What volume of carbon dioxide is released in the following case:
A power station burns coal at 45.5 tonnes per hour (1 tonne = 10^6 g). Assuming the coal is pure carbon and that all the coal is oxidized completely to carbon dioxide gas on combustion, what volume of carbon dioxide is released to the atmosphere per hour when the atmospheric pressure is 758 mmHg and the temperature is 19.0 degrees C?
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The power station burns coal at 45.5 tonnes per hour and it is assumed that the coal is pure carbon and that all of the coal is oxidized completely to carbon dioxide gas on combustion.
The combustion of carbon follows the reaction C + O2 --> CO2. One mole of carbon dioxide is released for a mole of carbon burnt. The molar mass of carbon is 12 g/mol. 45.5 ton of carbon is 45.5*10^6 g or 45.5*10^6/12 moles = 3.791*10^6 moles.
Using the ideal gas law PV = n*RT, where P is the pressure, V is the volume, n is the amount of the gas in moles, T is the temperature and R is a constant.
The required volume is: 3.791*10^6*62.36*292/758 L = 91.1*10^6 L
The volume of carbon dioxide released per hour by the power station is 91.1*10^6 L.
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