Enthalpy change

Hello, got this question that didn't have the answer to it in the back of the textbook, so I just wanna know if I'm right. :-)

"In a laboratory experiment, 1.16g of an organic liquid fuel was completely burned in oxygen. The heat formed during this combustion raised the temperature of 100g of water from 295.3K to 3578K. Calculate the standard enthalpy of combustion, delta H, of fuel. It's Mr is 58"

So my working was:

heat transferred = mc(delta t) = 100 x 4.2 x 62.5 = 26250

no. of moles = mass / mr = 1.16 / 58 = 0.02

delta H = heat transferred / no. of moles
= 26250 / 0.02
= 1312500 kJ / mol

Is this correct? Thank you.

Quote:

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Originally Posted by yorkey

Hello, got this question that didn't have the answer to it in the back of the textbook, so I just wanna know if I'm right. :-)

"In a laboratory experiment, 1.16g of an organic liquid fuel was completely burned in oxygen. The heat formed during this combustion raised the temperature of 100g of water from 295.3K to 3578K. Calculate the standard enthalpy of combustion, delta H, of fuel. It's Mr is 58"

So my working was:

heat transferred = mc(delta t) = 100 x 4.2 x 62.5 = 26250

no. of moles = mass / mr = 1.16 / 58 = 0.02

delta H = heat transferred / no. of moles
= 26250 / 0.02
= 1312500 kJ / mol

Is this correct? Thank you.

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If the temp change was 295.3K to 3578K
then delta T won't be 62.5K
>>

You forgot to change the mass of water to kg
and the ans that you will get should be -ve (opposite to the amount of heat energy that is taken is by water)

So the final ans should be -1312.5 KJ/mol (assuming that delta t is 62.5K)