S2 Unit 11 Week 13 (Due 04-06-2025)

Two metals of equal mass but with differing specific heat capacities are subjected to the same amount of heat. Which metal will undergo the smallest change in temperature if neither metal changes phase?

• the metal with the higher heat capacity

• the metal with the lower heat capacity

• both metals will undergo the same temperature change

• you need to know the initial temperatures of both metals to answer this question

• you need to know the identities of the metals to answer this question

Tags

NGSS.HS-PS3-4

A piece of a newly synthesized material of mass 12.0 g at 88.0°C is placed in a calorimeter containing 100.0 g of water at 20.0°C. If the final temperature of the system is 24.0°C, what is the specific heat capacity of this material?

• 10.2 J · g⁻¹ · (°C)⁻¹

• 1.58 J · g⁻¹ · (°C)⁻¹

• 2.18 J · g⁻¹ · (°C)⁻¹

• 9.50 J · g⁻¹ · (°C)⁻¹

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

A coffee cup calorimeter contains 150g of water at 24.6°C. A 110g block of metal at 40.0°C is then placed in the calorimeter. The contents of the calorimeter come to 28.0°C as the metal releases 2125 J of energy into the water.

What is the heat capacity of the metal?

• 1.61 J/g°C

• 0.867 J/g°C

• 2130 J/g°C

• 0.248 J/g°C

Tags

NGSS.HS-PS3-4

NGSS.HS-PS3-1

The enthalpy of fusion of methanol (CH₃OH) is 3.16 kJ/mol. How much heat would be absorbed or released upon freezing 25.6 grams of methanol?

• 2.52 kJ absorbed

• 3.95 kJ absorbed

• 0.253 kJ released

• 2.52 kJ released

• 3.95 kJ released

Tags

NGSS.HS-PS3-1

Calculate the enthalpy change that occurs when 1.00 kg of acetone condenses at its boiling point (329.4 K). The standard enthalpy of vaporization of acetone is 29.1 kJ · mol⁻¹.

• -501 kJ

• -29.1 kJ

• -2.91 x 10⁴ kJ

• +501 kJ

• +29.1 kJ

Tags

NGSS.HS-PS3-4

Calculate the enthalpy change that occurs when 1 lb (454 g) of mercury freezes at its freezing point (234.3 K). The standard enthalpy of fusion of mercury is 2.29 kJ · mol⁻¹.

• -2.29 kJ

• -1.04 x 10³ kJ

• +5.18 kJ

• +2.29 kJ

• -5.18 kJ

Tags

NGSS.HS-PS3-1

Juan freezes a bottle of water to ice (500 mL) in preparation for a road trip. How much heat can be absorbed by that ice before it is fully melted? The heat of fusion of water is 334 J/g.

• 1130 kJ

• 167 kJ

• 2090 kJ

• 6.02 kJ

• 0 kJ

Tags

NGSS.HS-PS3-4

How much heat is required to change the temperature of two cups of water (500 mL) from room temperature (25°C) to boiling? (Remember, the density of water is 1.00 g/mL)

• 78.5 kJ

• 157 kJ

• 1.57 kJ

• 15.7 kJ

• 0.785 kJ

Tags

NGSS.HS-PS3-4

What is the best definition of specific heat?

• the quantity of heat energy that must be absorbed to make one gram of a substance boil

• the quantity of heat energy that must be absorbed to increase the temperature of one gram of a substance by one degree Celsius

• the boiling point of a substance

• the difference between the freezing point and the boiling point of a substance

• 6.7 × 10⁵ J

• 1.7 × 10⁵ J

• 3.8 × 10⁴ J

• 6.7 × 10² J

• 3.8 × 10⁵ J

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4