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Question about Problem 8.41

Posted: Sun Jan 14, 2018 9:40 pm
by Isa Samad 1L
In the solutions manual, the answer uses the equation -q(water) = q(ice). Is this because the ice is lowering the temperature of the water?

Re: Question about Problem 8.41

Posted: Sun Jan 14, 2018 9:46 pm
by Ashin_Jose_1H
Yeah. The heat from the water is transferred to the ice.

Re: Question about Problem 8.41

Posted: Thu Jan 18, 2018 10:27 am
by Erica Nagase 1H
The liquid water will lose heat and its temperature will decrease, and the ice will absorb that heat and melt/temperature will increase. This is why the q(water) is negative and q(ice) is positive.

Re: Question about Problem 8.41

Posted: Thu Jan 18, 2018 10:35 am
by Johann Park 2B
Yes, in thermodynamics we must remember that energy is conserved and that qsys + qsurr = 0, and thus qsys = -qsurr; the system being the ice and the surroundings being the water.

Re: Question about Problem 8.41

Posted: Thu Jan 18, 2018 12:00 pm
by Meredith Steinberg 2E
Yes because there is a transfer of heat from the water to the ice

Re: Question about Problem 8.41

Posted: Thu Jan 18, 2018 12:09 pm
by Ashley Macabasco 2K
In the solution manual -q(water)=q(ice) illustrates that heat from water is being transferred exothermically to the ice shown with the lose of heat (-q). The ice is then gaining heat endothermically from the water which can also be seen with q being positive for ice.