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#### Matchu

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##### Calotemitry problem
« on: November 07, 2018, 04:42:22 PM »

A student conducts an experiment to determine the enthalpy of a solution for lithium chloride dissolved in water. The student combines 5 grams of lithium chloride with 100 ml of distilled water. The initial temperature of the water is 23°C and the highest the temperature after mixing reached was 33°C. Assume a density of 1 g/ml and a specific heat of 4.18. The calorimeter constant is 20. What is the energy change of the solution and calorimeter and what is the total ΛH of the solution in kJ/mol.
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#### billnotgatez

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##### Re: Calotemitry problem
« Reply #1 on: November 07, 2018, 05:40:10 PM »

You have to show your attempts or thoughts at solving the question to receive help.
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http://www.chemicalforums.com/index.php?topic=65859.0
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#### Matchu

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##### Re: Calotemitry problem
« Reply #2 on: November 08, 2018, 02:15:43 AM »

Oh, oops sorry I'm new and must not have seen that. So far on this question I have tried using the ΛH=mcpΛT formula by plugging in change in temperature, mass, and the specific heat to get .4389 kJ. But, I am unsure on where to go from there.
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#### mjc123

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##### Re: Calotemitry problem
« Reply #3 on: November 08, 2018, 05:25:40 AM »

Show your working, so we can see where you went wrong (yes, it's wrong).
What is the sign of ΔH? (BTW, not ΛH)
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