0.100 moles of an acid is mixed with 0.100 moles of a base in a calorimeter and the temperature of 85.0 g of the resulting solution increases from 23.3°C to 34.5°C. If the specific heat of the solution is 1.00 cal/g °C, what is the quantity of energy released or absorbed by the reaction? A) 952 cal released B)683 cal absorbed C)952 cal absorbed D)683 cal released E)95.2 cal absorbed
0.100 moles of an acid is mixed with 0.100 moles of a base in a calorimeter and the temperature of 85.0 g of the resulting solution increases from 23.3°C to 34.5°C. If the specific heat of the solution is 1.00 cal/g °C, what is the quantity of energy released or absorbed by the reaction? A) 952 cal released B)683 cal absorbed C)952 cal absorbed D)683 cal released E)95.2 cal absorbed
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section5.6: Calorimetry
Problem 5.7CYU: Assume 200. mL of 0.400 M HCl is mixed with 200. mL of 0.400 M NaOH in a coffee-cup calorimeter The...
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0.100 moles of an acid is mixed with 0.100 moles of a base in a calorimeter and the temperature of 85.0 g of the resulting solution increases from 23.3°C to 34.5°C. If the specific heat of the solution is 1.00 cal/g °C, what is the quantity of energy released or absorbed by the reaction?
A) 952 cal released
B)683 cal absorbed
C)952 cal absorbed
D)683 cal released
E)95.2 cal absorbed
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