Can anyone help me out with this: In a coffe-cup clorimeter, 125 mL of a 2.75 M solution of silver nitrate at 25.00 degrees C is comined with 350 mL of a 4.00 M strontium chloride solution, aslo at 25.00 C. The temperature of the final solution is 32.15 degrees C. If the density of the final solution is 1.25 g/mL and the heat cpacity of the final solution is 4.33 J/C*g, calculate delta H of silver chloride formed.
Any help would be highly apreciated, even if its just giving me a push in the right direction.
2007-04-13 07:39:17 · 1 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
How do I calculate the moles AgCl? I've calculated the moles of AgNo3 & moles of SrCl2. I'm still a bit confused. Thanks for your help though.
2007-04-14 11:38:35 · update #1
Heat = mass * 4.33*(32.15-25)
Now find the moles of AgCl formed.
2007-04-13 19:45:33 · answer #1 · answered by ag_iitkgp 7 · 0⤊ 1⤋