A hot iron bar is lowered into a 500 g sample of water which is at...
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hot iron bar is lowered into a 500 g sample of water which is at...
A hot gold bar that is 45kg is lowered into a 20kg ice bath that is...
A hot gold bar that is 45kg is lowered into a 20kg ice bath that is 30 percentage ice and the rest water that is in an iron container that has a mass of 2kg. Assume the ice bath and iron container is at thermal equilibrium to start. The final equilibrium temperature is 37 degree C. How much energy input is needed to convert the ice to water? Assuming no energy is lost to the environment and the system is...
A hot lump of 42.5 g of iron at an initial temperature of 98.4 °C is...
A hot lump of 42.5 g of iron at an initial temperature of 98.4 °C is placed in 50.0 mL of H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the iron and water given that the specific heat of iron is 0.449 J/(g·°C)? Assume no heat is lost to surroundings.
A hot lump of 30.9 g of iron at an initial temperature of 86.4 °C is...
A hot lump of 30.9 g of iron at an initial temperature of 86.4 °C is placed in 50.0 mL H, initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the iron and water, given that the specific heat of iron is 0.449 J/(g.°C)? Assume no heat is lost to surroundings.
2. A construction worker drops a hot 100-g iron rivet at 500 °C into a bucket...
2. A construction worker drops a hot 100-g iron rivet at 500 °C into a bucket containing 500 g of mercury at 20°C. Assuming that no heat is lost to the surroundings or the bucket, what is the final temperature of the rivet and mercury? 3. An unknown liquid of mass 400 g at a temperature of 80°C is poured into 400 g of water at 40°C. The final equilibrium temperature of the mixture is 49°C. What is the specific...
A 50.0 g piece of hot iron is placed in 165 g of water with an...
A 50.0 g piece of hot iron is placed in 165 g of water with an initial temperature of 22.8°C. The temperature of the combination rises to 25.7°C. What was the initial temperature of the iron? The specific heat of iron is 0.449 J/gK and the specific heat of water is 4.18 J/gK.
A large bucket contains 3000 g of 20 °C water. A 500 g cube of iron...
A large bucket contains 3000 g of 20 °C water. A 500 g cube of iron (c = 0.450 J/g•°C) is at 100 °C before it is placed in the water. What is the final temperature of the iron and water?
if a 100 kg sample of aluminum at 25.0 °C is heated with 500 kJ of...
if a 100 kg sample of aluminum at 25.0 °C is heated with 500 kJ of heat energy, what will be the final temperature of the metal sample? The specific heat of aluminum is 0.897 J/ g• °C
You cool a 120.0 g slug of red-hot iron (temperature 745 ∘C) by dropping it into...
You cool a 120.0 g slug of red-hot iron (temperature 745 ∘C) by dropping it into an insulated cup of negligible mass containing 75.0 g of water at 20.0 ∘C. Assume no heat exchange with the surroundings. a) What is the final temperature of the water? T final = ? degrees C b) What is the final mass of the iron and the remaining water? m final = ? g
A 52.9 g sample of iron is put into a calorimeter (see sketch at right) that contains 200.0 g of water. The iron sample...
A 52.9 g sample of iron is put into a calorimeter (see sketch at right) that contains 200.0 g of water. The iron sample starts off at 98.3 °C and the temperature of the water starts off at 24.0 °C. When the temperature of the water stops changing it's 26.5 °C. The pressure remains constant at 1 atm. insulated container water Calculate the specific heat capacity of iron according to this experiment. Be sure your answer is rounded to 2...
If a 125 g sample of iron is heated to 250.0 oC and then placed in...
If a 125 g sample of iron is heated to 250.0 oC and then placed in 500.0 g of water at 25.0 oC in an insulated container, what will the final temperature of the water and iron be? Assume that all of the heat transfers from the iron to the water without loss to the surroundings. ( qH2O = -q Fe ) cs (Fe) = 0.450 J/g oC cp (H2O) = 4.18 J/g oC
A hot gold bar that is 45kg is lowered into a 20kg ice bath that is 30 percentage ice and the rest water that is in an iron container that has a mass of 2kg. Assume the ice bath and iron container is at thermal equilibrium to start. The final equilibrium temperature is 37 degree C. How much energy input is needed to convert the ice to water? Assuming no energy is lost to the environment and the system is...
A hot lump of 30.9 g of iron at an initial temperature of 86.4 °C is placed in 50.0 mL H, initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the iron and water, given that the specific heat of iron is 0.449 J/(g.°C)? Assume no heat is lost to surroundings.
2. A construction worker drops a hot 100-g iron rivet at 500 °C into a bucket containing 500 g of mercury at 20°C. Assuming that no heat is lost to the surroundings or the bucket, what is the final temperature of the rivet and mercury? 3. An unknown liquid of mass 400 g at a temperature of 80°C is poured into 400 g of water at 40°C. The final equilibrium temperature of the mixture is 49°C. What is the specific...
A 52.9 g sample of iron is put into a calorimeter (see sketch at right) that contains 200.0 g of water. The iron sample starts off at 98.3 °C and the temperature of the water starts off at 24.0 °C. When the temperature of the water stops changing it's 26.5 °C. The pressure remains constant at 1 atm. insulated container water Calculate the specific heat capacity of iron according to this experiment. Be sure your answer is rounded to 2...
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