A calorimeter contains 30.0 mL of water at 14.0 °C. When 1.70 g of X (a substarice with a molar mass of 76.0 g/mol ) is added, it dissolves via the reaction X(s) + H20(1)-X(aq) and the temperature of the solution increases to 30.0 C Calculate the ethalpy change, AH, 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 30.0 mL of water at 14.0 °C. When 1.70 g of X (a substarice with a molar mass of 76.0 g/mol ) is added, it dissolves via the reaction X(s) + H20(1)-X(aq) and the temperature of the solution increases to 30.0 C Calculate the ethalpy change, AH, 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.
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter9: Energy And Chemistry
Section: Chapter Questions
Problem 9.101PAE
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