Ask your own question, for FREE!
Chemistry 71 Online
carlymiles12:

How much heat is evolved in converting 1.00 mol of steam at 160.0 ∘C to ice at -55.0 ∘C? The heat capacity of steam is 2.01 J/(g⋅∘C) and of ice is 2.09 J/(g⋅∘C).

Vocaloid:

divide this problem into steps: 1. cooling the steam from 160C to 100C 2. phase state change from steam to liquid water 3. cooling the liquid water from 100 to 0C 4. phase state change from liquid water to ice 5. cooling the ice from 0 to -55 for steps 1, 3, 5, the cooling steps without phase changes, you will simply use q = mCdeltaT where m is the mass, C is the specific heat (make sure to use the right C for each step, depending on what phase the water is in), and T is the temperature change for steps 2 and 4, the phase changes, you will simply multiply moles of water * molar heat of vaporization) for step 2, since we're going from steam to liquid or moles of water * molar heat of fusion for step 4, since we're going from liquid to ice after all the calculations are done simply add the results from steps 1-5, be ***very*** careful about units since molar heats are often in kJ/mol while specific heat is usu. in J/(g*C). also make sure not to confuse mass of water w/ moles of water.

Can't find your answer? Make a FREE account and ask your own questions, OR help others and earn volunteer hours!

Join our real-time social learning platform and learn together with your friends!
Can't find your answer? Make a FREE account and ask your own questions, OR help others and earn volunteer hours!

Join our real-time social learning platform and learn together with your friends!