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3. Calculate the heat absorbed by...
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....
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 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....
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
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...
Chapter 5: Thermodynamic 1) From the specific heat capacity (Cs), answer the following question: Aluminum (Cs...
Chapter 5: Thermodynamic 1) From the specific heat capacity (Cs), answer the following question: Aluminum (Cs = 0.901 J/(g.°C)) Iron (Cs 0.449 J/(g.°C) Water (Cs 4.184 J/(g.°C) Ethanol (Cs 2.43 J/(g.°C) (a) Order the materials based on the time required to heat them from the slowest to the fastest? (b) Which material will cool down the fastest? (c) Which material will take a lot of heat to change it temperature? 2) If the temperature of 35.6 g of ethanol increase...
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...
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...
SPECIFIC HEAT OF A METAL Specific heat is an intensive property, which is the amount of...
SPECIFIC HEAT OF A METAL Specific heat is an intensive property, which is the amount of heat required to raise the temperature of 1 gram substance by 1°C. Specific heat units areJ/g °C. Solve the following problems using your lecture notes: 1. When 8.50 g of metal, initially at 82 °C, is placed in 45 g water at 20°C, the final temperature of the metal and water is 22 °C. Calculate the specific heat of the metal in J/gºC. (specific...
1. Calculate the heat required to melt 5.4 g of naphthalene, C.H. AH, -18.8kJ /mol 2....
1. Calculate the heat required to melt 5.4 g of naphthalene, C.H. AH, -18.8kJ /mol 2. Ice at -10.0° C is combined with 50.0g of water at 75.0°C. Calculate the grams of ice present initially if the entire mixture comes to a final temperature of 25.0°C after the ice melts. Specific heat of water is 4.18 J/gºC, AH, = 334J/g Specific heat of water is 4.18 J/gºC, AH, = 3341/8 2. Consider the phase diagram of compound Z below: a....
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. 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....
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....
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...
Chapter 5: Thermodynamic 1) From the specific heat capacity (Cs), answer the following question: Aluminum (Cs = 0.901 J/(g.°C)) Iron (Cs 0.449 J/(g.°C) Water (Cs 4.184 J/(g.°C) Ethanol (Cs 2.43 J/(g.°C) (a) Order the materials based on the time required to heat them from the slowest to the fastest? (b) Which material will cool down the fastest? (c) Which material will take a lot of heat to change it temperature? 2) If the temperature of 35.6 g of ethanol increase...
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...
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...
SPECIFIC HEAT OF A METAL Specific heat is an intensive property, which is the amount of heat required to raise the temperature of 1 gram substance by 1°C. Specific heat units areJ/g °C. Solve the following problems using your lecture notes: 1. When 8.50 g of metal, initially at 82 °C, is placed in 45 g water at 20°C, the final temperature of the metal and water is 22 °C. Calculate the specific heat of the metal in J/gºC. (specific...
1. Calculate the heat required to melt 5.4 g of naphthalene, C.H. AH, -18.8kJ /mol 2. Ice at -10.0° C is combined with 50.0g of water at 75.0°C. Calculate the grams of ice present initially if the entire mixture comes to a final temperature of 25.0°C after the ice melts. Specific heat of water is 4.18 J/gºC, AH, = 334J/g Specific heat of water is 4.18 J/gºC, AH, = 3341/8 2. Consider the phase diagram of compound Z below: a....
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