You take a 15 gram cube of copper and heat it to 65 degrees Celsius. You...
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take a 15 gram cube of copper and heat it to 65 degrees Celsius.
You...
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...
an ice cube at 0.00 degrees celsius with a mass of 4.52 g is placed into...
an ice cube at 0.00 degrees celsius with a mass of 4.52 g is placed into 55g of water, initially at 23 degrees celsius. If no heat is lost to the surroundings, what is the final temperature of the entire water sample after all the ice is melted? (Specific heat of water is 4.184J/g*degrees celsius)
An 80g ice cube at 0 degrees Celsius is placed in 798g of water at 30...
An 80g ice cube at 0 degrees Celsius is placed in 798g of water at 30 degrees Celsius. What is the final temperature of the mixture? The latent heat of fusion for water is 3.33x10^5J/kg and the specific heat of water is 4186J/(kg x degrees Celsius).
if 300 g of a metal at 98 degrees Celsius is mixed into 500 g of...
if 300 g of a metal at 98 degrees Celsius is mixed into 500 g of water in a 200 g aluminum cup (cup and water both at 10 degrees celsius) and the final temperature of the mixture is 14.3 degrees celsius, what is the specific heat capacity of the metal? what is the metal?
A 25.00 gram sample of an unknown metal initially at 99.0 degrees Celsius is added to...
A 25.00 gram sample of an unknown metal initially at 99.0 degrees Celsius is added to 50.00 grams of water initially at 14.37 degrees Celsius. The final temperature of the metal and water is 20.15 degrees Celsius Calculate the specific heat of the metal (The specific heat of water is 4.184J'g'C). (HINTS Recall that the qof a system is equal to the of the surroundings So you can set up two equations here one for the loss of heat from...
A 25.00 gram sample of an unknown metal initially at 99.0 degrees Celsius is added to...
A 25.00 gram sample of an unknown metal initially at 99.0 degrees Celsius is added to 50.00 grams of water initially at 12.16 degrees Celsius. The final temperature of the metal and water is 20.15 degrees Celsius. Calculate the specific heat of the metal. (The specific heat of water is 4.184 J/g*C). (HINTS: Recall that the q of a system is equal to the -q of the surroundings. So you can set up two equations here: one for the loss...
1. An unknown sample is being evaluated in lab. What is the specific heat of the...
1. An unknown sample is being evaluated in lab. What is the specific heat of the compound if it requires 105.06 J to raise the temperature of 51.68 grams of the unknown from 15.25 °C to 22.9 °C. 2. A 25.00 gram sample of an unknown metal initially at 99.0 degrees Celsius is added to 50.00 grams of water initially at 5.94 degrees Celsius. The final temperature of the system is 20.15 degrees Celsius. Calculate the specific heat of the...
1. An unknown sample is being evaluated in lab. What is the specific heat of the...
1. An unknown sample is being evaluated in lab. What is the specific heat of the compound if it requires 105.06 J to raise the temperature of 51.68 grams of the unknown from 15.25 °C to 22.9 °C. 2. A 25.00 gram sample of an unknown metal initially at 99.0 degrees Celsius is added to 50.00 grams of water initially at 5.94 degrees Celsius. The final temperature of the system is 20.15 degrees Celsius. Calculate the specific heat of the...
A 200 g piece of ice at 0 degrees Celsius is place in 500 g of...
A 200 g piece of ice at 0 degrees Celsius is place in 500 g of water at 20 degrees Celsius. The system is in a container of negligible heat capacity and insulated from its surroundings. a) What is the final equilibrium temperature of the system? b) How much of the ice melts? The latent heat of fusion for water is (333.5 KI/kg). The specific heat of water is 4.18 KI/kg K Useful equations: Q = mlf and Q =...
Please answer in detail. Question 3: When you put heat into an object and the temperature...
Please answer in detail.
Question 3: When you put heat into an object and the temperature changes, what factors influence how much the temperature will change? Site experimental results that support what you say. Question 4: a) If you add 20 calories to 10 grams of water at 10 degrees Celsius, what will happen? b) If you add 20 calories to 1 gram of water at 10 degrees Celsius, what will happen? c) If you add 20 calories to 1...
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 25.00 gram sample of an unknown metal initially at 99.0 degrees Celsius is added to 50.00 grams of water initially at 14.37 degrees Celsius. The final temperature of the metal and water is 20.15 degrees Celsius Calculate the specific heat of the metal (The specific heat of water is 4.184J'g'C). (HINTS Recall that the qof a system is equal to the of the surroundings So you can set up two equations here one for the loss of heat from...
A 200 g piece of ice at 0 degrees Celsius is place in 500 g of water at 20 degrees Celsius. The system is in a container of negligible heat capacity and insulated from its surroundings. a) What is the final equilibrium temperature of the system? b) How much of the ice melts? The latent heat of fusion for water is (333.5 KI/kg). The specific heat of water is 4.18 KI/kg K Useful equations: Q = mlf and Q =...
Please answer in detail.
Question 3: When you put heat into an object and the temperature changes, what factors influence how much the temperature will change? Site experimental results that support what you say. Question 4: a) If you add 20 calories to 10 grams of water at 10 degrees Celsius, what will happen? b) If you add 20 calories to 1 gram of water at 10 degrees Celsius, what will happen? c) If you add 20 calories to 1...
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