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130 Cards in this Set
- Front
- Back
correct value for Avogadro's number
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6.022 x 10(exponent23)
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A ____________ formula tells what elements are present and gives the simplest whole-number ration of atoms in the compound.
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empirical
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How many atoms are in 2.00kg of copper?
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2.84 x 10(exponent 24) atoms Cu
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What is the molar mass of NaCl
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58.44 g
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Which of the following is not a property of gas?
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malleability
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the coefficients of a balanced equation give molar ratios rather than mass ratios
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true
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Balanced equations are required in order to perform stoichiometric calculations correctly.
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true
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The mass of a known substance may be converted to moles using the gram-molecular mass of that substance.
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true
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The number of helium atoms in a mole of helium is equal to the number of lead atoms in a mole of lead.
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false
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Which of the following is not an assumption of the kinetic theory?
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Gas molecule lose energy when they collide with one another.
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Which property of gases best explains the fact than an ordor produced in one part of a room can soon be detected throughout the room?
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permeability
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Which of the following pairs is related by an inverse relationship?
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pressure and temperature
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Which gas law focuses on the relationship between pressure and volume?
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Boyle's law
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Which gas law is represented by the equation PV=nRT?
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ideal gas law
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The gas law that focuses on the relationship between volume and temperature is ___________________.
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Charles's law
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The volume occupied by Avogadro's number of molecules of gas at STP is known as the _____________.
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molar volume
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The gas law that focuses on the relationship between pressure and temperature is
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Gay-Lussac's law
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The volumes of reacting gases and their gaseous products are expressed in small whole numbers.
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the law of combining volumes
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What law states that the total pressure of a mixture of gases equals the sum of the partial pressures?
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Dalton's law of partial pressures
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All gas molecules of the same the have the same speed at the same temperature.
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False
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Diffusion could not occur if molecules were not in constant motion.
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True
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The abbreviation STP represents the standard conditions of 760 atm and 273K.
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false
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if the temperature of a quantity of gas changes from 100 Celsius to 200 Celsius, the volume of the gas will double if the pressure remains constant.
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false
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Charles's law is an example of a direct relationship.
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True
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The gas laws cannot be violated.
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? (it's on test 10 question 17)
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Only ideal gases actually behave according to the kinetic theory.
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true
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Gay-Lussac's law describes the observation that the pressure in hot tires is greater than it is in the same tires when they are cold.
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true
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According to the kinetic theory, gravitational, electrical, and chemical forces between molecules must be considered in addition to collisions.
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true
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Collisions constantly change the speed and direction of gas molecules.
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true
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When solving gas law equations you can use either the Celsius or Kelvin temperature scale.
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Test chapter 10 question 22 ???
answer??? |
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A mole of any gas will always occupy 22.4 L at STP.
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true
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A gas quickly expands to fill a low pressure region.
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expansibility
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A gas easily mingles with another porous substance.
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? Chapter 10 #24
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A gas easily mingles with another porous substance.
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? Chapter 10 #25
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Collisions of gas molecules conserve energy
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elasticity
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High pressure can squeeze gases into smaller volumes.
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compressibility
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Gas molecules move constantly to uniformly fill their containers.
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? Chapter 10 # 28
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has lower values for gases than for solids and liquids
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density
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determined by the average kinetic energy of molecules
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temperature
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depends on the force and numbers of collisions per second
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pressure
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has the same value for 1 mole of any ideal gas at STP
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volume
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For a constant quantity of gas at a constant pressure, if you decrease the temperature the volume must _____________.
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decrease
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For a constant quantity of gas at constant temperature, if you decrease the volume, the pressure will __________.
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decrease (? you might want to check to be sure test 10 question 34)
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For a given quantity of gas in a container with a fixed volume, if you increase the temperature, the pressure will ____________________.
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increase
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A solution is ____________________
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homogenous mixture
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A student desires to remove the odor of naphthalene, a nonpolar aromatic hydrocarbon, from his laboratory coat. Which solvent would you suggest?
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benzene (nonpolar)
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The rate of solution of glucose in water will NOT be increased by `
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higher pressure
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The molarity of a solute in a solution is the number of
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moles of solute per liter of solution
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When one mole of LiBr is dissolved in one kilogram of water, the concentration of the Br (with a negative sign up in the air) is
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1.0 molar
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Which of the following is not a colligative property of a solution?
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color
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Which of the following is not an example of a colloid?
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fruit punch
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A solution has a variable rather than a fixed composition
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true
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The process of separation solutes from each other involves the absorption of heat.
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? Chapter 12 number 12
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Gases are generally more soluable at higher temperatures than at lower temperatures.
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false
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Percent by mass is defined as the mass of the solute divided by the mass of the solvent multiplied by 100%.
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true.
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The abbreviation for molarity is M.
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true
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I skipped these 2 questions because they were bonus, and I didn't know if you had been given the correct answers or not.
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Chapter 12 numbers 16 & 17
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Colligative properties depend on the type, not the number, of particles in solution.
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false
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Substances that cannon be broken apart by water molecules.
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insoluble
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Two substances when mixed together do not form a solid.
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immiscible
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Addition of solutes affects the boiling point
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boiling pint elevation
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addition of solutes affects the freezing point
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freezing point elevation
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An endothermic reaction involves
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a gain of energy in the form of heat
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An exothermic reaction involves
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breaking of weaker bonds to from stronger bonds
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Which of the following has the greatest entropy?
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1 mole of NaCl (g) at 50 degrees Celsius
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According to the __________, the enthalpy change of a reaction equals the sum of the enthalpy changes for each step of the reaction.
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Hess's Law
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Thermochemistry can answer the question "Can 2 substance react together?"
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true
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Spontaneous reactions always occur rapidly.
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false
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Energy is always required to break bonds.
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true
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When ice melts, entropy increases.
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True
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The stronger the bond, the less energy released when it forms.
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false
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A reaction is favorable if the free energy change is negative.
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true
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The lower the specific heat of a substance is, the more heat will be required to cause a temperature change in the substance.
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false
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According to the laws of thermodynamics, the universe could not have formed spontaneously.
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true
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The heat that, when applied to a substance, results in bonds breaking but no temperature change.
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latent heat
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The heat that, when applied to a substance, results in a temperature change in the substance.
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sensible heat
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States that energy can be neither created nor destroyed.
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first law of thermodynamics
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An equation that combines the change in enthalpy and the change in entropy.
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Gibbs free energy
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States that natural processes decrease the order of the universe.
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collision theory
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Explains why reactions occur at greater rates, depending on reaction conditions.
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enthalpy of reeaction
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A single criterion for favorability for a reaction to occur.
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second law of thermodynamics
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The quantity represented by (a small triangle or delta sign in front of) H
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free energy
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Which of the following is a special and distinct class of catalysts comprised of naturally occurring biological substances.
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enzyme
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Solid materials that are capable of adsorbing molecules of gases or liquids onto their surfaces are called ________ catalysts.
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heterogeneous
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Any substance that changes a reaction rate without being permanently changed or consumed is called a _________________.
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catalyst
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The process of molecules of one substance collecting on the surface of another is called
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adsorption
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Rate laws are determined
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experimentally
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Doubling the concentration of a reactant always causes the reaction rate to double.
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false
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Spontaneous reactions always occur rapidly.
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false
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A catalyst does not affect the concentration of products formed in a reaction; it only affects the rate at which they are produced.
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true
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A reaction that has a large activation energy is more likely to occur than a reaction with a low activation energy.
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false
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Any factor that increases the number of effective collisions increases the reaction rate.
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true
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A rate law with a specific rate constant allows you to calculate how fast a reaction will occur.
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true
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A thermodynamically favorable reaction proceeds spontaneously.
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false
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Indicates how the rate of a reaction is affected by a specific reactant's concentration
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reaction order
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the study of the rates of reaction and the steps by which they occur
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kinetics
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the minimum amount of kinetic energy that must be possessed by reactants before they can react
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activation energy
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a theoretical, unstable, high-energy, transitional substance in a reaction
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activated complex
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usually tells how fast reactants change into products
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reaction rate
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the series of steps that make up a reaction
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reaction mechanism
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an equation that mathematically describes how fast a reaction can occur
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rate law
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explains why reaction occur at greater or slower rates, depending on reaction conditions
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collision theory
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What states than when an equilibrium is stressed, it will proceed in the direction that will relieve the stress?
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Le Chatelier's principle
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Once a chemical system reaches equilibrium, there is no further reaction between the particles of the reactants and the products.
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true (check chapter 15 # 13)
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An increase in temperature favors the exothermic reaction in an equilibrium reaction.
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true (check chapter 15 # 14)
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Adding a catalyst changes the value of the equilibrium constant
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true ((check chapter 15 # 15)
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If the produce of the concentrations of the ions making up the solution is greater than the K(with a subscript sp) for the precipitate, the solution is supersaturated.
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true
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Le Chatelier's principle indicates that when the equilibrium of a reaction is disturbed,it reacts to minimize the disturbance.
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true
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When the pressure of a system in equilibrium is decreased, the system will favor the direction of the smaller number of moles of gas to reestablish equilibrium.
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false
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There are quite a few questions from test chapter 15 that I could not type.
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There are quite a few questions from test chapter 15 that I could not type.
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At 25 degrees Celcius, what does the pH + the pOH equal
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0
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A neutralization reaction produces both water and
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? Chapter 15 (it says 15 but I think it's really 16) number 5
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The strength of an acid is determined by
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how many types of particles are in the solution
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What do indicators tell?
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the pH of a solution
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Why would you do a titration?
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to determine if a buffer should be used
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The Lewis definitions deal with an acid donating or taking protons.
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false ? it says 15 but I think it's really 16 # 11)
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Buffers help to maintain a neutral pH.
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false
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Acids taste sour.
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true
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When acids lose protons, it is called protonation.
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false
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If an acid is strong, its conjugate base must be weak.
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true
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All Arrhenius acids are Bronsted-Lowry acids.
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true
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When sulfur changes from an oxidation state of -2 to +6 in the sulfate ion, the sulfur must
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lose 8 electrons
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The gaining of electrons by an ion or atom is
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reduction
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The losing of electrons by an ion or atom is
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oxidation
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All of the following changes in oxidation represent oxidation with the exception of
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-1 to -3
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An oxidizing agent is a substance that
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supplies electrons
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Oxidation reaction always involve the element oxygen.
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false
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Redox reactions can occur only when electrons are transferred between metals and nonmetals.
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false
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Oxidation and reduction are simultaneous reactions.
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true
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In redox reactions, the reducing agent gains electrons.
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false
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