Question

When 0.187 g of benzene, C6H6, is burned in a bomb calorimeter, the surrounding water bath rises in temperature by 7.48 ∘C. Assuming that the bath contains 250.0 g of water and that the calorimeter itself absorbs a negligible amount of heat, calculate combustion energies (ΔE) for benzene in both kilojoules per gram and kilojoules per mole.

Answer 1

q=m*c*dT

Answer 2

C is specific heat capacity

Answer 3

what does it have to do with dE?

Answer 4

should the answer be 1.39?

Answer 5

find the heat released by the the combustion of benzene using the equation, in this case q=E, because heat IS energy.

Answer 6

could you answer this question...Liquid butane (C4H10), the fuel used in many disposable lighters, has ΔH∘f=−147.5 kJ/mol and a density of 0.579 g/mL. Use Hess’s law to calculate the enthalpy of combustion in kJ/mol.

Answer 7

since q(benzene)=q(water), you need only to use the temperature difference, the mass of the water and the heat capacity of the water.

once you find q, you divide by the mass of benzene you used to find the units in J/g
then convert the mass to moles and divide q by the moles to get J/mol units.

Answer 8

write a balanced equation first

Answer 9

yes...what do i do next??

Answer 10

you use Hess's law:

dH(rxn)=Hf(prod)-Hf(reactants)

Answer 11

the Hf of h2o and co2 are not given

Answer 12

you have to look them up in your book