If 1.10 g of steam at 100.0 degrees celsius condenses into 38.5 g of water, initially at 27.0 degrees celsius, in an insulated container, what is the final temperature of the entire water sample? Assume no loss of heat into the surroundings
Chemistry - DrBob222, Tuesday, November 9, 2010 at 12:34am
heat lost by 100 C water + heat gained by cold water - heat lost by condensation =0
1.1*4.184*(Tf-100) +[38.5*4.184*(Tf-27)] - 1.1*2257 = 0
Solve for Tf.
You can do it another way if you wish.
First calculate how much the condensing steam will raise the T of cold water.
1.1*2257 = 2482.7 J released.
38.5*4.184*(Tf-27) = 2482.7
Tf = 42.41 THEN
heat lost by 1.1g steam @ 100C + heat gained by 41.41 C water = 0 and recalculate Tf EXCEPT, of course, Tinitial is 42.41 and not 27.0 C. Same answer is obtained.
Chemistry - Please Help!, Tuesday, November 9, 2010 at 9:14pm
Thank you! what is the 2257 from?
Chemistry - Chandler, Tuesday, November 4, 2014 at 12:07pm
2257 is the heat of vaporization of water.