Chapter 10 - ReviewStates of Matter

Milbank High School

Chapter 10 - Review

•What happens to the range of energies of the molecules in matter when the temperature is increased?

•What happens to the average kinetic energy of the particles in a sample of matter as the temperature is increased?

Chapter 10 - Review•Consider an iron ball and an

aluminum ball. If the two balls were at the same temperature, how would their average kinetic energies compare?

•Which temperature scale provides a direct measure of the average kinetic energy of a substance?

Chapter 10 - Review

•What instrument is normally used to measure atmospheric pressure?

•What is the SI unit of pressure?•How does the atmospheric

pressure at altitudes below sea level compare with atmospheric pressure at sea level?

Chapter 10 - Review•What volume does 3.00 moles

of gas particles occupy at STP?•What is the volume occupied

by 2.20 mol of hydrogen at STP•What is the number of moles of

gas in 20.0 L of oxygen at STP•What is the number of

molecules of nitrogen in 11.2 L at STP?

Chapter 10 - Review

•What is the volume occupied by 71.0 g of chlorine gas at STP?

•What is the number of grams of neon present in 78.4 L of neon at STP?

Chapter 10 - Review•What happens when a gas is

heated?•The average kinetic energy of

the particles of a substance is proportional to the ____ of the substance.

•The temperature at which the motion of particles theoretically ceases is ____

Chapter 10 - Review

•What is the pressure of one standard atmosphere?

•Standard conditions when working with gases are defined as ____.

•The pressure of a gas in a container is 152 mm Hg. This is equivalent to _____ atm.

Chapter 10 - Review

•Which states of matter can flow?

•Which would have the greatest kinetic energy: steam at 200 oC, or water at 373 K

•What happens to the evaporation rate of a liquid as the liquid is cooled?

Chapter 10 - Review

•If heat is added to a boiling liquid, what happens to the temperature of the liquid?

•What types of forces exist between particles of a liquid?

Chapter 10 - Review• The first particles to evaporate

from a liquid are ____.• Which of the following will

evaporate fastest: water at 20 oC, or water at 40 oC?

•The direct change of a substance from a solid to a gas is called ____.

Chapter 10 - Review

•What is the pressure when a liquid is boiling at it’s normal boiling point?

•When the vapor pressure of a liquid is equal to atmospheric pressure, the liquid ____.

•Water could be made to boil at 105 oC instead of 100 oC by ___.

Chemistry – Chapter 11 ReviewThermochemistry: Heat and

Chemical Change

Milbank High School

Chapter 11 Review

• How many joules are there in 148 calories? (1 cal = 4.18 J)

• What is the amount of heat (in calories) required to raise the temperature of 200 g of Aluminum by 10 oC? (specific heat of Al = 0.21 cal/g x oC)

Chapter 11 Review

• What is the specific heat of a substance if 1560 calories is required to raise the temperature of a 312 gram sample by 15 oC?

Chapter 11 Review

• How much heat does it take to warm 16 g of pure water from 90.0 oC to 100.0 oC? (specific heat of water = 4.18 J / g x oC)

Chapter 11 Review

• When 45 g of an alloy at 52 oC is dropped into 100.0 g of water at 25 oC, the final temperature is 37 oC. What is the specific heat of the alloy? (in calories/g x oC)

Chapter 11 Review

• A piece of metal is heated, and then submerged into cool water. What happens to the temperature of the metal, and the temperature of the water?

• How does a calorie compare to a joule?

Chapter 11 Review• Two objects are sitting next to

each other in direct sunlight. Object A gets hotter than object B. How does the specific heat of object A compare to object B?

Chapter 11 Review• Compared to 100 g of iron, a 10 g

sample of iron has _____ specific heat.

• A process that absorbs heat is called a(n) _____ process.

• If you were to touch the flask in which an endothermic reaction were occurring, how would it feel?

Chapter 11 Review

• What are valid units for specific heat capacity?

• What does the symbol “H” stand for?

Chapter 11 Review

• Calculate the energy required to produce 7.00 mol Cl2O7 based on the following given equation: 2Cl2(g) + 7O2(g) + 130 kcal 2 Cl2O7(g)

• If the heat involved in a chemical reaction has a negative sign, then heat is ____ the surroundings.

Chapter 11 Review

• What is the standard heat of reaction

(H) for this reaction:

C2H4(g) + H2(g) C2H6(g)

(Hof for C2H4(g) = +52.5 kj/mol; and

Hof for C2H6(g) = -84.7 kj/mol)

Chapter 11 Review

• The change in enthalpy is equal to _____. (give the formula)

Chapter 11 Review

• To determine the heat change for a reaction in an aqueous solution, _____.

• What is the amount of heat needed to melt one mole of a solid called?

• What is the heat of solution?