Question 1 please 1. In determining the calorimeter constant, a student added 50.00 mL H₂O at 48.5°C to 50.00mL H₂O at 23.2°C in a calorimeter. The temperature of the mixture was 35.4°C. Calculate thecalorimeter constant given that the density of H₂O is 1.00 g/mL and the specific heat capacityof water is 4.18J/g °C.2. A student mixed 50.00 mL of 1.00 M HCl at 20.5 °C with 50.00 mL of 1.00 M NH3 at20.5 °C. After mixing, the temperature rose to 26.6 °C. The calorimeter constant had beendetermined to be 18.0 J/°C. Assume the density and specific heat capacity of the solution arethe same as water, 1.00 g mL-¹ and 4.18 J g-¹ °C-¹, respectively.a)b)Calculate the enthalpy of neutralization in kJ per mole NH3 consumed.Is this reaction endothermic or exothermic?

Answered: Image /qna-images/answer/0bfd8b37-4aec-4424-8aba-4e33a20c05c7.jpg

1. In determining the calorimeter constant, a student added 50.00 mL H₂O at 48.5°C to 50.00 mL H₂O at 23.2°C in a calorimeter. The temperature of the mixture was 35.4°C. Calculate the calorimeter constant given that the density of H₂O is 1.00 g/mL and the specific heat capacity of water is 4.18J/g °C.

1. In determining the calorimeter constant, a student added 50.00 mL H₂O at 48.5°C to 50.00 mL H₂O at 23.2°C in a calorimeter. The temperature of the mixture was 35.4°C. Calculate the calorimeter constant given that the density of H₂O is 1.00 g/mL and the specific heat capacity of water is 4.18J/g °C.

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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