17. A solution of 75.0 mL of 3.20 M HNO3 was mixed with 50.0 mL of 2.00 M Ca(OH)2 in a large Styrofoam coffee cup; the cup is fitted with a lid through which a calibrated thermometer passes. The temperature of both solutions before mixing was 20.1 °C. After the Ca(OH)2 solution is added to the coffee cup and the mixed solutions are stirred with the thermometer, the maximum temperature measured was 39.2 °C. Assume that the volumes are additive but that the density of the mixed solution is 1.10 g/mL, the specific heat of the mixed solution is 4.18 J/g °C, and no heat is lost to the surroundings. In much the same way as you did for the previous question, calculate the enthalpy change per mole of HNO3 in the reaction. Consider that only reactants that actually react will account for the heat produced. The following problems are essentially calorimetry problems involving heat transfer from dissolving substances in water. Use the concept that the heat given off (or absorbed) by dissolving the substance equals the heat gained (or lost) by the water. In other words, start all problems with this equation: qsoln +9H20 = 0.

17. A solution of 75.0 mL of 3.20 M HNO3 was mixed with 50.0 mL of 2.00 M Ca(OH)2 in a large Styrofoam coffee cup; the cup is fitted with a lid through which a calibrated thermometer passes. The temperature of both solutions before mixing was 20.1 °C. After the Ca(OH)2 solution is added to the coffee cup and the mixed solutions are stirred with the thermometer, the maximum temperature measured was 39.2 °C. Assume that the volumes are additive but that the density of the mixed solution is 1.10 g/mL, the specific heat of the mixed solution is 4.18 J/g °C, and no heat is lost to the surroundings. In much the same way as you did for the previous question, calculate the enthalpy change per mole of HNO3 in the reaction. Consider that only reactants that actually react will account for the heat produced. The following problems are essentially calorimetry problems involving heat transfer from dissolving substances in water. Use the concept that the heat given off (or absorbed) by dissolving the substance equals the heat gained (or lost) by the water. In other words, start all problems with this equation: qsoln +9H20 = 0.

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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Question

17. A solution of 75.0 mL of 3.20 M HNO3 was mixed with 50.0 mL of 2.00 M Ca(OH)2 in a large
Styrofoam coffee cup; the cup is fitted with a lid through which a calibrated thermometer passes. The
temperature of both solutions before mixing was 20.1 °C. After the Ca(OH)2 solution is added to the
coffee cup and the mixed solutions are stirred with the thermometer, the maximum temperature measured
was 39.2 °C. Assume that the volumes are additive but that the density of the mixed solution is 1.10
g/mL, the specific heat of the mixed solution is 4.18 J/g °C, and no heat is lost to the surroundings.
In much the same way as you did for the previous question, calculate the enthalpy change per mole of
HNO3 in the reaction. Consider that only reactants that actually react will account for the heat produced.
The following problems are essentially calorimetry problems involving heat transfer from dissolving substances in
water. Use the concept that the heat given off (or absorbed) by dissolving the substance equals the heat gained (or
lost) by the water. In other words, start all problems with this equation: soln +9H20 = 0.

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