3. The amount of energy needed to raise the temperature of one gram of substance by one degree is called its specific heat. For example, the specific heat of water can be expressed as 1.00 calorie /g°C (or 4.18 Joules/g®C) whereas the specific heat of and 2 units in the denominator glass is 0.20 calorie/g C (or 0.84 Joules/g C).. Whenever a substance is heated from a lower to higher temperature, or vice versa, the amount of energy absorbed from the surroundings (to heat it) or released to the surroundings (as it cools) can be calculated by this general formula: Note: There are 3 units required for specific heat: one unit in the numerator (calorie or Joules) (grams and Celsius). energy exchanged - (mass of substance)(specific heat)(temperature change) The temperature change, usually called delta-T or "AT" is simply the final temperature minus the initial temperature: AT -Ttal - Tiatat where Tnal is the final temperature, and T mnial is the initial temperature. Note that AT can be either nositive or negative. When water is being considered, and we use units of calories, the equation becomes: 1.00 cal calories exchanged = mass x × (AT) Let us calculate the number of heat calories absorbed by the water from the Bunsen burner when you boiled it in Step I above. We will assume that the water started out at room temperature (evèn though that might not really be the case). (d) AT= (d) AT- °C- °C- °C (e) If the density of water is 1.00 g/mL., what is the mass of the water you used for boiling? () grams Show your work here: () calories () Using your calculated values from parts (d) and (e), determine the number of calories absorbed by your heated water: 1.00 cal grams of water x "C - g °C cal
3. The amount of energy needed to raise the temperature of one gram of substance by one degree is called its specific heat. For example, the specific heat of water can be expressed as 1.00 calorie /g°C (or 4.18 Joules/g®C) whereas the specific heat of and 2 units in the denominator glass is 0.20 calorie/g C (or 0.84 Joules/g C).. Whenever a substance is heated from a lower to higher temperature, or vice versa, the amount of energy absorbed from the surroundings (to heat it) or released to the surroundings (as it cools) can be calculated by this general formula: Note: There are 3 units required for specific heat: one unit in the numerator (calorie or Joules) (grams and Celsius). energy exchanged - (mass of substance)(specific heat)(temperature change) The temperature change, usually called delta-T or "AT" is simply the final temperature minus the initial temperature: AT -Ttal - Tiatat where Tnal is the final temperature, and T mnial is the initial temperature. Note that AT can be either nositive or negative. When water is being considered, and we use units of calories, the equation becomes: 1.00 cal calories exchanged = mass x × (AT) Let us calculate the number of heat calories absorbed by the water from the Bunsen burner when you boiled it in Step I above. We will assume that the water started out at room temperature (evèn though that might not really be the case). (d) AT= (d) AT- °C- °C- °C (e) If the density of water is 1.00 g/mL., what is the mass of the water you used for boiling? () grams Show your work here: () calories () Using your calculated values from parts (d) and (e), determine the number of calories absorbed by your heated water: 1.00 cal grams of water x "C - g °C cal
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Transcribed Image Text:3. The amount of energy needed to raise the temperature of one
gram of substance by one degree is called its specific heat. For
example, the specific heat of water can be expressed as
1.00 calorie /g°C (or 4.18 Joules/g°C) whereas the specific heat of and 2 units in the denominator
glass is 0.20 calorie/g°C (or 0.84 Joules/g C).
Whenever a substance is heated from a lower to higher
temperature, or vice versa, the amount of energy absorbed from
the surroundings (to heat it) or released to the surroundings (as it
cools) can be calculated by this general formula:
Note: There are 3 units required
for specific heat: one unit in the
numerator (calorie or Joules)
(grams and Celsius).
energy exchanged - (mass of substance)(specific heat(temperature change)
The temperature change, usually called delta-T or "AT" is simply
the final temperature minus the initial temperature:
AT - T fnal - Tinitial
where T final is the final temperature, and Tial is the initial
temperature. Note that AT can be either nositive or negative.
When water is being considered, and we use units of calories, the
equation becomes:
1.00 cal
-((AT)
g °C
calories exchanged = mass x
Let us calculate the number of heat calories absorbed by the water
from the Bunsen burner when you boiled it in Step I above. We will
assume that the water started out at room temperature (evèn though
that might not really be the case).
(d) AT =
C
(d) AT-
°C -
°C =
°C
(e) If the density of water is 1.00 g/mL, what is the mass of the
water you used for boiling?
(e).
grams
Show your work here:
(1)
calories
(1) Using your calculated values from parts (d) and (e), determine
the number of calories absorbed by your heated water:
1.00 cal
grams of water x
°C =
8 °C
cal
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