Abeka 11th Grade Chemistry Test 9

A chemist is trying to precipitate silver sulfate using the following reaction. (14.3)

H2SO4

What law states that the higher the particle pressure of a gas, the greater the solubility of the gas at a given temperature? (12.2)

Henry's law

What is the best explanation for why a catalyst does not affect the final concentrations at equilibrium? (14.2)

It alters the rates of both the forward and reverse reactions equally.

What is the Ksp expression for Mg(OH)2? (14.3)

Ksp = [Mg2+][OH-] to the power of 2

What principle is used to determine how a stress will affect an equilibrium reaction? (14.2)

Le Chatelier's principle

What process is used to produce nitric acid? (10.2)

Ostwald process

In general, what effect does a 10°C rise in temperature have on reaction rate? (13.1)

Rate doubles

What is the best reason that phosphorous compounds can cause eutrophication? (10.2)

They act as fertilizer for algae in lakes and streams.

What phenomenon causes light passed through a colloid to be scattered and have a blue tinge? (12.6)

Tyndall effect

What is a short-lived, high-energy, unstable arrangement of atoms formed briefly during a reaction? (13.2)

activated complex

most abundant metal; used as a lightweight structural material (11.1)

aluminum

What is the ratio of the mole amount of a solute to the volume of a solution? (12.3)

amount concentration

Which of the following substances should an equilibrium constant expression include? (14.3)

aqueous solution

Which alkaline earth metal is a major component of limestone? (11.1)

calcium

What is the study of rates of reactions and the pathways taken by reactions? (13.1)

chemical kinetics

Which halogen is used in household bleaches and disinfectants as well as in most medicines? (10.3)

chlorine

What is the general term for properties that depend on the number of particles and not on the identity of the particles? (12.4)

colligative property

What type of reaction involves a substance reacting with oxygen to produce carbon dioxide, water, heat, and light? (10.2)

combustion

second most conductive metal; used in electrical wiring (11.2)

copper

What is the equilibrium constant expression for the following equilibrium reaction? (14.3) Ni(s) + 4 CO(g) <-----> Ni(CO)4 (g)

d. K = [Ni(CO)4] / [CO] to the 4th power

What term refers to the separation of ions from each other that occurs when an ionic compound is placed in a solvent? (12.1)

dissociation

Chemical equilibrium is a state of ____equilibrium. (14.1)

dynamic

Refining steel by using electricity to melt and purify the metal is the ____ process. (11.2)

electric arc

What are catalysts found in living cells and organs called? (13.3)

enzymes

When a system is in chemical equilibrium, the opposing rates of reactions are ____. (14.1)

equal

most reactive element (10.3)

fluorine

Which noble gas is used as a low-temperature coolant in scientific research and to dilute oxygen in air used by deep-sea divers? (10.3)

helium

A catalyst that exists in the same phase as the reactants is a _____ catalyst. (13.3)

homogeneous

What is the most abundant element in the universe? (10.1)

hydrogen

The primary use of the main-group metal _____ is in car and truck batteries. (11.1)

lead

Increasing the temperature of an exothermic reaction shifts the equilibrium to the ____ (14.2)

left

What equilibrium shift will adding O2 cause? (14.2)

left

What equilibrium shift will decreasing temperature cause? (14.2)

left

What does a small Ksp indicate about a substance's solubility? (14.3)

low solubility

What is the science of extracting metals from their naturally occurring materials and preparing them for use? (11.1)

metallurgy

Liquids that are completely soluble in each other in all proportions are _____ (12.1).

miscible

What is the ratio of the mole amount of a solute to the solvent mass? (12.3)

molality

main component of air; used in the production of ammonia (10.2)

nitrogen

What equilibrium shift will adding a catalyst cause? (14.2)

no shift

What is the general terms for salts of phosphoric acid? (10.2)

phosphates

has red and white allotropes; used in the manufacture of strike-anywhere matches (10.2)

phosphorus

Which precious metal is used as a catalyst in pollution-control devices? (11.2)

platinum

A graph showing how energy changes as a reaction progresses is a ____ diagram. (13.2)

potential energy

What is a reaction in which aqueous compounds exchange ions to form an insoluble solid called? (12.5)

precipitation

What is the process of quickly cooling red-hot metal by dipping it in a bath of cold water or oil to increase the hardness? (11.2)

quenching

What is an equation that relates reaction rate to reactant concentrations called? (13.4)

rate law

A series of steps that describes the way in which a reaction proceeds is a _____ (13.4)

reaction mechanism

A reaction that involves the transfer of electrons between atoms is called a _____ reaction. (12.5)

redox

What is the term for a reaction that can be made to go either direction? (14.1)

reversible reaction

A large value of K means that an equilibrium reaction lies to the left. (14.3)

right

What equilibrium shift will increasing the pressure cause? (14.2)

right

What type of solution contains as much solute as possible under equilibrium conditions? (12.2)

saturated

Which silicon compound forms glass when it is melted ad cooled? (11.3)

silica

second most abundant element; used in the manufacture of computer chips and electronic devices (11.3)

silicon

What is the term for the equilibrium constant of a solution equilibrium? (14.3)

solubility product constant

has several elemental allotropes; important element in thiols (10.2)

sulfur

What compound of sulfur is the most important industrial chemical in the United States? (10.2)

sulfuric acid

What is a heterogeneous mixture with particles large enough to settle out of the dispersing medium? (12.6)

suspension

Which of the following is the best description of a state of chemical equilibrium? (14.1)

the rates of the forward and the reverse reactions are equal.

Honey is a supersaturated solution of sugars. Which of the following techniques can be used to turn crystallized honey back into a liquid? (12.2)

warming

The solubility of PbCl2 if 0.450 g/100mL solution. What is the solubility product constant? The molar mass of PbCl2 is 278.1 g/mol.

1.69 x 10 to the -5 power

For the reaction HC2 H3O2(aq) + H2O <-------> H3O(l) + C2H3O2-(aq), the equilibrium concentrations at 25 degrees Celsius in a particular experiment where [HC2H3O2] = 0.966 mol/L, [H3O+] = 3.98 x 10 to the -3 mol/L, and [C2 H3 O2-] and [C2H3O2-] = 4.52 x 10 to the -3 mol/L. What is the value of K at 25 degrees Celsius.

1.86 x 10 to the -5

A chemist mixes 15.0 mL of 1.35 mol/L BaCl2 with excess K2SO4 (aq). What mass of BaSO4 forms? The molar mass of BaSO4 is 233.39 g/mol. BaCl2 (aq) + K2 SO4(aq) ------> BaSO4(s) + 2 KCl(aq) (0.0150)(1.35)(1 mol/1 mole)(233.39)

4.73

What mass of CuSO4 is needed to prepare 125 mL of 0.35 mol/L solution? The molar mass of CuSO4 is 159.60 g/mol. n=VC (0.125 L)(0.35 mol/L) = 0.043 75 Take that and multiply buy 159.60

6.98 g = 7.0g

Calcium hydroxide is a slightly soluble salt. Although it ionizes completely in solution, a calcium hydroxide solution conducts electricity poorly. What is the best explanation for this behavior? (12.4)

A saturated solution contains very few dissolved ions.