Posted by **Selena** on Sunday, January 29, 2012 at 4:52pm.

An 850 gram chunk of ice at 0 degrees Celsius is dropped into a container holding 1.7 kg of water at an initial temperature of 35 degrees Celsius. Due to the presence of the ice, the temperature of the water eventually drops to 0 degrees Celsius. Show a mathematical solution to answer this question:

Does the 850 gram chunk of ice completely melt?

Formulas: Q= mHf Q=mHv Q= m∆TCp

The specific heat of liquid is 4.18J/gᵒC

The specific heat of solid water (ice) is 2.11J/gᵒC

The heat energy released during melting is 334J/g

- Chemistry -
**DrBob222**, Sunday, January 29, 2012 at 5:07pm
heat to melt ice at zero C = 850 x heat fusion = ?

heat removed from 35 C water = 1,700 x specific heat water x (0-35) = ?

I get about 280,000 J to melt the ice and about 250,000 J from the water. The ice won't melt completely. The end solution will be a mixture of ice and water at zero C. You can calculate how much ice is left if you wish. There is enough data to do that.

- Chemistry -
**Selena**, Sunday, January 29, 2012 at 7:43pm
Could you please prove how the ice doesn't completely melt? Don't you subtract 280,000 J and 250,000 J and get 30,000 J? and then you divide it by 334 J/g and get 105 g? But I don't know what you do next.

- Chemistry -
**DrBob222**, Sunday, January 29, 2012 at 8:48pm
I caution you not to use my estimates. Those are just close numbers; you need to run them yourself.

What I did above SHOWS that the ice doesn't completely melt. Yes, you subtract 280,000 - 250,000 and show that you are 30,000 J short of having enough heat to melt all of the ice. I don't think anything else is necessary. Again, that 30,000 is an estimate. You need to run that number too.

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