Calculate Total Heat For A T Change/Phase Transition Sequence
From the following data, calculate the total heat needed to convert 0.219 mol ice at -6.50°C to liquid water at 7.26°C.
Melting point at 1 atm0°C
csolid2.09J/g°C
cliquid4.21J/g°C
ΔHfus6.02 kJ/mol
2007-01-16 05:44:43 · 2 answers · asked by Tanya s 1 in Science & Mathematics ➔ Chemistry
Start with csolid to get from -6.5C to 0C
Use delta Hfus to turn solid to liquid
Use cliquid to heat liquid to 7.26C
Add all the kJs to get total
2007-01-16 06:17:58 · answer #1 · answered by teachbio 5 · 0⤊ 0⤋
get waiting!! ive basically merely began my anthralpy exchange in chemistry so this may be relatively incorrect yet the two way curiously sturdy hehe!! mxc(L)x(t2-t1) this might supply us the anthralpy exchange of the heating exchange whilst it is a liquid.. figuring out the mass! water is H2O there fore 2X1 + sixteen equals 18 that's the molcular mass.. mass -> form of moles X molcular mass 2.09 X 18.00 equals 3.ninety 4 save to an identical sig figs! this provides us the mass then plug it in alongside with the proper particular warmth capacity and the pace exchange then upload the surprising 2 3.ninety two*2.09*6.50-> fifty 3.55KjKmol-a million 3.ninety two*4.21*7.26-> one hundred twenty.49KjKmol-a million entire Enthalpy exchange 174.04KjKmol-a million
2016-12-16 06:05:20 · answer #2 · answered by lacross 4 · 0⤊ 0⤋