Initially, 48.0 g of ice at 0 °?? is in an aluminum calorimeter can of mass...
Initially, 48.0 g of ice at 0 °?? is in an aluminum calorimeter can of mass 2.0 g, also at 0 °??. Then 75.0 g of water at 80 °?? is poured into the can. What is the final temperature?
Homework Answers
When you solve ice water
problem then you have to aware about melting (change of state) the
ice then you can go to check the heat flow in change in temp.
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Initially, 48.0 g of ice at 0 °?? is in an aluminum calorimeter
can of mass...
A 95-g aluminum calorimeter is filled with ice taken from the freezer at -8.50C. The calorimeter...
A 95-g aluminum calorimeter is filled with ice taken from the freezer at -8.50C. The calorimeter is then filled with 100 g of steam at a temperature of 1030C. Assume the aluminum calorimeter has the same initial temperature as the ice. The final situation is observed to be all water at 90.00C. What was the mass of the ice?
An aluminum calorimeter with a mass of 100 g contains 250 g of water. The calorimeter...
An aluminum calorimeter with a mass of 100 g contains 250 g of water. The calorimeter and water are in thermal equilibrium at 10°C. Two metallic blocks are placed into the water. One is a 51.0-g piece of copper at 80°C. The other has a mass of 544 g and is originally at a temperature of 100°C. The entire system stabilizes at a final temperature of 20°C. (a) Determine the specific heat of the unknown sample. (J/Kg*C) (b) Using the...
A 200 g aluminum calorimeter can contain 500 g of water at 20 C. A 100...
A 200 g aluminum calorimeter can contain 500 g of water at 20 C. A 100 g piece of ice cooled to -20 C is placed in the calorimeter. Find the final temperature of the system, assuming no heat losses. (Assume that the specific heat of ice is 2.0 kJ/kg K) A second 200 g piece of ice at -20 C is added. How much ice remains in the system after it reaches equilibrium? Would your answer to part b...
An aluminum calorimeter with a mass of 425.00 g contains 1062.50 g of water. The calorimeter...
An aluminum calorimeter with a mass of 425.00 g contains 1062.50 g of water. The calorimeter and water are in thermal equilibrium at 12.50 ° C. Two metal blocks are placed in the water. One is a piece of copper from 212.50 g to 85.00 ° C. The other has a mass of 202.50 g and is originally at a temperature of 105.00 ° C. The entire system is stabilized at a final temperature of 22.50 ° C. (a) Determine...
237 g of water at 98 °C is poured into a 146 -g insulated aluminum calorimeter...
237 g of water at 98 °C is poured into a 146 -g insulated aluminum calorimeter cup at an initial temperature 20 °C. The final temperature of this system is 88.8773°C. What is the change in entropy in this process?
0. Consider a 600 g metallic cylinder initially at 90 °C is added to a calorimeter....
0. Consider a 600 g metallic cylinder initially at 90 °C is added to a calorimeter. The mass of the inner aluminum cup is 65 g and the mass of water is 180 g. The initial temperature of the water and cup) is 20 °C. After the hot cylinder is added to the calorimeter, the equilibrium temperature is 48 °C. Calculate the specific heat of the cylinder and identify the metal.
What is the mass of ice (in g) at 0 °C that can be completely melted...
What is the mass of ice (in g) at 0 °C that can be completely melted into liquid water at 0°C by a 119 g aluminum block at temperature 112 °C? Assume the aluminum block can melt the ice until its temperature drops to 0 °C. The heat capacity of aluminum is 0.903 J g-1 °C-1 and the heat of fusion of water is 6.02 kJ mol-1. Express your answer to 3 significant figures.
1) An aluminum calorimeter of mass 58 g, has 155 g water, both at a temperature...
1) An aluminum calorimeter of
mass 58 g, has 155 g water, both at a temperature of 21°C. A 108-g
piece of metal originally kept in boiling water (T = 100°C) is
transferred to the calorimeter. The final equilibrium temperature
of the mixture is 26.6°C. Calculate the specific heat of the metal
(in J/kg). Specific Heats: Al = 900 J/kg, water =4186 J/g
2) How much heat, in kilo-joules, is required to convert 19 g of
ice at -13°C into...
255 g of water initially at 27 oC is poured onto the ice at 0 oC...
255 g of water initially at 27 oC is poured onto the ice at 0 oC and the ice-water system is then isolated. After a while the equilibrium at 0 oC is established. If the latent heat of fusion of water is 80 cal/g the amount of ice that has melted is
A copper calorimeter can with mass 0.100kg contains 0.160kg of water and 0.018kg of ice in...
A copper calorimeter can with mass 0.100kg contains 0.160kg of water and 0.018kg of ice in thermal equilibrium at atmospheric pressure. Part A If 0.750kg of lead at a temperature of 255 c is dropped into the calorimeter can, what is the final temperature? Assume that no heat is lost to the surroundings
0. Consider a 600 g metallic cylinder initially at 90 °C is added to a calorimeter. The mass of the inner aluminum cup is 65 g and the mass of water is 180 g. The initial temperature of the water and cup) is 20 °C. After the hot cylinder is added to the calorimeter, the equilibrium temperature is 48 °C. Calculate the specific heat of the cylinder and identify the metal.
1) An aluminum calorimeter of
mass 58 g, has 155 g water, both at a temperature of 21°C. A 108-g
piece of metal originally kept in boiling water (T = 100°C) is
transferred to the calorimeter. The final equilibrium temperature
of the mixture is 26.6°C. Calculate the specific heat of the metal
(in J/kg). Specific Heats: Al = 900 J/kg, water =4186 J/g
2) How much heat, in kilo-joules, is required to convert 19 g of
ice at -13°C into...
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