Question 4C.11

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Brittney Hun 2C
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Joined: Wed Sep 11, 2019 12:15 am

Question 4C.11

Postby Brittney Hun 2C » Sun Feb 02, 2020 3:30 pm

The problem is: how much heat is needed to convert 80.0 g of ice at 0.0 8C into liquid water at 20.0 8C? It says to use the table 4A.1 and 4A.C but I'm unsure of what information I need. The water is turning from solid to liquid, which is fusion. The enthalpy for the fusion of water is already given, but how does the 80.0g play a role?

Jacey Yang 1F
Posts: 101
Joined: Fri Aug 09, 2019 12:17 am

Re: Question 4C.11

Postby Jacey Yang 1F » Sun Feb 02, 2020 4:00 pm

Use Table 4C.1 to find the enthalpy of fusion of water. Convert 80.0 grams of ice to moles and multiply by the enthalpy of fusion to get the heat needed to melt the ice. Then, use 80.0 g in the equation q= mCΔT to find the heat needed to raise the temperature from 0 to 25 degrees C.

Brittney Hun 2C
Posts: 104
Joined: Wed Sep 11, 2019 12:15 am

Re: Question 4C.11

Postby Brittney Hun 2C » Mon Feb 03, 2020 7:21 pm

Jacey Yang 1F wrote:Use Table 4C.1 to find the enthalpy of fusion of water. Convert 80.0 grams of ice to moles and multiply by the enthalpy of fusion to get the heat needed to melt the ice. Then, use 80.0 g in the equation q= mCΔT to find the heat needed to raise the temperature from 0 to 25 degrees C.


Do you know why the solution manual says to add the two energies together?

Jessica Chen 2C
Posts: 103
Joined: Thu Jul 11, 2019 12:17 am

Re: Question 4C.11

Postby Jessica Chen 2C » Wed Feb 05, 2020 1:19 am

You need to add the energy required to melt the ice cube to the energy required to raise the temperature of the (liquid) water in order to get the total energy that needs to be used in this process.

Morgan Carrington 2H
Posts: 54
Joined: Wed Nov 14, 2018 12:22 am

Re: Question 4C.11

Postby Morgan Carrington 2H » Wed Feb 05, 2020 3:37 pm

When finding the value of q, would you use the specific heat for liquid water or solid water?


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