Do you want enthalpy/grams or enthalpy/mol. Most prefer it to be kJ/mol.
q = g H2O x specific heat H2O x (Tfinal-Tinitial)
That gives you q/2.30g X = ? J/g
If you want J/mol it is J/g x 82.0 = ? J/mol. You can change that to kJ/mol if you wish.
A calorimeter contains 32.0mL of water at 13.0∘C . When 2.30g of X (a substance with a molar mass of 82.0g/mol is added, it dissolves via the reaction
X(s)+H2O(l)�¨X(aq)
and the temperature of the solution increases to 30.0∘C .
Calculate the enthalpy change, ĢH for this reaction per mole of X .
Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C) ], that density of water is 1.00 g/mL , and that no heat is lost to the calorimeter itself, nor to the surroundings.
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