Heating and Cooling Curve Calculations

Last updated about 2 months ago

9 questions

Instructions

Required

Heating and Cooling Curve Calculations

Last updated about 2 months ago

9 questions

Instructions

Energy constants (H2O)
334 J/g  Heat of fusion (melting or freezing) Hf
2260 J/g Heat of vaporization (evaporating or condensing) Hv
2.1 J/g˚C Heat capacity (c) of solid water
4.18 J/g˚C Heat capacity (c) of liquid water

For each of the problems sketch a warming or cooling curve to help you decide which equation(s) to use to solve the problem. Keep a reasonable number of sig figs in your answers.

How to put units in to get it right on formative.
Q= J
c= J/gC
m= g
T =C

Use and type C or J for the units for your answers :) 

Required

A cup of coffee (140 g) cools from 75˚C down to comfortable room temperature 20.˚C. How much energy does it release to the surroundings?

Use 0oC for the melting point.
Use 100oC for the boiling point

Required

Suppose during volleyball practice, you lost 909 g of water due to sweating. If all of this water evaporated, how much energy did the water absorb from your body? Express your answer in J.

Use 0oC for the melting point.
Use 100oC for the boiling point

Required

Suppose that during the Icy Hot lab that 65 kJ of energy were transferred to 450 g of water at 20˚C. What would have been the final temperature of the water? Use c= 4.18 J/gC

Round to the whole number.

Required

The heat capacity of solid iron is 0.447 J/g˚C. If the same quantity of energy as in #3 were transferred to a 450 g chunk of iron at 20.˚C, what would be the final temperature?

Round to the nearest tens place (add a 0 in the ones place). Include units.

Required

Suppose a bag full of ice (450 g) at 0.0 ˚C sits on the counter and begins to melt to liquid water. How much energy must be absorbed by the ice if 2/3 of it melted?

Use 0oC for the melting point.
Use 100oC for the boiling point

Required

A serving of Cheez-Its releases 130 kcal (1 kcal = 4.18 kJ) when digested by your body. If this same amount of energy were transferred to 2.5 kg of water at 27˚C, what would the final temperature be?

Required

How much energy must be absorbed by a 150 g sample of ice at 0.0 ˚C that melts and then warms to 25.0˚C?

Round to the hundreds place.

Required

A 12oz can of soft drink (assume m = 340 g) at 25˚C is placed in a freezer where the temperature is – 12 ˚C. How much energy must be removed from the soft drink for it to reach this temperature?

Round your number to the thousand place.

Required

65.0 kilojoules of energy are added to 150 g of ice at 0.0˚C. What is the final temperature of the water?

Round to the nearest TENTHS.
Hint: Do a heat of fusion calculation first. See what is the leftover energy is. Find the final temperature from the leftover energy using Q=mCΔT.

Heating and Cooling Curve Calculations

Heating and Cooling Curve Calculations

Energy constants (H2O)

A cup of coffee (140 g) cools from 75˚C down to comfortable room temperature 20.˚C. How much energy does it release to the surroundings?Use 0oC for the melting point. Use 100oC for the boiling point

Suppose during volleyball practice, you lost 909 g of water due to sweating. If all of this water evaporated, how much energy did the water absorb from your body? Express your answer in J. Use 0oC for the melting point.Use 100oC for the boiling point

Suppose that during the Icy Hot lab that 65 kJ of energy were transferred to 450 g of water at 20˚C. What would have been the final temperature of the water? Use c= 4.18 J/gC Round to the whole number.

The heat capacity of solid iron is 0.447 J/g˚C. If the same quantity of energy as in #3 were transferred to a 450 g chunk of iron at 20.˚C, what would be the final temperature?Round to the nearest tens place (add a 0 in the ones place). Include units.

Suppose a bag full of ice (450 g) at 0.0 ˚C sits on the counter and begins to melt to liquid water. How much energy must be absorbed by the ice if 2/3 of it melted?Use 0oC for the melting point.Use 100oC for the boiling point

A serving of Cheez-Its releases 130 kcal (1 kcal = 4.18 kJ) when digested by your body. If this same amount of energy were transferred to 2.5 kg of water at 27˚C, what would the final temperature be?

How much energy must be absorbed by a 150 g sample of ice at 0.0 ˚C that melts and then warms to 25.0˚C?Round to the hundreds place.

A 12oz can of soft drink (assume m = 340 g) at 25˚C is placed in a freezer where the temperature is – 12 ˚C. How much energy must be removed from the soft drink for it to reach this temperature?Round your number to the thousand place.

65.0 kilojoules of energy are added to 150 g of ice at 0.0˚C. What is the final temperature of the water?Round to the nearest TENTHS. Hint: Do a heat of fusion calculation first. See what is the leftover energy is. Find the final temperature from the leftover energy using Q=mCΔT.

Energy constants (H2O)

A cup of coffee (140 g) cools from 75˚C down to comfortable room temperature 20.˚C. How much energy does it release to the surroundings?Use 0oC for the melting point. Use 100oC for the boiling point

Suppose during volleyball practice, you lost 909 g of water due to sweating. If all of this water evaporated, how much energy did the water absorb from your body? Express your answer in J. Use 0oC for the melting point.Use 100oC for the boiling point

Suppose that during the Icy Hot lab that 65 kJ of energy were transferred to 450 g of water at 20˚C. What would have been the final temperature of the water? Use c= 4.18 J/gC Round to the whole number.

The heat capacity of solid iron is 0.447 J/g˚C. If the same quantity of energy as in #3 were transferred to a 450 g chunk of iron at 20.˚C, what would be the final temperature?Round to the nearest tens place (add a 0 in the ones place). Include units.

Suppose a bag full of ice (450 g) at 0.0 ˚C sits on the counter and begins to melt to liquid water. How much energy must be absorbed by the ice if 2/3 of it melted?Use 0oC for the melting point.Use 100oC for the boiling point

A serving of Cheez-Its releases 130 kcal (1 kcal = 4.18 kJ) when digested by your body. If this same amount of energy were transferred to 2.5 kg of water at 27˚C, what would the final temperature be?

How much energy must be absorbed by a 150 g sample of ice at 0.0 ˚C that melts and then warms to 25.0˚C?Round to the hundreds place.

A 12oz can of soft drink (assume m = 340 g) at 25˚C is placed in a freezer where the temperature is – 12 ˚C. How much energy must be removed from the soft drink for it to reach this temperature?Round your number to the thousand place.

65.0 kilojoules of energy are added to 150 g of ice at 0.0˚C. What is the final temperature of the water?Round to the nearest TENTHS. Hint: Do a heat of fusion calculation first. See what is the leftover energy is. Find the final temperature from the leftover energy using Q=mCΔT.

A cup of coffee (140 g) cools from 75˚C down to comfortable room temperature 20.˚C. How much energy does it release to the surroundings?

Use 0oC for the melting point.
Use 100oC for the boiling point

Suppose during volleyball practice, you lost 909 g of water due to sweating. If all of this water evaporated, how much energy did the water absorb from your body? Express your answer in J.

Use 0oC for the melting point.
Use 100oC for the boiling point

Suppose that during the Icy Hot lab that 65 kJ of energy were transferred to 450 g of water at 20˚C. What would have been the final temperature of the water? Use c= 4.18 J/gC

Round to the whole number.

The heat capacity of solid iron is 0.447 J/g˚C. If the same quantity of energy as in #3 were transferred to a 450 g chunk of iron at 20.˚C, what would be the final temperature?

Round to the nearest tens place (add a 0 in the ones place). Include units.

Suppose a bag full of ice (450 g) at 0.0 ˚C sits on the counter and begins to melt to liquid water. How much energy must be absorbed by the ice if 2/3 of it melted?

Use 0oC for the melting point.
Use 100oC for the boiling point

How much energy must be absorbed by a 150 g sample of ice at 0.0 ˚C that melts and then warms to 25.0˚C?

Round to the hundreds place.

A 12oz can of soft drink (assume m = 340 g) at 25˚C is placed in a freezer where the temperature is – 12 ˚C. How much energy must be removed from the soft drink for it to reach this temperature?

Round your number to the thousand place.

65.0 kilojoules of energy are added to 150 g of ice at 0.0˚C. What is the final temperature of the water?

Round to the nearest TENTHS.
Hint: Do a heat of fusion calculation first. See what is the leftover energy is. Find the final temperature from the leftover energy using Q=mCΔT.

A cup of coffee (140 g) cools from 75˚C down to comfortable room temperature 20.˚C. How much energy does it release to the surroundings?

Use 0oC for the melting point.
Use 100oC for the boiling point

Suppose during volleyball practice, you lost 909 g of water due to sweating. If all of this water evaporated, how much energy did the water absorb from your body? Express your answer in J.

Use 0oC for the melting point.
Use 100oC for the boiling point

Suppose that during the Icy Hot lab that 65 kJ of energy were transferred to 450 g of water at 20˚C. What would have been the final temperature of the water? Use c= 4.18 J/gC

Round to the whole number.

The heat capacity of solid iron is 0.447 J/g˚C. If the same quantity of energy as in #3 were transferred to a 450 g chunk of iron at 20.˚C, what would be the final temperature?

Round to the nearest tens place (add a 0 in the ones place). Include units.

Suppose a bag full of ice (450 g) at 0.0 ˚C sits on the counter and begins to melt to liquid water. How much energy must be absorbed by the ice if 2/3 of it melted?

Use 0oC for the melting point.
Use 100oC for the boiling point

How much energy must be absorbed by a 150 g sample of ice at 0.0 ˚C that melts and then warms to 25.0˚C?

Round to the hundreds place.

A 12oz can of soft drink (assume m = 340 g) at 25˚C is placed in a freezer where the temperature is – 12 ˚C. How much energy must be removed from the soft drink for it to reach this temperature?

Round your number to the thousand place.

65.0 kilojoules of energy are added to 150 g of ice at 0.0˚C. What is the final temperature of the water?

Round to the nearest TENTHS.
Hint: Do a heat of fusion calculation first. See what is the leftover energy is. Find the final temperature from the leftover energy using Q=mCΔT.