What is the heat of combustion of 1 mol of C4H10 in kJ/mol, if 1.041 g is burned and a calorimeter absorbs +51.0 kJ of heat?
qrxn= -q calorimeter =
-51.0 kJ --> -51.0 kJ/ 1.041 g C4H10 X 58.0 g C4H10/ 1 mol of C4H10 = -2841 kJ/mol C4H10
Everything make sense execept for the 58.0 grams. Where does it come from and how can I calculate it? Thank you!
2007-10-11 05:27:17 · 6 answers · asked by Jamie 3 in Science & Mathematics ➔ Chemistry
Because you have C4H10.
The atomic weight of carbon is 12 and hydrogen is 1. That's how many grams are in 1 mole of each.
C4H10 = (12)x4 + (1)x10 = 48 + 10 = 58 grams per mole
2007-10-11 05:33:24 · answer #1 · answered by Anonymous · 0⤊ 0⤋
58 grams/mol is the molecular weight of C4H10(butane)
C4H10 = 12(4) + 10 = 58
2007-10-11 05:33:11 · answer #2 · answered by Jr Levesque 2 · 0⤊ 0⤋
It's the molar mass of Butane (C4H10).
2007-10-11 05:36:26 · answer #3 · answered by BB 7 · 0⤊ 0⤋
I would say carry the 8
2007-10-11 05:30:10 · answer #4 · answered by Watch it bub! 3 · 0⤊ 0⤋
That's the molecular weight of butane.
2007-10-11 05:30:10 · answer #5 · answered by Fly On The Wall 7 · 0⤊ 0⤋
difficult aspect. lookup into the search engines. that will help!
2014-12-08 20:19:30 · answer #6 · answered by ? 3 · 0⤊ 0⤋