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.