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3. Calculate the heat absorbed by 25.0 g of water needed to raise its temperature from 20.0°C to 65.0'C. The specif...
3. Calculate the heat absorbed by 25.0 g of water needed to raise its temperature from...
3. Calculate the heat absorbed by 25.0 g of water needed to raise its temperature from 20.0°C to 65.0°C. The specific heat of water is 4.18 J/gºC. Show your work Final Answer 4. Aluminum metal has a specific heat of 0.901 J/g C. How much heat is transferred to a 6.75 g piece of aluminum initially at room temperature, 20.0°C, when it is placed into boiling water? The temperature of boiling water is 100°C. Show your work Final Answer 5....
please write clearly and use significant figures. thanks in advance 3. Calculate the heat absorbed by...
please write clearly and use significant figures. thanks in
advance
3. Calculate the heat absorbed by 25.0 g of water needed to raise its temperature from 20.0°C to 65.0°C. The specific heat of water is 4.18 J/gºC. Show your work Final Answer 4. Aluminum metal has a specific heat of 0.901 J/gºC. How much heat is transferred to a 6.75 g piece of aluminum initially at room temperature, 20.0°C, when it is placed into boiling water? The temperature of boiling...
Calculate the heat absorbed by 25.0 g of water needed to raise its temperature from 20.0...
Calculate the heat absorbed by 25.0 g of water needed to raise its temperature from 20.0 to 65.0 degrees C. The specific heat of water is 4.18 J/gC
Calculate the amount of heat that must be absorbed by 100.0 g of water at 20.0°C...
Calculate the amount of heat that must be absorbed by 100.0 g of water at 20.0°C to convert it to steam (water vapor) at 110.0°C. Given: Specific heats: (liq) = 4.18 J/g·°C (steam) = 1.84 J/g·°C DHvap = 40.7 kJ/mol
3) If 28.0 g of water at 26.4 °C gain 5,563 J of heat, what is...
3) If 28.0 g of water at 26.4 °C gain 5,563 J of heat, what is the final temperature of water? (Specific heat of water is 4.184 J/g.°C)) 4) If 46.2 g piece of aluminum is cooled from 84.5 °C to 29.5 °C, how much energy was lost by aluminum? (specific heat of aluminum is 0.901 J/(g.°C)) 5) If 78.6 g piece of iron is dropped into 100.0 g of water initially at 24.6 °C. The final temperature of both...
How much heat does 29.0 of water absorb, if its temperature increases from 20.0 C to...
How much heat does 29.0 of water absorb, if its temperature increases from 20.0 C to 46.0 C ? The specific heat capacity of water is 4.18 J/(g.C)
is dropped into an insulated container containing 300.0 g of water at 20.0 °C A 36.0...
is dropped into an insulated container containing 300.0 g of water at 20.0 °C A 36.0 g sample of iron, which has a specific heat capacity of 0.449 J-g C and a constant pressure of 1 atm. The initial temperature of the iron is 90.2 °C Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has the correct number of significant digits. ? X
I know the answers but I don't know how to solve the work. Please show the...
I know the answers but I don't know how to solve the work.
Please show the work
1.)
Answer: D
2.)
Answer: D
3.)
Answer: A
Aluminum has a specific heat of 0.902 J/g.°C. How many joules of heat are required to change the temperature of 8.50 grams of aluminum from 25.0°C to 93.4°C? a. 7.67 J b. 71.7 J c. 192J d. 524 J Water has a specific heat of 4.18 J/g. °C. If 35.0 g of water at...
1) An aluminum calorimeter of mass 58 g, has 155 g water, both at a temperature...
1) An aluminum calorimeter of
mass 58 g, has 155 g water, both at a temperature of 21°C. A 108-g
piece of metal originally kept in boiling water (T = 100°C) is
transferred to the calorimeter. The final equilibrium temperature
of the mixture is 26.6°C. Calculate the specific heat of the metal
(in J/kg). Specific Heats: Al = 900 J/kg, water =4186 J/g
2) How much heat, in kilo-joules, is required to convert 19 g of
ice at -13°C into...
Substance molar heat capacity (C.)/J•mol-1.°C-1 75.3 specific heat capacity (C.) /J•g-lo°C-1 0.384 H2O(1) Cu(s) C,H,OH(l) (ethanol)...
Substance molar heat capacity (C.)/J•mol-1.°C-1 75.3 specific heat capacity (C.) /J•g-lo°C-1 0.384 H2O(1) Cu(s) C,H,OH(l) (ethanol) Fe(s) 111.5 0.449 1. Fill in the empty entries in the table above. 2. If the same amount of energy is transferred to 1.0 g samples of each of the substances listed above, order them from largest AT to smallest AT. Explain. 3. Which is the consequence of copper's relatively low specific heat (0.385 J/(g°C)) compared to water (4.18 J/(g°C)) on the temperature change...
3. Calculate the heat absorbed by 25.0 g of water needed to raise its temperature from 20.0°C to 65.0°C. The specific heat of water is 4.18 J/gºC. Show your work Final Answer 4. Aluminum metal has a specific heat of 0.901 J/g C. How much heat is transferred to a 6.75 g piece of aluminum initially at room temperature, 20.0°C, when it is placed into boiling water? The temperature of boiling water is 100°C. Show your work Final Answer 5....
please write clearly and use significant figures. thanks in
advance
3. Calculate the heat absorbed by 25.0 g of water needed to raise its temperature from 20.0°C to 65.0°C. The specific heat of water is 4.18 J/gºC. Show your work Final Answer 4. Aluminum metal has a specific heat of 0.901 J/gºC. How much heat is transferred to a 6.75 g piece of aluminum initially at room temperature, 20.0°C, when it is placed into boiling water? The temperature of boiling...
3) If 28.0 g of water at 26.4 °C gain 5,563 J of heat, what is the final temperature of water? (Specific heat of water is 4.184 J/g.°C)) 4) If 46.2 g piece of aluminum is cooled from 84.5 °C to 29.5 °C, how much energy was lost by aluminum? (specific heat of aluminum is 0.901 J/(g.°C)) 5) If 78.6 g piece of iron is dropped into 100.0 g of water initially at 24.6 °C. The final temperature of both...
is dropped into an insulated container containing 300.0 g of water at 20.0 °C A 36.0 g sample of iron, which has a specific heat capacity of 0.449 J-g C and a constant pressure of 1 atm. The initial temperature of the iron is 90.2 °C Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has the correct number of significant digits. ? X
I know the answers but I don't know how to solve the work.
Please show the work
1.)
Answer: D
2.)
Answer: D
3.)
Answer: A
Aluminum has a specific heat of 0.902 J/g.°C. How many joules of heat are required to change the temperature of 8.50 grams of aluminum from 25.0°C to 93.4°C? a. 7.67 J b. 71.7 J c. 192J d. 524 J Water has a specific heat of 4.18 J/g. °C. If 35.0 g of water at...
1) An aluminum calorimeter of
mass 58 g, has 155 g water, both at a temperature of 21°C. A 108-g
piece of metal originally kept in boiling water (T = 100°C) is
transferred to the calorimeter. The final equilibrium temperature
of the mixture is 26.6°C. Calculate the specific heat of the metal
(in J/kg). Specific Heats: Al = 900 J/kg, water =4186 J/g
2) How much heat, in kilo-joules, is required to convert 19 g of
ice at -13°C into...
Substance molar heat capacity (C.)/J•mol-1.°C-1 75.3 specific heat capacity (C.) /J•g-lo°C-1 0.384 H2O(1) Cu(s) C,H,OH(l) (ethanol) Fe(s) 111.5 0.449 1. Fill in the empty entries in the table above. 2. If the same amount of energy is transferred to 1.0 g samples of each of the substances listed above, order them from largest AT to smallest AT. Explain. 3. Which is the consequence of copper's relatively low specific heat (0.385 J/(g°C)) compared to water (4.18 J/(g°C)) on the temperature change...
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