A quantity of 3.10 × 102 mL of 0.650 M HNO3 is mixed with 3.10 × 102 mL of 0.325 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 18.46°C. The heat of neutralization when 1.00 mol of HNO3 reacts with 0.500 mol Ba(OH)2 is −56.2 kJ/mol. Assume that the densities and specific heats of the solution are the same as for water (1.00 g/mL and 4.184 J/g ·°C, respectively). What is the final temperature of the solution?

Calculation of no. of mol of HNO3: Calculation of no. of mol of Ba(OH)2:

Answered: A quantity of 3.10 × 102 mL of 0.650 M…

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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A quantity of 3.10 × 10² mL of 0.650 M HNO₃is mixed with 3.10 × 10² mL of 0.325 M Ba(OH)₂

in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 18.46°C.

The heat of neutralization when 1.00 mol of HNO₃ reacts with 0.500 mol Ba(OH)2 is −56.2 kJ/mol.

Assume that the densities and specific heats of the solution are the same as for water (1.00 g/mL and 4.184 J/g ·°C, respectively). What is the final temperature of the solution?

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