The heat of combustion of ethane gas at 373 k cal per mole. Assume that 50% of heat is lost, how many litres of ethane measured at STP must be convert `50` kg of water at `10^(@)C` to steam at `100^(@)C` ? One mole of gas oc cupies `22.4` litres at STP. Take latent heat of steam `=2.25xx10^(6) j kg^(-1)` .

The heat of combustion of ethane gas at 373 k cal per mole. Assume that 50% of heat is useful, how many be burnt litres to convert 60 kg of water at 20^(@)C to steam at 100^(@)C ? One mole of gas oc cupies 22.4 litre at S.T.P. Latent heat of steam = 2.25 xx 10^(6) Jkg^(-1) .

The heat of combustion of ethane gas is -368 kcal mol^(-1) . Assuming that 60% of heat is useful, how many m^(3) of ethane measured at NTP must be burned to supply heat to convert 50 kg of water at 10^(@)C to steam at 100^(@)C ?

The heat of combustion of ethane gas is 368 kcal //mol . Assuming that 60% of the heat is useful, how many m^(3) of ethane 9 measured at STP ) must be burnt to supply enough heat to convert 50kg of water at 10^(@)C to steam at 100^(@)C ? Specific heat of water is 1 cal//g . Heat of vaporisation of H_(2)O is 540cal//g .

The heat of combustion of ethane gas is 368xx10^(3) cal mol^(-1) . If 62 per cent of heat is useful, how many m^(3) of ethane measured at STP must be burnt to supply enough heat to convert 50kg of water at 10^(@)C to steam at 100^(@)C ? Specific heat and heat of vaporisation of water are 1 cal //g and 540 cal//g respectively.

Calculate the volume of ethane required to be burnt to convert 100 kg of water at 20^@C to steam at 100^@C , assuming that only 40% of heat is useful. Heat of combustion of ethane is 371 kcal "mol"^(-1) . (One mole of gas occupies 22.4 litres at S.T.P. and latent heat of water is 2.25 xx 10^6 J kg^(-1) )

How much work in joule is done in producing heat necessary to convert 10g of ice at -5^(@)C into steam at 100^(@)C ? Given specificheat of ice =0.5 cal g^(-1).^(@)C^(-1) , latent heat of steam = 540 cal g^(-1) .

400 kg of water is heated from 30^(@) C to 100^(@)C . What will be the increase in mass of water ? Take specific heat of wateer = 4.2 xx10^(3) " J kg"^(-1).^(@)C^(-1) .

500 kg of water is heated from 20^(@) to 100^(@) C . Calculate the increase in the mass of water.Given specific heat of water =4.2 xx 10^(3) J kg ^(-1) .^(@)C^(-1) .

calculate the increase in internal energy of 1 kg of water at 100(0)C when it is converted into steam at the same temperature and at 1atm (100 kPa). The density of water and steam are 1000 kg m^(-3) and 0.6 kg m^(-3) respectively. The latent heat of vaporization of water =2.25xx10^(6) J kg^(1) .