A calorimeter contains 18.0 mL of water at 14.0 °C. When 1.30 g of X (a substance with a molar mass of 74.0 g/mol ) is added, it dissolvesvia the reactionX(s) + H,O(1)→X(aq)and the temperature of the solution increases to 29.0 °CCalculate the enthalpy 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 noheat 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 is an insulated device in which a chemicalreaction is contained. By measuring the temperature change,AT, we can calculate the heat released or absorbed duringthe reaction using the following equation:q= specific heat x mass × ATOr, if the calorimeter has a predetermined heat capacity, C,the equation becomesq=C x ATAt constant pressure, the enthalpy change for the reaction,AH, is equal to the heat, qp, that is,AH= 4pbut it is usually expressed per mole of reactant and with asign opposite to that of q for the surroundings. The totalinternal energy change, AE (sometimes referred to asAU), is the sum of heat, q, and work done, wAE=q+wHowever, at constant volume (as with a bomb calorimeter)W-0 and so AE= qu.

Volume of water = 18 mLDensity Of water =1.00 g/mLMass of water = Volume of water * Density of…

A calorimeter contains 18.0 mL of water at 14.0 °C. When 1.30 g of X (a substance with a molar mass of 74.0 g/mol ) is added, it dissolves via the reaction X(s) + H,O(1)→X(aq) and the temperature of the solution increases to 29.0 °C. Calculate the enthalpy 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.

A calorimeter contains 18.0 mL of water at 14.0 °C. When 1.30 g of X (a substance with a molar mass of 74.0 g/mol ) is added, it dissolves via the reaction X(s) + H,O(1)→X(aq) and the temperature of the solution increases to 29.0 °C. Calculate the enthalpy 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.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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