What would be the final temperature of the
system if 28.4 g of lead at 99.5 ◦C is dropped
into 14.0 g of water at 8.61 ◦C in an insulated
container? The specific heat of lead is 0.128
J/g◦C.
3 answers
Jane -- I can't help you -- except to say this looks like a homework dump. Many of our tutors stay far away from a bunch of questions posted by the same person.
I agree with Ms. Sue. If you will start at the first post, tell us what you think about each problem, tell us EXACTLY what you don't understand about the problem and how much you know how to do on your own, I'll be more than happy to help through each and every one.
This will help you through this one. The heat given up by lead to the water must equal to the heat absorbed by the water wo there is zero change. It looks this way.
[mass Pb x specific heat Pb x (Tfinal-Tinitial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0
You have mass Pb, specific heat Pb, you're look for Tfinal,you have Tinitial Pb and Tinitial H2O. I assume you know specific heat H2O.
Post your work if you get stuck.
[mass Pb x specific heat Pb x (Tfinal-Tinitial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0
You have mass Pb, specific heat Pb, you're look for Tfinal,you have Tinitial Pb and Tinitial H2O. I assume you know specific heat H2O.
Post your work if you get stuck.
1 answer