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Question 4C.11

Posted: Sun Feb 02, 2020 3:30 pm
by Brittney Hun 2C
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?

Re: Question 4C.11

Posted: Sun Feb 02, 2020 4:00 pm
by Jacey Yang 1F
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.

Re: Question 4C.11

Posted: Mon Feb 03, 2020 7:21 pm
by Brittney Hun 2C
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?

Re: Question 4C.11

Posted: Wed Feb 05, 2020 1:19 am
by Jessica Chen 2C
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.

Re: Question 4C.11

Posted: Wed Feb 05, 2020 3:37 pm
by Morgan Carrington 2H
When finding the value of q, would you use the specific heat for liquid water or solid water?