Adv Chem Unit 12 Review Days 1 and 2

The Law of Conservation of Energy states that

• energy is the capacity to do work.
• energy is neither created nor destroyed.
• heat flows from a warmer body to a cooler body.
• the total amount of energy in the universe is increasing.

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-4

When a hydrocarbon is burned in the presence of oxygen, the amount of energy in the universe

• increases.
• decreases.
• remains the same.
• cannot be determined without the specific heat of the hydrocarbon.

Tags

NGSS.HS-PS1-4

What energy transformation takes place when something burns?

• Chemical Potential → Thermal
  
• Kinetic → Chemical Potential
  
• Electromagnetic → 
  Chemical Potential
• Chemical Potential → Electrical

Tags

NGSS.HS-PS1-4

Consider the following specific heats:
Which substance, once warmed, would be more likely to maintain its heat and keep you warm through a long football game on a cold night?

• copper
• lead
• glass
• water

Tags

NGSS.HS-PS3-4

Calculate the amount of heat absorbed in kilojoules to raise the temperature of a 79.0 g sample of ethanol from 298.0°C to 385.0°C.  The specific heat capacity of ethanol is 2.42 J/g°C.

• 16,600 kJ
• 16.6 kJ
• -16,600 kJ
• -16.6 kJ

Tags

NGSS.HS-PS3-1

A 6.50g sample of copper metal at 25.0°C is heated by the addition of 84.0 J of energy. The final temperature of the copper is ________°C. The specific heat capacity of copper is 0.38J/g·°C.

• 29.9
• 9.0
• 59.0
• 34.0

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

It takes 11.2 kJ of energy to raise the temperature of 145 g of benzene from 23.0°C to 68.0°C. What is the specific heat of benzene?

• 1.14 J/(g × °C)
• 1.72 J/(g × °C)
• 3.48 J/(g × °C)
• 5.25 J/(g × °C)

Tags

NGSS.HS-PS3-1

A piece of metal of mass 16.0 g at 107.0°C is placed in a calorimeter containing 50.0 g of water at 21.0°C. The final temperature of the mixture is 23.3°C. What is the specific heat capacity of the metal? Assume that there is no energy lost to the surroundings.

• 0.36J/g°C
• 2.8J/g°C
• 0.18J/g°C
• 4.2J/g°C

Tags

NGSS.HS-PS3-4

A 25.0g piece of iron at 398K is placed in a styrofoam coffee cup containing 25.0 mL of water at 298 K.  Assuming that no heat is lost to the cup or the surroundings, what will the final temperature of the water be?  The specific heat capacity of iron = 0.449 J/g·K and water = 4.18 J/g·K.

• 348 K
• 308 K
• 287 K
• 325 K

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

100.g of copper metal at 100°C is placed in 100.g of water at 20°C. 
The specific heat of copper is 0.385J/g°C.
The specific heat of water is 4.18J/g°C.

• Heat is released by the copper metal.
  The final temperature of the system will be closer to the initial temperature of the water.
• Heat is released by the water.
  The final temperature of the system will be closer to the initial temperature of the water.
• Heat is released by the copper metal.
  The final temperature of the system will be closer to the initial temperature of the copper metal.
• Heat is released by the water.
  The final temperature of the system will be closer to the initial temperature of the copper metal.

Tags

NGSS.HS-PS3-4