Abeka Chemistry Test 9 (Nine-weeks Exam)

chlorine

halogen used in the disinfection of drinking water and the synthesis of medicines, crop-protection chemicals, and PVC plastics

hydrogen

the most abundant element in the universe

helium

noble gas used as a lifting gas in airships and weather balloons, as an extremely low-temperature coolant, and as a laser medium

hydrogen

isotopes are commonly called protium, deuterium, and tritium

nitrogen

extracted from the air and used to make artificial fertilizers and explosives

oxygen

a gas found in air that is necessary for the survival of human and animals

oxygen

ozone is an allotrope of this element

fluorine

halogen used in dental hygiene and in the manufacture of refrigerants

phosphorus

exists in an unstable white allotrope and a more stable red allotrope; used to make matches and some fertilizers

sulfur

extracted from petroleum and natural used to make an important gas by the Claus process; industrial acid

metallurgy

the science of extracting metals from their ores and preparing them for use

electrolytes

substances that dissolve in water to produce ions that can conduct an electrical current

Le Chatelier's

the effects of changes on equilibrium systems is described by _________ principle

kinetics

the study of reaction rates and pathways is chemical _____?

activation energy

the minimum kinetic energy that a molecule must possess to undergo a chemical reaction is the _________?

catalyst

a substance that increases the rate of a chemical reaction without being consumed in the reaction is a _________?

sodium

alkali metal found in lye, washing soda, baking soda, and table salt

aluminum

the most abundant metal in the earth's crust; a lightweight metal widely used to make aircraft, spacecraft, and beverage cans

iron

the second most abundant metal in the earth's crust; a lightweight metal widely used to make aircraft, spacecraft, and beverage cans

gold

the most malleable and ductile metal known

platinum

precious metal used in automotive and industrial catalysts

silicon

most common semimetal; found in computer chips, glass, and sand

iron

the metal most commonly refined by means of blast furnaces

calcium

alkaline earth metal that helps compose limestone, slaked lime, and cement

copper

metal used in electrical wiring and as a component of brass and bronze

Which of the following changes would not increase the rate of a chemical reaction?

diluting reactant concentrations

A solution that contains as much dissolved solute as possible under equilibrium conditions is said to be ______?

saturated

The theory that when two molecules collide and chemically react they form a short-lived activated complex before breaking apart to form the products is the _______?

transition-state

Which of the following statements about catalysts is true?

a catalyst increase the reaction by lowering the reaction's activation energy

The rate of a chemical reaction is usually measured as ______?

the change in concentration of a given substance per unit of time

In a solution of sodium chloride in water, water is the ______?

solvent

Which of the following statements best describes a system at equilibrium?

Rates of forward and reverse reactions are equal

The flow of solvent through a semipermeable membrane from a more dilute solution to a more concentrated solution is called

osmosis

A mixture of two or more metals, usually melted together, is a ________?

alloy

A mixture containing tiny clumps or particles that remain suspended within the mixture and will not settle out is ______?

colloid

If the temperature of a chemical reaction is increased from 20C to 30C, we would ordinarily expect the reaction rate to __________?

double

T/F: a nonpolar substance will be more likely to dissolve in a polar solvent than in a nonpolar solvent

F, polar

T/F: a factor that causes a change in an equilibrium system is called a disturbance

F, stress

T/F: protein catalysts found in living things are enzymes

T

T/F: The energy diagram below represents an endothermic reaction

T

T/F: if a nonvolatile solute such as glucose is added to water, the boiling point will increase

T

T/F: When a gas is dissolved in water, decreasing the temperature tends to decrease the solubility of the gas

F, increase

T/F: A chemical system in which the rates of reaction in opposite directions have equalized so that the concentration of reactants and products is constant is in a state of chemical equilibrium

T

Removing the hydrogen iodide as soon it is formed would shift the equilibrium to the ________?

right

Increasing the pressure would shift the equilibrium to the _______?

No shift would occur

Adding a catalyst to the system would cause the concentration of HII to ________?

remain unchanged

Increasing the temperature would shift the equilibrium to the ________?

left

Adding hydrogen to the system would cause the concentration of HI to shift to the ________?

right

Adding iodine vapor to the system would shift the equilibrium to the _______?

right

Removing hydrogen iodide from the system would cause the concentration of iodine to __________?

decrease

What is the molarity of a solution containing 6.0 mol NaCL dissolved in 12 L of water?

0.50 M

For the reaction 3 Fe9 (s) + 4 H2 (g) in what direction does adding a catalyst shift the equilibrium

No shift would occur

For the reaction AgH2C2O3 -> Ag (aq) + H2C3O2 (aq), in what direction does an increase in pressure shift the equilibrium

No shift would occur

Write the equilibrium constant expression for the reaction 2 NO(g) + Br2 -> 2 NOBr (g)

K = NOBr2
No2Br2

Which of the following would not cause the reaction 2Al(s) + 6 HCl(aq) -> 3 H2 (g) + 2 AlCl3 (aq) to shift to the right?

increasing the pressure o the reaction chamber

Write the equilibrium constant expression for the reaction CaCl2(s) + 2 HCl(aq) -> CaCl2(aq)

K = CaCl2CO2
HCl2

Write the solubility product constant expression for aluminum hydroxide

K = AL-3OH-3

supersaturated

The solubility product of Ag2Co3 is 8.1 x 10-12. Is a 1.5 x 10-4 M solution of Ag2NO3, saturated, unsaturated, or supersaturated

Calculate K

290

Calculate NO

1.1 x 10 -5 M