Posted by **Please Help!** on Monday, November 8, 2010 at 11:57pm.

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.

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