A cube of ice is taken from the freezer at -9.5?Cand placed in a 95-g aluminum...

A cube of ice is taken from the freezer at -9.5?Cand placed in a 95-g aluminum calorimeter filled with 310g of water at room temperature of20.0 ?C. The final situation is observed to be all water at 15.0?C. The specific heat of ice is2100 J/kg?C?, the specific heat of aluminum is900 J/kg?C?, the specific heat of water is is4186 J/kg?C?, the heat of fusion of water is333 kJ/Kg. What was the mass of the ice cube?

Expert Solution

We have:

Specific heat of water = 4186 J/(kg.^oC)
Specific heat of ice = 2100 J/(kg.^oC)
Heat of fusion of ice = 3.33 x 10⁵ J/kg
Mass of water = 326 g = 0.326 kg

The temperature of the water decreased 5^o
For the water, Q = 0.326 * 4186 * 5 = 6823.18 joules

As the temperature of the water decreased 5^o, 6823.18 joules of heat energy was released.

For the ice to melt, the temperature of the ice must increase to 9.5 ^oC
Q = m * 2100 * 9.5 = m * 19950

During the melting, Q = m * 3.33 * 10⁵
Next, the temperature of the water increases from 0^o to 15^o
Q = m * 4186 * 15 = m * 62790

Total heat energy required by the ice cube = m * 19950 + m * 3.33 * 10⁵ + m * 62790

Total heat energy required by the ice cube = Total heat energy released by the water.

m * 19950 + m * 3.33 x 10⁵ + m * 62790 = 6823.18

Mass of ice cube = 6823.18 / (19950 + 3.33 x 10⁵ + 62790) =6823.18/415740
Mass of ice cube = 0.01641213258 kg = 16.41213258 grams.

genius_generous answered 4 months ago

An ice cube whose mass is 50 g is taken from a freezer at a temperature...

An ice cube whose mass is 50 g is taken from a freezer at a temperature of -10C and then dropped into a cup of water at 0C. If no heat is gained or lost from the outside, how much water will freeze onto the cup?

An ice cube with a mass of 0.0750kg is taken from a freezer, where the cube’s...

An ice cube with a mass of 0.0750kg is taken from a freezer, where the cube’s temperature was -10.0∞C, and dropped into a glass of water at 0.00∞C. a) If no heat is gained or lost from outside, how much water will freeze onto the cube? b) Is it possible to add so much ice to the glass that all the water freezes? Explain.

1. A 100 g ice cube at -10?C is placed in an aluminum cup whose initial...

1. A 100 g ice cube at -10?C is placed in an aluminum cup whose initial temperature is 70?C. The system comes to an equilibrium temperature of 20?C. What is the mass of the cup in kg. 2.Radiation from the head is a major source of heat loss from the human body. Model a head as a 20-cm-diameter, 20-cm-tall cylinder with a flat top.If the body's surface temperature is 36 ?C , what is the net rate of heat loss...

A 31 g ice cube at -15.0oC is placed in 139 g of water at 48.0oC....

A 31 g ice cube at -15.0oC is placed in 139 g of water at 48.0oC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is thermally insulated from the surroundings. Give your answer in oC with 3 significant figures. Specific heat of ice: 2.090 J/g K Specific heat of water: 4.186 J/g K Latent heat of fusion for water: 333...

A 26 g ice cube at -15.0oC is placed in 204 g of water at 48.0oC....

A 26 g ice cube at -15.0oC is placed in 204 g of water at 48.0oC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is thermally insulated from the surroundings. Give your answer in oC with 3 significant figures. Specific heat of ice: 2.090 J/g K Specific heat of water: 4.186 J/g K Latent heat of fusion for water: 333...

A 65 g ice cube at 0 °C is placed in an insulated box that contains...

A 65 g ice cube at 0 °C is placed in an insulated box that contains 8 g of steam at 200 °C. What is the equilibrium temperature reached by this closed system? Approximate the specific heat capacity of steam to be 1.5 J/g oC. All the other values can be found on the textbook. [Note: Assume that all of the steam condenses.]

A 50·g ice cube (at 0°C) is placed in an insulated cup with 250·g of water...

A 50·g ice cube (at 0°C) is placed in an insulated cup with 250·g of water which is at 46°C. The latent heat of fusion for ice is 80·cal/g and the specific heat of water is 1.0·cal/g/°C. (a) How much heat will the ice have to absorb from the water to completely melt (and turn into 0°C water)? ___ cal. (b) Find the temperature of the 250·g of water initially at 46°C after it loses the heat required to melt...

(a) You took two 50-g ice cubes from your −15 C kitchen freezer and placed them...

(a) You took two 50-g ice cubes from your −15 C kitchen freezer and placed them in 200 g of water in a thermally insulated container. If the water is initially at 25 C, what is the final temperature at thermal equilibrium? (b) What is the final temperature if only one ice cube is used? Hint: Watch out for the different possibilities!

a) A(n) 85-g ice cube at 0°C is placed in 920 g of water at 20°C....

a) A(n) 85-g ice cube at 0°C is placed in 920 g of water at 20°C. What is the final temperature of the mixture? b) A 103-g cube of ice at 0°C is dropped into 1.0 kg of water that was originally at 87°C. What is the final temperature of the water after the ice has melted? c) An aluminum cup contains 225 g of water and a 40-g copper stirrer, all at 27°C. A 432-g sample of silver at...

A 70.0 g ice cube at 0.0 degrees C is placed in a lake whose temperature...

A 70.0 g ice cube at 0.0 degrees C is placed in a lake whose temperature is 18.0 degrees C. Calculate the change in entropy (in joules/Kelvin) of the system as the ice cube comes to thermal equilibrium with the lake. (c for water = 4186 J/kg-K)

Question