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If you combine 410.0 mL of water at 25.0°C and 130.0 mL of water at 95.0°C, what is the final temperature of the mixture, in °C? Assume: • No heat is lost to the surroundings. • The specific heat and density of water: 4.184 J g‍¹ ºC-1 and 0.997 g mL −1, respectively. a. 37.1 °C b. 41.9 °C c. 50.6 °C d. 66.8 °C e. 80.7 °C

If you combine 410.0 mL of water at 25.0°C and 130.0 mL of water at 95.0°C, what is the final temperature of the mixture, in °C? Assume: • No heat is lost to the surroundings. • The specific heat and density of water: 4.184 J g‍¹ ºC-1 and 0.997 g mL −1, respectively. a. 37.1 °C b. 41.9 °C c. 50.6 °C d. 66.8 °C e. 80.7 °C

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 50E: How much heat is produced when loo mL of 0.250 M HCl (density, 1.00 g/mL) and 200 mL of 0.150 M NaOH...
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If you combine 410.0 mL of water at 25.0°C and 130.0 mL of water at 95.0°C, what is the final temperature of the mixture, in °C? Assume: • No heat is lost to the surroundings. • The specific heat and density of water: 4.184 J g‍¹ ºC-1 and 0.997 g mL −1, respectively. a. 37.1 °C b. 41.9 °C c. 50.6 °C d. 66.8 °C e. 80.7 °C
Transcribed Image Text:If you combine 410.0 mL of water at 25.0°C and 130.0 mL of water at 95.0°C, what is the final temperature of the mixture, in °C? Assume: • No heat is lost to the surroundings. • The specific heat and density of water: 4.184 J g‍¹ ºC-1 and 0.997 g mL −1, respectively. a. 37.1 °C b. 41.9 °C c. 50.6 °C d. 66.8 °C e. 80.7 °C
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