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1. How much energy is required to raise 125 grams of water from 22.0 °C to 43.2 °C? The M.S.AT specific heat (S) of water is 1.000 cal/g °C.

1. How much energy is required to raise 125 grams of water from 22.0 °C to 43.2 °C? The M.S.AT specific heat (S) of water is 1.000 cal/g °C.

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter12: Thermodynamic Processes And Thermochemistry
Section: Chapter Questions
Problem 15P
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At=trinal-t AT=(43.2-22) 21.2°C PRELAB QUESTIONS: S=1.00 cal/19°C 1. How much energy is required to raise 125 grams of water from 22.0 °C to 43.2 °C? The specific heat (S) of water is 1.000 cal/g °C. M.S.AT 125 g x 1.0 Cal дос x 21.2°C (tinitial) 9=12650 cal 2. An almond weighs 0.823 grams. When the almond is burned in a calorimeter that contains 124.2 grams of water, the water temperature changes from 23.5 °C to 45.7 °C. The water MSDT "uncombusted remains" of the almond weighs 0.615 grams. Q: amount of heat absorted by liquid a) Calculate the change in temperature (AT) of the water. iwater mi mass of liquid water T₁=23.52 TO US.TC T₂-1₁ = 45.7°C-235° = 22.2°C ● m=1259 Ti=22.0°C te=43.2°C. b) Calculate the amount of energy that was released from the almond sample. Assume that all of the energy released from the almond was transferred to the water. Specific teat liquid watter,s: 1.00 cal/g °C AT:22.2°C Q=M.SOT Massliquid 1₂0,m: 1242 Use the specific heat (S) of water (1.000 cal/g °C), the mass of the water that was in the flask, and the temperature change (AT) of the water to calculate the amount of energy (Q) that was transferred to the water, and thus the amount of energy that was Qalmond-quater released from almond. = 2757,24 cal =-2757 cal amount of heat released from almond is 2757 calories =2757.24 cal c) Calculate the mass of the almond that was "completely combusted". This is done by subtracting the mass of "uncombusted remains" of the almond from the original mass of the almond. 124.2g x1.000 si specific heat of liquid water. AT: Change in temper" Cal 9°C X22.2°C Original mass of almond: 0.8239 Mass of uncombusted of almond: 0.6159 Mass of completely combusted of almond: 0.8239-0.6159 = 0.208 d) Calculate the energy per gram of almonds by dividing the energy that was released from the almond (from part b) by the mass of the almond that was "completely combusted" (from part c). Gl Amount of heat released from almond q almond: 2757 mass of completely combusted of almond: 0.208g DH=2757 Cal 0.2089 -13255.cal/g -1.32x10¹ cal/g 2
Transcribed Image Text:At=trinal-t AT=(43.2-22) 21.2°C PRELAB QUESTIONS: S=1.00 cal/19°C 1. How much energy is required to raise 125 grams of water from 22.0 °C to 43.2 °C? The specific heat (S) of water is 1.000 cal/g °C. M.S.AT 125 g x 1.0 Cal дос x 21.2°C (tinitial) 9=12650 cal 2. An almond weighs 0.823 grams. When the almond is burned in a calorimeter that contains 124.2 grams of water, the water temperature changes from 23.5 °C to 45.7 °C. The water MSDT "uncombusted remains" of the almond weighs 0.615 grams. Q: amount of heat absorted by liquid a) Calculate the change in temperature (AT) of the water. iwater mi mass of liquid water T₁=23.52 TO US.TC T₂-1₁ = 45.7°C-235° = 22.2°C ● m=1259 Ti=22.0°C te=43.2°C. b) Calculate the amount of energy that was released from the almond sample. Assume that all of the energy released from the almond was transferred to the water. Specific teat liquid watter,s: 1.00 cal/g °C AT:22.2°C Q=M.SOT Massliquid 1₂0,m: 1242 Use the specific heat (S) of water (1.000 cal/g °C), the mass of the water that was in the flask, and the temperature change (AT) of the water to calculate the amount of energy (Q) that was transferred to the water, and thus the amount of energy that was Qalmond-quater released from almond. = 2757,24 cal =-2757 cal amount of heat released from almond is 2757 calories =2757.24 cal c) Calculate the mass of the almond that was "completely combusted". This is done by subtracting the mass of "uncombusted remains" of the almond from the original mass of the almond. 124.2g x1.000 si specific heat of liquid water. AT: Change in temper" Cal 9°C X22.2°C Original mass of almond: 0.8239 Mass of uncombusted of almond: 0.6159 Mass of completely combusted of almond: 0.8239-0.6159 = 0.208 d) Calculate the energy per gram of almonds by dividing the energy that was released from the almond (from part b) by the mass of the almond that was "completely combusted" (from part c). Gl Amount of heat released from almond q almond: 2757 mass of completely combusted of almond: 0.208g DH=2757 Cal 0.2089 -13255.cal/g -1.32x10¹ cal/g 2
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