A rod made of cobalt with a mass of 0.80 kg is heated to 850°C, then...
A rod made of cobalt with a mass of 0.80 kg is heated to 850°C, then dropped into 7.00 kg of water at 10°C. What is the total change in entropy (in J/K) of the rod-water system, assuming no energy is lost by heat from this system to the surroundings? The specific heat of cobalt is 420 J/(kg · K), and the specific heat of water is 4,186 J/(kg · K). (Hint: note that
dQ = mcdT.)
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A rod made of cobalt with a mass of 0.80 kg is heated to 850°C,
then...
A cylinder made of brass with a mass of 0.80 kg is heated to 850°C, then...
A cylinder made of brass with a mass of 0.80 kg is heated to 850°C, then dropped into 5.00 kg of water at 11°C. What is the total change in entropy (in J/K) of the cylinder-water system, assuming no energy is lost by heat from this system to the surroundings? The specific heat of brass is 380 J/(kg · K), and the specific heat of water is 4,186 J/(kg · K). (Hint: note that dQ = mcdT.)
at 860°C and dropped into 5.00 kg of Assuming entropy change of the horseshoe-plus-water system. is...
at 860°C and dropped into 5.00 kg of Assuming entropy change of the horseshoe-plus-water system. is take n from a forge water at 11.0°c A 0.80-kg iro de mcdT.) n horseshoe ssuming that no energy is lost by heat to the surroundings, determine the total hoe- plus-water system. (Suggestion: Note that J/K
A 1.00-kg iron horseshoe is taken from a forge at 900°C and dropped into 4.00 kg...
A 1.00-kg iron horseshoe is taken from a forge at 900°C and dropped into 4.00 kg of water at 10.0°C. Assuming that no energy is lost by heat to the surroundings, determine the total entropy change of the horseshoe-pluswater system.
A 125 g sample of an unknown substance is heated to 93.6 °C and then dropped...
A 125 g sample of an unknown substance is heated to 93.6 °C and then dropped into 100.0 g of water at 19.0°C in a calorimeter. The temperature of the water rises to 31.0°C. What is the specific heat of the substance? Assume no heat lost to the surroundings. The specific heat of water is 4.184 J/ (g•°C).
Determination of Specific Heat of Metals: (8 points) Ametal rod with a mass of 50.0 g was heated to 100°C in boilin...
Determination of Specific Heat of Metals: (8 points) Ametal rod with a mass of 50.0 g was heated to 100°C in boiling water for 10 minutes and then placed into a cup of water containing 40 mL of water at 22.5 C. The temperature increased to a maximum of 34.4'C. The specific heat of water (Cp) is 4.184 J/g K and q = mx CP X AT a). How much heat (in Joules) was gained by the water? b). How...
008 10.0 points A 0.0497 kg ingot of metal is heated to 197°C and then is...
008 10.0 points A 0.0497 kg ingot of metal is heated to 197°C and then is dropped into a bea 0.392 kg of water initially at 21°C ker containing If the final equilibrium state of the mixed system is 23.4°C, find the specific heat of the metal. The specific heat of water is 4186 J/kg.° C Answer in units of J/kg.° C
A blork of metal of mass .20 kg is heated to 142.11 and dropped in a...
A blork of metal of mass .20 kg is heated to 142.11 and dropped in a copper calorimeter of mass .250 kg that contains .2 kg of water at 30 he calorimeter and its contents are insulated from the environment and have a final temperature of 44.0°C upon reaching thermal equilibrium. Find the specific heat of the metal. Assume the specific heat of water is 4.190 x 10 J/(kg K) and the specific heat of copper is 386 J/(kg K)....
need help solving pls Problem 17.62 c) 11 of 19 An 850-g iron block is heated...
need help solving pls
Problem 17.62 c) 11 of 19 An 850-g iron block is heated to 360 C and placed in an insulated Part A (of negligible heat capacity) containing 35.0 g of water at 25.0 C What is the equilibrium temperature of this system? The average specific heat of iron over this temperature range is 560 J/(kg K). Provide Feedback Next > S3
Practice With Calorimetry And Heat 1. 75.0 g of cast iron was heated to 100°C and...
Practice With Calorimetry And Heat 1. 75.0 g of cast iron was heated to 100°C and then plunged into 100 g of water at 23.0°C. Calculate the final temperature. Cast iron has specific heat of 0.46 J/gºc 2. A 25.0 g sample of an unknown metal at 99.5°C is placed into a calorimeter holding 50.0 g of water at 22.3°C. The final temperature was 26.2°C; what was the specific heat of the metal? 3. 30.0 g of water at 7.00°C...
An insulated beaker with negligible mass contains liquid water with a mass of 0.350 kg and...
An insulated beaker with negligible mass contains liquid water with a mass of 0.350 kg and a temperature of 60.8 C How much ice at a temperature of -12.1 C must be dropped into the water so that the final temperature of the 29.0 C ? system will be 00 J/kg K, and the heat of Take the specific heat of liquid water to be 4190J/kg. K, the specific heat of ice to be 2 fusion for water to be...
at 860°C and dropped into 5.00 kg of Assuming entropy change of the horseshoe-plus-water system. is take n from a forge water at 11.0°c A 0.80-kg iro de mcdT.) n horseshoe ssuming that no energy is lost by heat to the surroundings, determine the total hoe- plus-water system. (Suggestion: Note that J/K
Determination of Specific Heat of Metals: (8 points) Ametal rod with a mass of 50.0 g was heated to 100°C in boiling water for 10 minutes and then placed into a cup of water containing 40 mL of water at 22.5 C. The temperature increased to a maximum of 34.4'C. The specific heat of water (Cp) is 4.184 J/g K and q = mx CP X AT a). How much heat (in Joules) was gained by the water? b). How...
008 10.0 points A 0.0497 kg ingot of metal is heated to 197°C and then is dropped into a bea 0.392 kg of water initially at 21°C ker containing If the final equilibrium state of the mixed system is 23.4°C, find the specific heat of the metal. The specific heat of water is 4186 J/kg.° C Answer in units of J/kg.° C
A blork of metal of mass .20 kg is heated to 142.11 and dropped in a copper calorimeter of mass .250 kg that contains .2 kg of water at 30 he calorimeter and its contents are insulated from the environment and have a final temperature of 44.0°C upon reaching thermal equilibrium. Find the specific heat of the metal. Assume the specific heat of water is 4.190 x 10 J/(kg K) and the specific heat of copper is 386 J/(kg K)....
need help solving pls
Problem 17.62 c) 11 of 19 An 850-g iron block is heated to 360 C and placed in an insulated Part A (of negligible heat capacity) containing 35.0 g of water at 25.0 C What is the equilibrium temperature of this system? The average specific heat of iron over this temperature range is 560 J/(kg K). Provide Feedback Next > S3
Practice With Calorimetry And Heat 1. 75.0 g of cast iron was heated to 100°C and then plunged into 100 g of water at 23.0°C. Calculate the final temperature. Cast iron has specific heat of 0.46 J/gºc 2. A 25.0 g sample of an unknown metal at 99.5°C is placed into a calorimeter holding 50.0 g of water at 22.3°C. The final temperature was 26.2°C; what was the specific heat of the metal? 3. 30.0 g of water at 7.00°C...
An insulated beaker with negligible mass contains liquid water with a mass of 0.350 kg and a temperature of 60.8 C How much ice at a temperature of -12.1 C must be dropped into the water so that the final temperature of the 29.0 C ? system will be 00 J/kg K, and the heat of Take the specific heat of liquid water to be 4190J/kg. K, the specific heat of ice to be 2 fusion for water to be...
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