2. An almond weighs 0.823 grams. When the almond is burned in a calorimeter that co 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 absorbed by liquid iwater a) Calculate the change in temperature (AT) of the water. 2 m: mass of liquid water s specific heat of liquid water AT: Change in temper" 5.7°C-235%= 22.2°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. M:R42 Use the specific heat (S) of water (1.000 cal/g °C), the mass of the water that was in watters: the flask, and the temperature change (AT) of the water to calculate the amount of energy (0) that was transferred to the water, and thus the amount of energy that was Qalmond-q water released from almond. Cal 2g x1.000 9°C X22.2°C ● =2757.21 cal =1-2757 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. Massot uncombusted of almond: 0.615- Original mass of almond; 0.8239 Mass of completely combusted of almond: 0.8239-0.6159
2. An almond weighs 0.823 grams. When the almond is burned in a calorimeter that co 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 absorbed by liquid iwater a) Calculate the change in temperature (AT) of the water. 2 m: mass of liquid water s specific heat of liquid water AT: Change in temper" 5.7°C-235%= 22.2°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. M:R42 Use the specific heat (S) of water (1.000 cal/g °C), the mass of the water that was in watters: the flask, and the temperature change (AT) of the water to calculate the amount of energy (0) that was transferred to the water, and thus the amount of energy that was Qalmond-q water released from almond. Cal 2g x1.000 9°C X22.2°C ● =2757.21 cal =1-2757 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. Massot uncombusted of almond: 0.615- Original mass of almond; 0.8239 Mass of completely combusted of almond: 0.8239-0.6159
Chemistry
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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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will you help me with number 2 questions, please?
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
124.2g x1.000
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.
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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