What is the amount of heat, in calories, given off from a 5 g piece of...
What is the amount of heat, in calories, given off from a 5 g piece of aluminum when it cools from 80°C to 20°C? The specific heat capacity of aluminum is 0.215 cal/g∙°C. Show your work.
Homework Answers
Heat, Q = m C dT
Q = 0.005 x 0.215 x (80 - 20)
Q = 0.0645 calories
Comment in case any doubt please rate my answer....
Add Answer to:
What is the amount of heat, in calories, given off from a 5 g piece of...
1. Calculate the heat (expressed in calories) required to heat 115 g of water from 15.4^C...
1. Calculate the heat (expressed in calories) required to heat 115 g of water from 15.4^C to 91.4^C 2. Calculate the heat (in calories) lost by 115 g of water as it cools from 91.4^C to 15.4^C 3. Calculate the temperature change caused by absorption of 3.85 kcal heat by 75.4 g water 4. Calculate the final temperature of 75.4 g of water originally at 12.6^C after it absorbs 3.85 kcal of heat 5. A 23.9 g piece of metal...
7. Calculation of the Amount of Energy Given Off in a Combustion Reaction Section PreLab Questions...
7. Calculation of the Amount of Energy Given Off in a Combustion Reaction Section PreLab Questions 1. Aluminum has a specific heat of 0.902 J/g x °C. How much heat is lost when a piece of aluminum with a mass of 23.984 g cools from a temperature of 415.0 °C to a temperature of 22.0 °C? = 8.50215 2. The temperature of a sample of water increases by 69.5 °C when 24 500 J are applied. The specific heat of...
7. Calculation of the Amount of Energy Given Off in a Combustion Reaction Section PreLab Questions...
7. Calculation of the Amount of Energy Given Off in a Combustion Reaction Section PreLab Questions 1. Aluminum has a specific heat of 0.902 J/g x°C. How much heat is lost when a piece of aluminum with a mass of 23.984 g cools from a temperature of 415.0 °C to a temperature of 22.0°C? 2. The temperature of a sample of water increases by 69.5 °C when 24 500 J are applied. The specific heat of liquid water is 4.18...
How many calories are required to heat 25.0 g of platinum from 24.5 °C to 75°C...
How many calories are required to heat 25.0 g of platinum from 24.5 °C to 75°C (specific heat of platinum 0.139 J/gK)? Pay careful attention to units 20 cal 047 cal 42 cal 48 cal 80 cal
Find what heat in calories (cal) is required to increase the temperature of 52 g water...
Find what heat in calories (cal) is required to increase the temperature of 52 g water from 0°C to 50 °C The specific heat capacity of water is 1 cal/g. C Express your answer to two significant figures and include the appropriate units. Calculate the quantity of heat absorbed by 12 g of water that warms from 30°C to 82 °C. Express your answer to two significant figures and include the appropriate units.
12) If you added 4450 calories of heat to 197 g of aluminum at 25.0 degrees...
12) If you added 4450 calories of heat to 197 g of aluminum at 25.0 degrees C what would the resulting temperature be? The specific heat of aluminum is 0.220 cal/g °C
12. Practice problems with other materials: (Look up values for . Also consider ail digits heat...
12. Practice problems with other materials: (Look up values for . Also consider ail digits heat capacity or specific heat shown here to be significant.) a. How hot (what temperature?) would 15 g of aluminum at 20°c get if 90 cal of heat were added? b. How much heat would it take to heat 15 g of copper from 19°C to 31°C? c. What is the specific heat of a metal which requires 80 cal to change 50 g from...
1. The specific heat of aluminum is 0.215 cal/goc. A 1000 g block of aluminum is...
1. The specific heat of aluminum is 0.215 cal/goc. A 1000 g block of aluminum is heated to 600 oC and then allowed to cool. If the aluminum loses 5000. cal to the atmosphere in 30 seconds, what will be its temperature at the end of that period? 2. molar heat capacity of a substance was found to be 5.73 calmoloC, and the specific The heat capacity was found to be 0.0902 calg°C. What is the atomic weight of this...
9. 100-g aluminum calorimeter contains 250-g of water. The two substances are in thermal equilibrium at...
9. 100-g aluminum calorimeter contains 250-g of water. The two substances are in thermal equilibrium at 10° C. Two metallic blocks are placed in the water. One is a 50- piece of copper at 80° C. The other sample has a mass of 70-g and is originally at temperature of 100° C. The entire system stabilizes at a final temperature of 200 C. Determine the specific heat of the unknown second sample. (Assume the specific heat of aluminum, and copper...
Prob. 2: Cooling Curve Circle: Emathermier Exothermis?) Cale, the amount of heat this time in calories...
Prob. 2: Cooling Curve Circle: Emathermier Exothermis?) Cale, the amount of heat this time in calories (cal) - Ilse I cal 4184 for conversions) lost or removed From 1.75 mol water as steam at a convert it to solid ice chilled in a freezer to a temperature of 47.2°C Cumulative Heat Lost To do this, follow the above drawn curve to determine the amount of heat lost for each of the five steps of this process to convert superheated steam...
7. Calculation of the Amount of Energy Given Off in a Combustion Reaction Section PreLab Questions 1. Aluminum has a specific heat of 0.902 J/g x °C. How much heat is lost when a piece of aluminum with a mass of 23.984 g cools from a temperature of 415.0 °C to a temperature of 22.0 °C? = 8.50215 2. The temperature of a sample of water increases by 69.5 °C when 24 500 J are applied. The specific heat of...
7. Calculation of the Amount of Energy Given Off in a Combustion Reaction Section PreLab Questions 1. Aluminum has a specific heat of 0.902 J/g x°C. How much heat is lost when a piece of aluminum with a mass of 23.984 g cools from a temperature of 415.0 °C to a temperature of 22.0°C? 2. The temperature of a sample of water increases by 69.5 °C when 24 500 J are applied. The specific heat of liquid water is 4.18...
How many calories are required to heat 25.0 g of platinum from 24.5 °C to 75°C (specific heat of platinum 0.139 J/gK)? Pay careful attention to units 20 cal 047 cal 42 cal 48 cal 80 cal
Find what heat in calories (cal) is required to increase the temperature of 52 g water from 0°C to 50 °C The specific heat capacity of water is 1 cal/g. C Express your answer to two significant figures and include the appropriate units. Calculate the quantity of heat absorbed by 12 g of water that warms from 30°C to 82 °C. Express your answer to two significant figures and include the appropriate units.
12) If you added 4450 calories of heat to 197 g of aluminum at 25.0 degrees C what would the resulting temperature be? The specific heat of aluminum is 0.220 cal/g °C
12. Practice problems with other materials: (Look up values for . Also consider ail digits heat capacity or specific heat shown here to be significant.) a. How hot (what temperature?) would 15 g of aluminum at 20°c get if 90 cal of heat were added? b. How much heat would it take to heat 15 g of copper from 19°C to 31°C? c. What is the specific heat of a metal which requires 80 cal to change 50 g from...
1. The specific heat of aluminum is 0.215 cal/goc. A 1000 g block of aluminum is heated to 600 oC and then allowed to cool. If the aluminum loses 5000. cal to the atmosphere in 30 seconds, what will be its temperature at the end of that period? 2. molar heat capacity of a substance was found to be 5.73 calmoloC, and the specific The heat capacity was found to be 0.0902 calg°C. What is the atomic weight of this...
9. 100-g aluminum calorimeter contains 250-g of water. The two substances are in thermal equilibrium at 10° C. Two metallic blocks are placed in the water. One is a 50- piece of copper at 80° C. The other sample has a mass of 70-g and is originally at temperature of 100° C. The entire system stabilizes at a final temperature of 200 C. Determine the specific heat of the unknown second sample. (Assume the specific heat of aluminum, and copper...
Prob. 2: Cooling Curve Circle: Emathermier Exothermis?) Cale, the amount of heat this time in calories (cal) - Ilse I cal 4184 for conversions) lost or removed From 1.75 mol water as steam at a convert it to solid ice chilled in a freezer to a temperature of 47.2°C Cumulative Heat Lost To do this, follow the above drawn curve to determine the amount of heat lost for each of the five steps of this process to convert superheated steam...
Most questions answered within 3 hours.
-
What's the streaming business's problem on the
horizon?
asked 49 minutes ago -
I need help with writing the conclusion for this online lab
report
Abstract
By testing the...
asked 1 hour ago -
For the reaction 1N2+3H2-----> 2NH3, would the reaction rate
trend be: delta[NH3]/ delta t = -2...
asked 1 hour ago -
Within your current/past organization, identify a problem/issue
and format a design to address same. You may...
asked 1 hour ago -
A sock stuck to the side of a clothes-dryer barrel has a
centripetal acceleration of 24...
asked 2 hours ago -
A perfect gas undergoes an isentropic process such that its
volume doubles. If the ratio of...
asked 2 hours ago -
list the elements in groups 3A to 6A in the same order as in the
periodic...
asked 2 hours ago -
Estimating effect size. Peng and Chen (2014)
evaluated effect size estimates for various tests. In their...
asked 3 hours ago -
Write a script in MySQL that creates and calls a stored
procedure name test. This procedure...
asked 3 hours ago -
If we test the following: H0: μ = 17
vs. H1: μ ≠ 17 and the...
asked 3 hours ago -
in the past year TVG had revenues of 3 million, cost
of goods sold of $25...
asked 3 hours ago -
4) In a polypeptide, which bond cannot rotate because of its
partial double bond character?
The...
asked 3 hours ago