33.6 L of CH4 are combusted under a dish containing ice. change in Hrxn for the combustion of CH4 is -802kJ/mol. How many grams of ice can you melt if none of the heat is lost to the environment? (change Hfus=6.00 kJ/mol)
is this how u do it? can u do it for me?
Calculate how many moles are in 33.6 L.
Moles X 802kJ/mol = total heat.
Total heat / 6.00 kJ/mol = moles of ice
moles of ice X mol wt. of ice = grams of ice melted
2007-12-11 15:23:17 · 2 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
Heat released in burning = heat used in melting ice
I presume that the CH4 is at 1 atm.
You need to find the number of moles of CH4. Do this using either PV = nRT, or the fact that 1 mol at STP occupies 22.4L.
Heat released per mol x number of mols = total heat released.
Divide that by the heat of fusion of ice (6.00 kJ/mol) to get the number of moles ice melted.
Finally, if you want g ice, multiply moles ice by the formula weight of ice.
Yes I can do it for you, but that would be completely pointless so I won't.
2007-12-11 22:07:52 · answer #1 · answered by Facts Matter 7 · 0⤊ 0⤋
You did it for yourself. The only hangup is to specify the pressure of the methane (it is a gas).
2007-12-11 23:35:23 · answer #2 · answered by cattbarf 7 · 0⤊ 0⤋