Chem II Final Exam

The volume of a sample of oxygen is 300.0 mL with the pressure is 1.00 ATM and the temperature is 27.0°C. At what temperature is the volume 1.00L and the pressure of 0.500 ATM? A. 22.0°C B. 45.0°C C. 0.50 K D. 227°C

D. 227°C

A 1.00 L sample of a gas has a mass of 1.25 g at STP. What is the mass of 1.00 mol of this gas? A. 0.855 g B. 1.25 g C. 22.4 g D. 28.0 g

D. 28.0 g

How many moles of ions are produced by the dissociation of 1 mol of MgCl2? A. 0 B. 1 mol C. 2 mol D. 3 mol

D. 3 mol

A sample of oxygen occupies 560. mL when the pressure is 800.00 mm Hg. At constant temperature, what volume does a gas occupy when the pressure decreases to 700.0 mm Hg? A. 80.0 mL B. 490. mL C. 600. mL D. 640. mL

D. 640. mL

The molar enthalpy of fusion for water is 6.008 KJ/mol. What quantity of energy is released 253 g of liquid water freezes? (Molar mass of water is 18.02 g/mol) A. 759KJ B. 0.429 KJ C. 2.33 KJ D. 84.4 KJ

D. 84.4 KJ

Which of the following expresses concentration? A. Molality B. Molarity C. Moles of solute per liter of solution D. All of the above

D. All of the above

The name if a binary acid A. Has no prefix B. Begins with the prefix Bi- C. Ends with the suffix -ous D. Begins with the prefix hydro-

D. Begins with the prefix hydro-

Bases taste A. Soapy B. Sour C. Sweet D. Bitter

D. Bitter

Which of these can happen due to decreasing the average energy of a liquid's particles? A. Vaporization B. Evaporation C. A random arrangement D. Freezing

D. Freezing

Pressure has the greatest effect on the solubility of A. Solids in liquids B. Liquids in liquids C. Gases in gases D. Gases in liquid

D. Gases in liquid

Which of the following is an amorphous solid? A. Ice B. Diamond C. Graphite D. Glass

D. Glass

The formula for the hydronium ion is A. H+ B. H2O+ C. H3O- D. H3O+

D. H3O+

At 7.0°C, the volume of a gas is 49 mL. At the same pressure, its volume is 74 mL at what temperature? A. 3.0°C B. 423°C C. 120°C D. 150°C

D. 150°C

Iron ( IV ) oxide, FeO2, is produced by the reaction of Fe + O2 -> FeO2 ( 87.8 g/mol ). How many grams of FeO2 can be produced from 50.0 L of O2 at STP? A. 19.5 g B. 37.8 g C. 50 g D. 196. g

D. 196. g

How many ions are produced by each formula unit of solid in a dissociation? A. 0 B. 1 C. 2 D. 2 or more

D. 2 or more

Which of the following has components in a nonuniform arrangement? A. Homogeneous mixture B. Solution C. Salt Water D. Heterogeneous mixture

D. Heterogeneous mixture

Which of the following pairs of solutions produces a precipitate when combind? A. KOH and NH4Cl B. Fe(NO)3 and KCl C. Na2SO4 and KCl D. NH4Cl and AgNO3

D. NH4Cl and AgNO3

Which ions do not appear in the net equation for the precipitation reaction involving solutions of Zn(NO3)2 and Na3PO4? A. Zn^2+(aq) and NO3^-(aq) B. Na+(aq) and Zn^2+(aq) C. Zn^2+(aq) and PO4^3-(aq) D. Na^+(aq) and NO3^-(aq)

D. Na^+(aq) and NO3^-(aq)

What is the spectator ion in the equation Cu^2+(aq) + Zn^2+(aq) -> CuS(s) + ZnS(s) A. Cu^2+ B. Zn^2+(aq) C. S^2-(aq) D. None of the above

D. None of the above

When solutions of NH4OH and K2SO4 are combined, what precipitate(s) forms? A. (NH4)2SO4 B. KOH C. (NH4)2SO4 and KOH D. None of the above

D. None of the above

What is the value of the gas constant? A. 0.0821 L ATM/mol K B. 0.281 L ATM C. 0.0281 L ATM/mol K D. 0.0821 mol K

A. 0.0821 L ATM/mol K

A sample of gas at 25°C has volume of 11 L and exerts a pressure of 660 mm Hg. How many moles of gas are in the sample? A. 0.39 mol B. 3.9 mol C. 9.3 mol D. 87 mol

A. 0.39 mol

If 0.5 L of O2 ( g ) reacts with H2 to produce 1 L of H2O ( g ), what is the volume of H2O, ( g ) obtained from 1 L of O2 ( g )? A. 0.5 L B. 1.5 L C. 2 L D. 2.5 L

C. 2 L

How many moles of ions are produced by the dissociation of 1 mol of NH4Br? A. 0 B. 1 mol C. 2 mol D. 5 mol

C. 2 mol

Which of the following is a binary acid? A. H2SO4 B. CH3COOH C. HBr D. NaOH

C. HBr

What is the number of moles of H2 to produce when 23 g of sodium react with water according to the equation 2Na ( s ) + 2H2O ( l ) -> 2NaOH ( aq ) + H2 ( g )? A. 0.50 mol B. 1.0 mol C. 2.0 mol D. 4.0 mol

A. 0.50 mol

What is the molarity of a solution that contains 125 g NaCl in 4.00 L solution? (Molar mass of NaCl = 58.44 g/mol) A. 0.535 M B. 2.14 M C. 8.56 M D. 3.13 M

A. 0.535 M

How many milliliters of a 0.171 M solution contain 1.00 g of NaCl? (Molar mass of NaCl = 58.44 g/mol) A. 100. mL B. 1000. mL C. 171 mL D. 17.1 mL

A. 100. mL

The standard molar volume of a gas at STP is A. 22.4 L B. g/22.4 L C. g-mol wt/22.4 L D. 1 L

A. 22.4 L

The standard molar enthalpy of vaporization for water is 40.79KJ/mol. What mass of steam is required to release 500. KJ of energy upon condensation? (Molar mass of water is 18.02 g/mol) A. 221 g B. 325 g C. 1130 g D. 1660 g

A. 221 g

Which of the following is the right side of the equation for dissolving K2S(s)? A. 2K^+(aq) + S^2-(aq) B. K2^2+(aq) + S^2-(aq) C. K^2+(aq) + S^2-(aq) D. 2K(aq) + S(aq)

A. 2K^+(aq) + S^2-(aq)

#26 -chart- A sample of gas is collected by water displacement at 600.0 mm Hg and 30°C. What is the partial pressure of the gas? A. 568.2 mm Hg B. 600.0 mm Hg C. 630 mm Hg D. 631.8 mm Hg

A. 568.2 mm Hg

The volume of a gas is 93 mL when the temperature is 91°C. If the temperature is reduced to 0°C without changing the pressure, what is the new volume of the gas? A. 70. mL B. 93 mL C. 120 mL D. 273 mL

A. 70. mL

#25 -chart- what is the partial pressure of water vapor in oxygen gas collected by water displacement at 10°C and 750 mm Hg? A. 9.2 mm Hg B. 740.8 mm Hg C. 6.5 mm Hg D. 750.8 mm Hg

A. 9.2 mm Hg

At pressures is greater than one ATM, water will boil at A. A temperature higher than 100°C B. A temperature lower than 100°C C. 100°C D. 4°C

A. A temperature higher than 100°C

Bases react with A. Acids to produce salts and water B. Salts to produce acids and water C. Water to produce acids and salts D. Neither acids, salts, nor water

A. Acids to produce salts and water

Which is an example of effusion? A. Air slowly escaping from a pinhole in a tire B. The aroma of a cooling pie spreading across a room C. helium dispersing into a room after a balloon pops D. Oxygen and gasoline fumes mixing in an automobile carburetor

A. Air slowly escaping from a pinhole in a tire

According to the kinetic-molecular theory, particles of matter A. Are in constant motion B. Have different shapes C. Have different colors D. Are always fluid

A. Are in constant motion

#17 -graph- according to the figure, what is the most volatile substance shown? A. Benzene B. Water C. Toluene D. Aniline

A. Benzene

If the temperature of a liquid vapor system at equilibrium is reduced, the A. Concentration of the vapor will decrease B. Rate of evaporation will increase C. Equilibrium is unaffected D. Percentage of liquid in the system will decrease

A. Concentration of the vapor will decrease

What is the net equation for the precipitation reaction between copper(II) chloride and sodium hydroxide? A. Cu^2+(aq) + 2OH^-(aq) -> Cu(OH)2(s) B. Na^+(aq) + Cl^-(aq) -> NaCl(s) C. Cu^2+(aq) + 2OH^-(aq) + 2Cl^-(aq) -> Cu(OH)2(s) + 2 Cl^-(aq) D. Cu^2+(aq) + 2Cl^-(aq) + 2Na^+(aq) + 2OH^-(aq) -> Cu(OH)2(s) + 2NaCl(s)

A. Cu^2+(aq) + 2OH^-(aq) -> Cu(OH)2(s)

Nonvolatile solutes A. Depress freezing point and elevate boiling point B. Elevate freezing point and depress boiling point C. Depress both freezing point and boiling point D. Elevate both freezing point and boiling point

A. Depress freezing point and elevate boiling point

Which substance has the lowest density? A. H2O(g) B. H2O(l) C. Hg(l) D. Hg(g)

A. H2O(g)

Dissolving HCl in water produces A. H3O+ and Cl- B. H+ and Cl- C. H3OCl(aq) D. H3O- and Cl+

A. H3O+ and Cl-

Diffusion between two gases occurs most rapidly if the gases are at A. High temperature and the molecules are small B. Low temperature and the molecules are large C. Low temperature and the molecules are small D. High temperature and the molecules are large

A. High temperature and the molecules are small

The solubility of gases in liquid A. Increases with increasing pressure B. Cannot reach equilibrium C. Decreases with increasing pressure D. Does not depend on pressure

A. Increases with increasing pressure

Increasing the surface area of the solute A. Increases the rate of dissolution B. Decreases the rate of dissolution C. Has no effect on the rate of dissolution D. Can increase, decrease, or have no effect on the rate of dissolution

A. Increasing the rate of dissolution

Why is vapor-pressure lowering a colligative property? A. It is independent of the concentration of a non-electrolyte solute and does not depend on solute identity B. It depends on the concentration of an electrolyte solute and does not depend on solute identity C. It depends on the concentration of a non-electrolyte solute and on solute identity D. It depends on the concentration of an electrolyte solute and on solute identity

A. It is independent of the concentration of a non-electrolyte solute and does not depend on solute identity

"Like dissolves like" is a very general rule used for predicting whether A. One substance will form a solution with another B. One substance will react with another C. A reaction will reach equilibrium D. A mixture will contain two or three phases

A. One substance will form a solution with another

All of the following equations are statements of ideal gas law except A. P = nRTV B. PV/T = nR C. P/n = RT/V D. R = PV/nT

A. P = nRTV

The rate of diffusion in solids is very low because the A. Particles are not free to move about B. Surfaces of solids usually contact gases C. Attractive forces are weak D. Melting points are high

A. Particles are not free to move about

What is the actual freezing point depression of a 0.020 m aqueous NaCl solution? Kf = -1.86°C/m A. Slightly less than -0.0744°C B. Exactly -0.0744°C C. Slightly more than -0.0744°C D. Exactly 0°C

A. Slightly less than -0.0744°C

Which of the following is an electrolyte? A. Sodium chloride B. Sugar C. Pure water D. Glass

A. Sodium chloride

Forces holding particles together are strongest in a A. Solid B. Liquid C. Gas D. Vapor

A. Solid

An equation for the dissociation of an ionic solid shows A. The solid on the left side and aqueous ions on the right B. An aqueous solid on the left side and ions on the right side C. Aqueous ions on the left side and the solid on the right side D. Ions on the left side and an aqueous solid on the right side

A. The solid on the left side and aqueous ions on the right

If gas A has a molar mass greater than that of gas B and samples of each gas at identical temperatures and pressures contain equal numbers of molecules, then A. The volumes of gas A and gas B are equal B. The volume of gas A is greater than that of gas B C. The volume of gas B is greater than that of gas A D. Their volumes are proportional to their molar masses

A. The volumes of gas A and gas B are equal

V is original volume, V' is the new volume, T is the original Kelvin temperature, and T' is the new Kelvin temperature, how is Charles law expressed mathematically? A. V = V' T/T' B. V = V ( T/T' ) C. V = V - ( T/T' ) D. V = ( V/T' ) + T

A. V = V' T/T'

What is the approximate freezing point depression of a 0.050 m aqueous Na2SO4 solution? Kf = -1.86°C/m A. -0.11°C B. -0.28°C C. -0.22°C D. -0.39°C

B. -0.28°C

In the reaction represented by the equation N2 ( g ) + 2O2 ( g ), what is the volume ratio of N2 to NO2? A. 1:1 B. 1:2 C. 2:1 D. 2:5

B. 1:2

What is the net ionic equation for the precipitation reaction between silver nitrate solution and sodium sulfide solution? A. 2Ag^+(aq) + 2NO^3-(aq) + 2Na^+(aq) +S^2-(aq) -> Ag2S(s) + 2Na^+(aq) +2No3^-(aq) B. 2Ag^+(aq) + S^2-(aq) ->Ag2S(s) C. Na^+(aq) + No#^-(aq) -> NaNo3(s) D. 2Ag^+(aq) + 2NO3^-(aq) + 2Na^+(aq) + S^2-(aq) -> Ag2S(s) + 2NaNO3(s)

B. 2Ag^+(aq) + S^2-(aq) ->Ag2S(s)

Standard pressure is the pressure exerted by a column of mercury exactly A. 273 mm high B. 760 mm high C. 760 cm high D. 1.00 m high

B. 769 mm high

Compared with a 0.01 m sugar solution, a 0.01 m KCl solution has A. The same freezing point depression B. About twice the freezing point depression C. the same freezing point elevation D. About six time the freezing point elevation

B. About twice the freezing point depression

Which of the following is the right side of the equation for dissolving Al(NO3)3? A. Al^+ + (N)3)3^- B. Al^3+(aq) + 3NO3^-(aq) C. Al^3+ + NO3^3- D. Al^3-(aq) + 3NO3^+(aq)

B. Al^3+(aq) + 3NO3^-(aq)

A metal solution is a(n) A. Colloid B. Alloy C. Suspension D. Emulsion

B. Alloy

Two gases with unequal molar masses are injected into opposite ends of a long tube at the same time and allowed to diffuse toward the center. They should begin to mix A. In approximately five minutes B. Closer to the end that holds the heavier gas C. Closer to the end that holds the lighter gas D. Exactly in the middle

B. Closer to the end that holds the heavier gas

Effervescent is the A. Dissolution of gas in liquid B. Escape of gas from a gas-liquid solution C. Escape of liquid from a liquid-liquid solution D. Escape of solid from a solid-liquid solution

B. Escape of gas from a gas-liquid solution

A volatile liquid A. Has strong attractive forces between particles B. Evaporates readily C. Has no odor D. Is ionic

B. Evaporates readily

Which term best describes the process by which particles escape from the surface of a non-boiling liquid and enter the gas state? A. Sublimation B. Evaporation C. Surface tension D. Aeration

B. Evaporation

By which process do gases take the shape of their container? A. Evaporation B. Expansion C. Adhesion D. Diffusion

B. Expansion

Which of the following is not a net ionic equation? A. Ag^+(aq) + Cl^-(aq) -> AgCl(s) B. Fe^2+(aq) + 2Cl^-(aq) + 2OH^-(aq) -> Fe(OH)2(s) + 2Cl^-(aq) C. 3Ca^2+(aq) + 2P^3-(aq) -> Ca3P2(s) D. Cu^2+(aq) + S^2-(aq) -> CuS(s)

B. Fe^2+(aq) + 2Cl^-(aq) + 2OH^-(aq) -> Fe(OH)2(s) + 2Cl^-(aq)

Which of the following is chlorous acid? A. HClO B. HClO2 C. HClO3 D. HClO4

B. HClO2

The hydrogen ion A. Has a charge of 2+ B. Is a proton C. Has a negative charge D. Is a bare electron

B. Is a proton

Why is freezing-point depression a colligative property? A. It is inversely proportional to the molal concentration of a solution B. It is directly proportional to the molal concentration of a solution C. It does not depend on a molal freezing-point constant for each solvent D. It depends on the properties of an electrolyte in a solvent

B. It is directly proportional to the molal concentration of a solution

Water in air is an example of which solute-solvent combination? A. Gas-liquid B. Liquid-gas C. Liquid-liquid D. Gas-gas

B. Liquid-gas

A substance whose water solution is a poor conductor of electricity is a(n) A. Polar substance B. Non-electrolyte C. Electrolyte D. Ionic substance

B. Non-electrolyte

Compared with a 0.01 m sugar solution, a 0.01 m KCl solution has A. The same boiling point elevation B. Roughly twice the boiling point elevation C. The same boiling point depression D. About half the boiling point depression

B. Roughly twice the boiling point elevation

Which mixture is made up if the smallest particles? A. Milk B. Salt water C. Shaving cream D. Muddy water

B. Salt water

Acids taste A. Sweet B. Sour C. Bitter D. Salty

B. Sour

The triple point of a substance is the temperature and pressure conditions at which A. Density is greatest B. States of a substance coexist at equilibrium C. Equilibrium cannot occur D. Kinetic energy is at a minimum

B. States of a substance coexist at equilibrium

Colligative Properties depend on A. The identity of the solute particles B. The concentration of the solute particles C. The physical properties of the solute particles. D. The boiling point and freezing point of the solution

B. The concentration of the solute particles

If the amount of solute present in a solution at a given temperature is less than the maximum amount that can dissolve at that temperature, the solution is said to be A. Saturated B. Unsaturated C. Supersaturated D. Concentrated

B. Unsaturated

Particles within a solid A. Do not move B. Vibrate about fixed positions C. Move about freely D. Exchange positions easily

B. Vibrate about fixed positions

What is the approximate freezing-point depression of a 0.010 m aqueous CaCl2 solution? Kf = -1.86°C/m A. -0.019°C B. -0.037°C C. -0.056°C D. -0.074°C

C. -0.056°C

What is the molality of a solution that contains 31.0 g HCl in 5.00 kg water? (Molar mass of HCl = 36.46 g/mol) A. 0.062 m B. 0.425 m C. 0.170 m D. 15.5 m

C. 0.170 m

The volume of a gas is 400.0 mL when the pressure is 1.00 ATM. At the same temperature, what is the pressure at which the volume of the gas is 2.0 L? A. 0.5 ATM B. 5.0 ATM C. 0.20 ATM D. 800 ATM

C. 0.20 ATM

A water solution containing an unknown quantity of a nonelectrolyte solute has a freezing point of -0.665°C. What is the molal concentration of the solution if Kf = -1.86°C/m? A. 0.010 m B. 0.355 m C. 0.358 m D. 2.66 m

C. 0.358 m

Standard temperature is exactly A. 100°C B. 273°C C. 0°C D. 0 K

C. 0°C

The concentration of a water solution of NaCl is 2.48 m, and it contains 806 g of water. How much NaCl is in the solution? (Molar mass of NaCl = 58.4 g/mol) A. 2.00 g B. 89.3 g C. 117 g D. 224 g

C. 117 g

Calculate the approximate temperature of a 0.50 mol sample of gas at 750 mm Hg and a volume of 12 L. A. -7°C B. 11°C C. 15°C D. 288°C

C. 15°C

What is the pressure exerted by 1.2 mol of a gas with a temperature of a 20.°C and a volume of 9.5 L? A. 0.030 ATM B. 1.0 ATM C. 3.0 ATM D. 30. ATM

C. 3.0 ATM

Acids generally release H2 gas when they react with A. Nonmetals B. Semimetals C. Active metals D. Inactive metals

C. Active metals

When solutions of BaCO3 and Fe2(SO4)3 are combined, what precipitate(s) forms? A. BaSO4 B. Fe2(CO3)3 C. BaSO4 and Fe2(CO3)3 D. None of the above

C. BaSO4 and Fe2(CO3)3

What is the net ionic equation for the precipitate reaction between BaCl2 and N2SO4? A. BaCl2(aq) + Na2SO4(aq) -> BaSO4(s) + 2NaCl(aq) B. Na^+(aq) + Cl^-(aq) -> NaCl(s) C. Ba^2+(aq) + SO4^2-(aq) -> BaSO4(s) D. Ba^2+(aq) + 2Cl^-(aq) + 2Na^+(aq) + SO4^2-(aq) -> BaSO4(s) + 2Cl^-(aq) + 2Na^+(aq)

C. Ba^2+(aq) + SO4^2-(aq) -> BaSO4(s)

Stirring increases the rate of dissolution because it A. Raises the temperature B. Lowers the temperature C. Brings fresh solvent into contact with the solute D. Decreases the surface are of the solute

C. Brings fresh solvent into contact with the solute

Which compound dissociates to produce the ions Ca^2+(aq) and NO3^-(aq)? A. CaNO3(s) B. Ca2NO3 C. Ca(NO3)2(s) D. Ca2(NO3)3

C. Ca(NO3)2(s)

The particles in a liquid are usually A. Closer together and lower in energy than those in a solid B. Farther apart and higher in energy than those in a gas C. Closer together and lower in energy than those in a gas D. Farther apart and lower in energy than those in a solid

C. Closer together and lower in energy than those in a gas

Which of the following pairs of solutions produces a precipitate when combined? A. Cu(NO3)2 and NaCl B. Fe(NO3)3 and MgCl2 C. Cu(NO3)2 and K2CO3 D. CaCl2 and NaNO3

C. Cu(NO3)2 and K2CO3

A solute crystal is dropped into a solution containing dissolved solute. It falls to the bottom of the beaker and does not dissolve after vigorous stirring. What does this indicate about the solution? A. It is probably unsaturated B. It is probably supersaturated C. It is probably saturated D. It is not at equilibrium

C. It is probably saturated

If the temperature of a fixed quantity of gas decreases and the pressure remains unchanged, A. It's volume increases B. It's volume is unchanged C. It's volume decreases D. It's density decreases

C. It's volume decreases

Which of the following is expressed in grams of solute instead of moles of solute? A. Molality B. Molarity C. Neither A nor B D. Both A and B

C. Neither A nor B

Electrolytes have a greater effect on freezing-point depression than nonelectrolytes because electrolytes A. Have lower freezing points B. Are very volatile C. Produce more moles of solute per mole of solvent D. Are attracted to one another in solution

C. Produce more moles of solute per mole of solvent

Bases feel A. Rough B. Moist C. Slippery D. Dry

C. Slippery

Which if the following is a non-electrolyte? A. Sodium chloride B. Hydrogen chloride C. Sugar D. Potassium chloride

C. Sugar

Which of the following does not increase the rate of dissolving a solid in a water? A. Raising the temperature of the water B. Stirring the solution C. Using larger pieces of solid D. Crushing the solid

C. Using larger pieces of solid

If the temperature remains constant, V and P represents the original volume and pressure, and V' and P' represents the new volume and pressure, what is the mathematical expression for Boyles law? A. P' V = V' P B. V V' = PP' C. VP = V' P' D. V = VP'/P

C. VP= V' P'

What is the freezing-point depression of an aqueous solution of an electrolyte that produces three ions for every formula unit that dissociates if the electrolyte's concentration is 1.25 m? Kf = -1.86°C/m A. -1.25°C B. -1.86°C C. -5.58°C D. -6.98°C

D. -6.98°C

What is the boiling point elevation of a solution made from 10.0 g of a nonelectrolyte solute and 300.0 g of water? the molar mass of the solute is 50.0 g and the molal boiling point constant for water is 0.51°C/m A. 0.01°C B. 0.2°C C. 0.32°C D. 0.34°C

D. 0.34°C

The intermolecular forces between particles are A. Weaker in solids than in liquids B. Stronger in gases than in solids C. Equal in strength in gases and in liquids D. Stronger in liquids than in gases

D. Stronger in liquids than in gases

Glycerol boils at a slightly higher temperature than water. This reveals that glycerol's attractive forces are A. Nonexistent B. Weaker than those of water C. The same as those of water D. Stronger than those of water

D. Stronger than those of water

Two immiscible substances A. Exist together in one phase B. Will not separate on standing C. Dissolve freely in one another in any proportion D. Will not form a solution

D. Will not form a solution