Chapter 10 review states of matter
Download
1 / 25

Chapter 10 - Review States of Matter - PowerPoint PPT Presentation


  • 256 Views
  • Updated On :

Chapter 10 - Review States 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?.

loader
I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.
capcha
Download Presentation

PowerPoint Slideshow about 'Chapter 10 - Review States of Matter' - aldis


An Image/Link below is provided (as is) to download presentation

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript
Chapter 10 review states of matter

Chapter 10 - ReviewStates of Matter

Milbank High School


Chapter 10 review
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 review1
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 review2
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 review3
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 review4
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 review5
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 review6
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 review7
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 review8
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 review9
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 review10
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 review thermochemistry heat and chemical change

Chemistry – Chapter 11 ReviewThermochemistry: Heat and Chemical Change

Milbank High School


Chapter 11 review
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 review1
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 review2
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 review3
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 review4
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 review5
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 review6
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 review7
Chapter 11 Review

  • What are valid units for specific heat capacity?

  • What does the symbol “H” stand for?


Chapter 11 review8
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 review9
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 review10
Chapter 11 Review

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


Chapter 11 review11
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?