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Moose100

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## Homework Statement

The Heat of combustion of Ethane is 373 kcal/mole. Assuming that 60% of the heat is useful , how many liters of ethane,, measured at standard temperature and pressure, must be burned to convert 50.0kg of water ar 10.0C to steam at 100.0C? One mole of a gas occupies 22.4 liters at precisely 0C and 1atm.

## Homework Equations

PV=nRT Q=mcΔT

## The Attempt at a Solution

Qburned=Q heat up

=mL + mcΔT

540g/C(50g)+ 50(1cal/gC)(100-10)

Q=31500 cal

n= Q/heat of combustion(60%)

n=0.1407mol

PV=nRT

V=0.1407mol(8314j/kmolK)(273K)/1atm

V=3193680 L

The book has it at 315000. Is there something wrong here? I feel like I am missing a term or left something out?