0.32g (0.010mol) of methanol was burned to heat up 200g of water the temp of water rose by 40 degree what was the enthalpy change per mole?

can anyone explain step by step including the conversion to kjmol-1 at the end if that's needed 

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  • 2 months ago
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    Calculate the amount of energy absorbed by the water, which is also the amount of energy produced by the combustion.

    (4.184 J/g·°C) x (200 g) x (40°C) = 33472 J = 33.472 kJ absorbed by the water

    Calculate how much energy is produced per mole of methanol.

    (33.472 kJ) / (0.010 mol) = 3347 kJ/mol

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