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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: Matchu on November 07, 2018, 04:42:22 PM

Title: Calotemitry problem
Post by: Matchu 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.
Title: Re: Calotemitry problem
Post by: billnotgatez on November 07, 2018, 05:40:10 PM
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Title: Re: Calotemitry problem
Post by: Matchu 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.
Title: Re: Calotemitry problem
Post by: mjc123 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)