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: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter8: Thermochemistry
Section: Chapter Questions
Problem 80QAP: Equal masses of liquid A, initially at 100C, and liquid B, initially at 50C, are combined in an...
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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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F48a6e007-582f-4184-a15e-8474ea605642%2Fa7ea73f4-24bb-4f9b-9b3c-75c863d47eca%2Fb2sq68_processed.png&w=3840&q=75)
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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