Question

Calculate the mass of a piece of copper that released 95.0 calories when cooled from 100.0...

Calculate the mass of a piece of copper that released 95.0 calories when cooled from 100.0 °C to 25.3 °C. The specific heat of copper is 0.0924 cal/(g°C).​ Remember significant.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A 40.0 g Ice Cube floats in 200.0 g of water in a 100.0 g copper...
A 40.0 g Ice Cube floats in 200.0 g of water in a 100.0 g copper cup! All are at a temperature of 0.000C. Then, a piece of lead at 98.00C is dropped into the cup, and the final equilibrium temperature is 12.00C. The specific heat of water and ice is 1.00 cal/g 0C, the specific heat of copper is 0.0924 cal/g 0C, the specific heat of lead is 0.0305 cal/g 0C, and the heat of fusion of ice is...
How much heat is released when 105 g of steam at 100.0°C is cooled to ice...
How much heat is released when 105 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol • °C), and the molar heat capacity of ice is 36.4 J/(mol • °C).
a/ Compute the quantity of heat released by 25.0 g of steam initially at 100.0 oC,...
a/ Compute the quantity of heat released by 25.0 g of steam initially at 100.0 oC, when it is cooled to 34.0°C and by 25.0 g of water initially at 100.0 oC, when it is cooled to 34.0°C. b/ You put your hand into this steam or this water (which is not recommended!), in which case your hand will be burnt more severely? Explain. The heat of vaporization of water is 2.256×106 J/kg and the specific heat of water is...
a/ Compute the quantity of heat released by 25.0 g of steam initially at 100.0 oC,...
a/ Compute the quantity of heat released by 25.0 g of steam initially at 100.0 oC, when it is cooled to 34.0°C and by 25.0 g of water initially at 100.0 oC, when it is cooled to 34.0°C. b/ You put your hand into this steam or this water (which is not recommended!), in which case your hand will be burnt more severely? Explain. The heat of fusion of water is 2.256×106 J/kg and the specific heat of water is...
A copper cylinder with a mass of 125 g and temperature of 345°C is cooled by...
A copper cylinder with a mass of 125 g and temperature of 345°C is cooled by dropping it into a glass beaker containing 565 g of water initially at 20.0°C. The mass of the beaker is 50.0 g and the specific heat of the glass is 840 J/kg∙K. What is the final equilibrium temperature of the system, assuming the cooling takes place very quickly, so that no energy is lost to the air? The specific heat of copper is 385...
If a piece of Cd with a mass = 37.6 g and initial temperature of 100.0...
If a piece of Cd with a mass = 37.6 g and initial temperature of 100.0 o C is dropped in 25.0 mL of water at 23 o C, what is the final temperature of the system? specific heat of Cd = 0.232 J/g o C; specific heat of water = 4.184 J/g o C.
One piece of copper metal at 105 degrees celcius has twice the mass of another copper...
One piece of copper metal at 105 degrees celcius has twice the mass of another copper piece at 45 degrees celcius. What is the final temp. if these two pieces are placed in a calorimeter? Specific heat of copper is 0.387 J/g K When 25.0mL of 0.500 M HCl is added to 25.0 mLof 0.500 M KOH in a coffee-cup calorimeter at 23.50 degrees celcius, the temp. rises to 30.17 degrees celcius. Calculate delta H of this reaction (assume density...
Please show all steps and reasoning to question. A piece of copper with heat capacity 50...
Please show all steps and reasoning to question. A piece of copper with heat capacity 50 cal/C° is removed from an oven at 95°C and placed into a container with a 40-g sample of water at 20°C. The two substances are allowed to come into thermal equilibrium. (Note: Ignore thermal interactions with the air and the container itself.) A. Consider the heat transfer needed to change the temperature of the water sample by 1C°. • How many calories are transferred?...
A 40 g block of ice is cooled to -78°C. and is then added to 610...
A 40 g block of ice is cooled to -78°C. and is then added to 610 g of water in an 80 g copper calorimeter at a temperature of 26°C. Determine the final temperature of the system consisting of the ice, water, and calorimeter. 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 = 2090 J/kg°C
A 40 g block of ice is cooled to -69°C. and is then added to 630...
A 40 g block of ice is cooled to -69°C. and is then added to 630 g of water in an 80 g copper calorimeter at a temperature of 27°C. Determine the final temperature of the system consisting of the ice, water, and calorimeter. 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 = 2090 J/kg°C.