Review for 3rd Quarter Benchmark

Solids, Liquids and Gases

  1. Which of the states of matter has the largest intermolecular forces?solids
  1. Which of the states of matter has the weakest intermolecular forces?gases
  1. What is the key characteristic that distinguishes a solid from a liquid?shape
  1. Which of the following states of matter has particles that can only vibrate in place?
  2. Solid
  3. Liquid
  4. Gas
  1. Which of the following states of matter has particles that are not bonded and can randomly move around to fill the volume of their container?
  2. Solid
  3. Liquid
  4. Gas
  1. Which of the following states of matter has particles that slide past one another in random patterns?
  2. Solid
  3. Liquid
  4. Gas
  1. What are the values for the temperature and pressure at STP?

Pressure=1atm or 760mmHg

Temperature=0oC or 273Kelvin

  1. What volume does one mole occupy at STP?22.4L
  1. What is absolute zero?-273oCand 0 K
  1. What happens at absolute zero?all motion stops
  1. Can you have a temperature below absolute zero?no
  1. Convert the following temperatures from Celsius to Kelvin.

a.225oC498 K

b.300oC573 K

c.-270oC3 K

  1. Convert the following temperatures from Kelvin to Celsius.

a.95 K-178oC

b.273 K0oC

c.1550 K1277oC

  1. If you open a sealed container of gas and the gas spreads out to fill the volume of the room, this process is called?
  2. Gas pressure
  3. Depression
  4. Diffusion
  5. Kinetic energy

True or false

  1. Diffusion is the going from level of high concentration to a level of lower concentration. true
  2. Gas pressure is determined when gas molecules collide with the walls of a container. true

Gas Laws

  1. Charles law says that V1/T1 = V2/T2 so what happens to the temperature if the volume increases? increase
  2. Charles law says that V1/T1 = V2/T2 so what happens to the temperature if the volume decreases? decrease
  3. Gay-Lussac’s law says that P1/T1 = P2/T2 so what happens to the temperature if the pressure increases? increase
  4. Gay-Lussac’s law says that P1/T1 = P2/T2 so what happens to the temperature if the pressure decreases? decrease
  5. Boyles’s law says that P1V1 = P2V2 so what happens to the volume if the pressure increases? decrease
  6. Boyles’s law says that P1V1 = P2V2 so what happens to the volume if the pressure decreases? increase
  1. A gas at 45K and a pressure of 0.333 atm is heated to 800K. Predict whether the pressure will increase or decrease? What will the new pressure be?

.333atm(800K) = 5.92

45K

  1. A container filled with 60L of gas at 2000K is cooled to 500K. Predict whether the volume will increase or decrease? What will the new volume be?

60L(500K) = 15L

2000K

  1. A gas at 250 L and a pressure of 6 atm is heated to 900 L. Predict whether the pressure will increase or decrease? What will the new pressure be?

250L(6atm) = 1.667atm

900L

Solutions

  1. What is a solute?Gets dissolved
  1. What is a solvent? Substance a solute is dissolved in
  1. What is a solution?the mixture
  1. If salt is dissolved in water, what is the solvent and what is the solute? Salt salute, water solvent

True or false

  1. When salt dissolves in water the salt crystal separates into ions.true
  1. Stirring increases the rate of dissolving?true

Solutions

  1. What is the molarity of a solution made with 30 g of NaOH dissolved in 2.5 L of water?

30g x 1mole = 0.75moles

40g

0.75moles = 0.3M

2.5L

  1. If you made 3 L of a 5 M solution of NaCl how much NaCl did you need to use?

3L x 5mole = 15moles

L

Thermochemistry

  1. What happens to the temperature in an endothermic reaction?

It gets colder

  1. What happens to the temperature in an exothermic reaction?

It heats up

  1. If a reaction gives off heat is it endothermic or exothermic?

exothermic

  1. If a reaction absorbs heat is it endothermic or exothermic?

endothermic

What do we call the following changes of state (melting, freezing…) and are they endothermic or exothermic.

Phase change Endo/Exothermic

  1. Converting from a solid to a liquid.Melting endothermic
  2. Converting from a liquid to a solid.Freezing exothermic
  3. Converting from a liquid to a gas.boiling endothermic
  4. Converting from a gas to a liquid.Condensationexothermic
  5. Converting from a solid to a gas.Sublimationendothermic
  6. Converting from a gas to a solid.depositionexothermic
  1. How much heat will be released when 4.72 g of carbon reacts with excess O2 according to the fallowing equation?

C + O2 CO2∆H°= -393.5 kJ/moles

4.72g x 1mole = 0.3933mole

12g

0.3933mole x -393.5kJ = -154.77kJ

mole

  1. How much heat will be absorbed when 38.2 g of bromine reacts with excess H2 according to the fallowing equation?

H2 + Br2 2HBr∆H°= -72.80 kJ/moles

38.2g x 1moleBr = 0.239 mole

159.8g

0.239mole x -72.80kJ = -17.4 kJ

mole

  1. For the following energy diagrams label products, reactants, the activation energy and if it is an exothermic or endothermic reaction.