A 16.0 g sample of ice at -12.0°C is mixed with 120.0 g of water at 87.0°C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(l) are 2.08 and 4.18 J/g°C, respectively, and the enthalpy of fusion for ice is 6.02 kJ/mol.
2006-06-20 04:26:25 · 4 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
First, find the energy required to get the ice to 0 C:
mass of ice X (0 - temperature) X Heat capacity = Energy (ice)
Then, find the energy required to melt the ice:
convert the enthalpy of fusion to units of J/g, (you will need to determine the molar mass of water) and calculate
mass of ice X enthalpy of fusion = Energy (melt)
Add the energy from the ice and the energy of melting the ice together.
Energy (ice) + Energy (melt) = Energy (cold)
Energy (cold) / (mass of water X heat capacity of water) = temperature drop from 87 C.
2006-06-20 05:16:28 · answer #1 · answered by Anonymous · 0⤊ 0⤋
For 7. no longer some thing will ensue. 8. CaCO3 will precipitate 9. CuCl ought to precipitate, uncertain, lookup your solutbility table. 10. Acid base-make NaNO3 and water 11. i imagine of that reaction is composed of iron-chloride complexes, yet i'm uncertain 12. you receives some redox, chloride gasoline will take shipping of off and also you receives sulphuric acid.
2016-11-15 00:41:30 · answer #2 · answered by ? 4 · 0⤊ 0⤋
Sorry - I got a D in Chemistry last semester, therefore, I must repeat it.....
2006-06-20 06:30:44 · answer #3 · answered by Penny 3 · 0⤊ 0⤋
DO YOUR OWN HOMEWORK!!!!!!
2006-06-20 09:58:01 · answer #4 · answered by ? 3 · 0⤊ 0⤋