It's a question in m revision book, that I have no idea about how to do it (I've looked in my books and I can find nothing abut concentration)...
"The temperature rose when excess zinc was added to copper sulphate solution was found to be 10degreesC. If the concentration of the copper sulphate solution was 0.1moldm-3 what would the enthalpy change of the reaction be?
"The temperature rose when excess zinc was added to copper sulphate solution was found to be 10degreesC. If the concentration of the copper sulphate solution was 0.1moldm-3 what would the enthalpy change of the reaction be?
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Let's assume we have 1.00 L of solution on hand and that it is composed of 1000 g of water in addition to the 0.1 mole of dissolved CuSO4.
q = (1000 g) (10 C) (4.184 J/g C) = 41840 J = 41.840 kJ
ΔH = 41.840 kJ / 0.1 mol = -418.4 kJ/mol
I added the minus sign since this is an exothermic reaction.
q = (1000 g) (10 C) (4.184 J/g C) = 41840 J = 41.840 kJ
ΔH = 41.840 kJ / 0.1 mol = -418.4 kJ/mol
I added the minus sign since this is an exothermic reaction.