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Assuming that 50% of the heat is useful,...

Assuming that 50% of the heat is useful, how many kg of water at `15^@C` can be heated to `95^@C` by burning 200 litres of methane at NTP? `DeltaH_("combustion") (CH_4)` = 211 kcal/mole, sp. heat of water = 1 kcal/kg K.

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To solve the problem step by step, we will follow these calculations: ### Step 1: Calculate the number of moles of methane (CH₄) We know that at NTP (Normal Temperature and Pressure), 1 mole of any gas occupies 22.4 liters. Given: - Volume of methane = 200 liters ...
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Assuming that 50% of the heat is useful, ow many kg of water at 15^(@)C can be heated to 95^(@)C by burning 200 litre of methane at STP ? The heat of combustion of methane is 211kcal//mol . Specific heat of water is 1.0 kcal kg^(-1)K^(-1) .

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 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) .

Propane (C_(3)H_(8)) is used for heating water for domestic supply. Assume that for 150 kg of how water supply per day water must be heated from 10^(@)C to 65^(@)C . What moles and volume of propane in litres at S.T.P would have to be used for heating this amount of water? [ DeltaH (combustion) C_(3)H_(8) = -2050 kJ and specific heat of water = 4.184 xx 10^(-3)(kJ)/(g) ].

Heat released by 1kg steam at 150^(@)C if it convert into 1kg water at 50^(@)C .

The thermochemical equation for the combustion of ethylene gas, C_(2)H_(4) , is C_(2)H_(4)(g) rarr 2CO_(2)(g) +2H_(2)O(l), DeltaH^(Theta) =- 337 kcal Assuming 70% efficiency, calculate the weight of water at 20^(@)C that can be converted into system at 100^(@)C by buring 1m^(3) of C_(2)H_(4) gas measured at STP . The heat of vaporisation of water at 20^(@)C and 100^(@)C are 1.00 kcal kg^(-1) and 540 kcal kg^(-1) respectively.

Calculate the increase in mass of water if 200 kg of water is heated from 0^(@)C to 50^(@)C .

One litre sample of a mixture of CH_(4) and O_(2) measured at 32^(@)C and 760 torr, was allowed to react at constant pressure in a calorimeter. The complete combustion of CH_(4) to CO_(2) and water caused a temperature rise in calorimeter of 1K . calculate mole % of CH_(4) in original mixture. [Given: Heat of combustion of CH_(4) is -210.8 Kcal//mol . Total heat capacity of the calorimeter = 2108 cal K ]

100g of water is heated from 30^@C to 50^@C . Ignoring the slight expansion of the water, the change in its internal energy is (specific heat of water is 4184J//kg//K ):

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