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13 Dec 2019
A calorimeter contains 22.0mL of water at 11.0?C . When 2.30g of X (a substance with a molar mass of 42.0g/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, ?H, 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.
Express the change in enthalpy in kilojoules per mole to three significant figures.
A calorimeter contains 22.0mL of water at 11.0?C . When 2.30g of X (a substance with a molar mass of 42.0g/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, ?H, 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.
Express the change in enthalpy in kilojoules per mole to three significant figures.
Reid WolffLv2
17 Dec 2019