol^(-1) , respectively, at 25^(@)C .

A gas mixture of 3.67L of ethylene and methane on complete combustion at 25^(@)C produces 6.11 L of CO_(2) . Find out the heat evolved on buring 1L of the gas mixture. The heats of combustion of ethylene and methane are -1423 and -891kJ mol^(-1) , respectively, at 25^(@)C .

A gas mixture of 3.67L of ethylene and methane on complete combustion at 25^(@)C produces 6.11 L of CO_(2) . Find out the heat evolved on buring 1L of the gas mixture. The heats of combustion of ethylene and methane are -1423 and -891kJ mol^(-1) , respectively, at 25^(@)C .

Calculate the standard heat of formation of carbon disulphide (l). Given that the standard heats of combustion of carbon (s), sulphur (s) and carbon disulphide (l) are -393.3, -293.72 and -1108.76 kJ mol^(-1) respectively.

How much heat is evolved if 3.2 g of methane is burnt and if the heat of combustion of methane is -880" kJ mol"^(-1) ?

How much heat is evolved if 3.2 g of methane is burnt and if the heat of combustion of methane is -880" kJ mol"^(-1) ?