If 320.18 g of Cu at 155.19 degrees C is added to 500 g of H2O...
If 320.18 g of Cu at 155.19 degrees C is added to 500 g of H2O at 25 oC, what is the final temperature of the copper and water? (Sp. H of Cu = 0.382 J/g oC)
Homework Answers
75 g of water is contained in a copper beaker of mass 102 g. The water and the Cu beaker are both at 25 oC. If 1.00 x 10...
75 g of water is contained in a copper beaker of mass 102 g. The water and the Cu beaker are both at 25 oC. If 1.00 x 103 J of thermal energy (heat) is added, what would be the final temperature?
015 10.0 points A 31 g block of ice is cooled to -80°C. It is added...
015 10.0 points A 31 g block of ice is cooled to -80°C. It is added to 547 g of water in an 98 g copper calorimeter at a temperature of 25°C Find the final temperature. The specific heat of copper is 387 J/kg °C and of ice is 2090 J/kg-oC. The latent heat of fusion of water is 3.33 × 105 J/kg and its specific heat is 4186 J/kg .°C. Answer in units of C
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...
If a 40 g block of copper metal at 100oC is added to 100 g of...
If a 40 g block of copper metal at 100oC is added to 100 g of water at 25oC, calculate the final temperature of the system. Cs water = 4.18 J/g oC. Cs copper= 0.385J/g oC.
A 25 g block of ice is cooled to −74 ◦C. It is added to 559...
A 25 g block of ice is cooled to −74 ◦C. It is added to 559 g of water in an 80 g copper calorimeter at a temperature of 21◦C. Find the final temperature. The specific heat of copper is 387 J/kg · ◦C and of ice is 2090 J/kg · ◦C . The latent heat of fusion of water is 3.33 × 105 J/kg and its specific heat is 4186 J/kg · ◦C . Answer in units of ◦C.
If a 40 g block of copper metal at 100oC is added to 100 g of water at 25oC, calculate the final ...
If a 40 g block of copper metal at 100oC is added to 100 g of water at 25oC, calculate the final temperature of the system. Cs water = 4.18 J/g oC. Cs copper= 0.385J/g oC.
A hot lump of 32.3g of Copper at an initial temperature of 96.5 degrees Celsius in...
A
hot lump of 32.3g of Copper at an initial temperature of 96.5
degrees Celsius in 50mL H2O initially at 25.0 degrees Celsius and
allowed to reach thermal equilibrium. What is the final temperature
of the copper and water, given that the specific hear is 0.385J/g°C
and the specific heat of water is 4.184J/g°C?
4. A hot lump of 41.3 g of copper at an initial temperature of 94.8 °C is placed in 50.0 mL H2O initially at 25.0 °C...
A 500-g water block of copper at a temperature of 70°C is dropped into 300 g...
A 500-g water block of copper at a temperature of 70°C is dropped into 300 g of water at 40°C. The is contained in a 100-g glass container. What is the final temperature of the mixture? oC
A 40-g block of ice is cooled to -71°C and is then added to 610 g...
A 40-g block of ice is cooled to -71°C and is then added to 610 g of water in an 80-g copper calorimeter at a temperature of 23°C. Determine the final temperature of the system consisting of the ice, water, and calorimeter. (If not all the ice melts, determine how much ice is left.) Remember that the ice must first warm to 0°C, melt, and then continue warming as water. (The specific heat of ice is 0.500 cal/g·°C = 2,090...
.5 M H2O4 17) A 100-gram sample of copper at 100.0°C is added to 50.0 grams...
.5 M H2O4 17) A 100-gram sample of copper at 100.0°C is added to 50.0 grams of water at 26.5°C in a thermally insulated container. What will be the final temperature of the Cu-H20 mixture if the specific heat of Cu-0.384 J/goC? (assume the specific heat of water is 4.184 J/g C and the density of water is 1.00 g/mL) (10 pts) your answer
015 10.0 points A 31 g block of ice is cooled to -80°C. It is added to 547 g of water in an 98 g copper calorimeter at a temperature of 25°C Find the final temperature. The specific heat of copper is 387 J/kg °C and of ice is 2090 J/kg-oC. The latent heat of fusion of water is 3.33 × 105 J/kg and its specific heat is 4186 J/kg .°C. Answer in units of C
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...
A
hot lump of 32.3g of Copper at an initial temperature of 96.5
degrees Celsius in 50mL H2O initially at 25.0 degrees Celsius and
allowed to reach thermal equilibrium. What is the final temperature
of the copper and water, given that the specific hear is 0.385J/g°C
and the specific heat of water is 4.184J/g°C?
4. A hot lump of 41.3 g of copper at an initial temperature of 94.8 °C is placed in 50.0 mL H2O initially at 25.0 °C...
A 500-g water block of copper at a temperature of 70°C is dropped into 300 g of water at 40°C. The is contained in a 100-g glass container. What is the final temperature of the mixture? oC
A 40-g block of ice is cooled to -71°C and is then added to 610 g of water in an 80-g copper calorimeter at a temperature of 23°C. Determine the final temperature of the system consisting of the ice, water, and calorimeter. (If not all the ice melts, determine how much ice is left.) Remember that the ice must first warm to 0°C, melt, and then continue warming as water. (The specific heat of ice is 0.500 cal/g·°C = 2,090...
.5 M H2O4 17) A 100-gram sample of copper at 100.0°C is added to 50.0 grams of water at 26.5°C in a thermally insulated container. What will be the final temperature of the Cu-H20 mixture if the specific heat of Cu-0.384 J/goC? (assume the specific heat of water is 4.184 J/g C and the density of water is 1.00 g/mL) (10 pts) your answer
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