Chem ch 4 & 9 review

In the laboratory, hydrogen gas is usually made by the following reaction: Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq) How many liters of H2 gas, collected over water at an atmospheric pressure of 752 mm Hg and a temperature of 21.0°C, can be made from 4.566 g of Zn and excess HCl? The partial pressure of water vapor is 18.65 mm Hg at 21.0°C

1.75 L

How many grams of XeF6 are required to react with 0.579 L of hydrogen gas at 6.46 atm and 45°C in the reaction shown below? XeF6(s) + 3 H2(g) → Xe(g) + 6 HF(g)

11.7 g

Based on the balanced chemical equation shown below, what volume of 0.250 M K2S2O3(aq), is needed to completely react with 12.4 mL of 0.125 M KI3(aq)? 2 S2O3 2-(aq) + I3 -(aq) → S4O6 2-(aq) + 3 I-(aq)

12.4

Which of the following compounds is not an Arrhenius acid

CH3NH2

In a solution prepared by mixing CH3OH with H2O the major species present are

CH3OH and H2O

Which one of the following compounds behaves as an acid when dissolved in water?

HBr

The mixing of which pair of reactants will result in a precipitation reaction?

K2SO4(aq) + Ba(NO3)2(aq)

Which pair of compounds is soluble in water?

KI and Ba(NO3)2

Which of the following compounds is an Arrhenius base in water?

KOH

Each of three identical 15.0-L gas cylinders contains 7.50 mol of gas at 295 K. Cylinder A contains Ar, cylinder B contains Cl2, and cylinder C contains N2. According to the kinetic molecular theory, which gas has the highest collision frequency?

N2

Which of the following gases has the lowest average speed at 25°C?

NH2NH2

What ion is provided when Arrhenius bases dissolve in water?

OH-

Which one of the following compounds is insoluble in water?

PbCl2

Which of the following compounds is an Arrhenius base?

Sr(OH)2

Some assumptions from the kinetic molecular theory are listed below. Which one is most frequently cited to explain Charles' law?

The average kinetic energy of gas particles is proportional to the Kelvin temperature

The reaction 2 HNO3(aq) + Ba(OH)2(aq) → Ba(NO3)2(aq) + 2 H2O(l) is best classified as a(n)

acid-base neutralization reaction

In the reaction 2 H2O2(l) → 2 H2O(l) + O2(g) oxygen is

both oxidized and reduced.

Which of the following instruments directly measures the pressure of a gas?

manometer

The combustion reaction CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) can be classified as a(n)

oxidation-reduction reaction

The reaction C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(l) is best classified as a(n)

oxidation-reduction reaction

The reaction Cu(s) + 2 AgNO3(aq) → Cu(NO3)2(aq) + 2 Ag(s) is best classified as a(n)

oxidation-reduction reaction

What is the total pressure in a 9.00-L flask which contains 0.127 mol of H2(g) and 0.288 mol of N2(g) at 20.0°C?

1.11 atm

A basketball is inflated to a pressure of 1.50 atm in a 20.0°C garage. What is the pressure of the basketball outside where the temperature is -5.00°C?

1.37 atm

What is the density of oxygen gas at STP?

1.43 g/L

A basketball is inflated to a pressure of 1.70 atm in a 22.0°C garage. What is the pressure of the basketball outside where the temperature is -3.00°C?

1.56 atm

If CO2 and NH3 are allowed to effuse through a porous membrane under identical conditions, the rate of effusion for NH3 will be ________ times that of CO2

1.6

According to the balanced equation shown below, 4.00 mole of oxalic acid, H2C2O4, reacts with ________ moles of permanganate, MnO4 -. 5 H2C2O4(aq) + 2 MnO4 -(aq) + 6 H+(aq) → 10 CO2(g) + Mn2+(aq) + 8 H2O(l)

1.60

What is the density of fluorine gas at STP?

1.70 g/L

A balloon contains 0.76 mol N2, 0.18 mol O2, 0.031 mol He and 0.026 mol H2 at 754 mm Hg. What is the partial pressure of O2?

136 mm Hg

The pressure in the eye of a hurricane is less than atmospheric pressure. Which one of the following pressure readings could not have been taken in the eye of a hurricane?

15 lbs/in2

According to the balanced chemical equation 5 H2C2O4(aq) + 2 MnO4 -(aq) + 6 H+(aq) → 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l) 0.3500 grams of oxalic acid, H2C2O4 will react with ________ mL of 0.100 M potassium permanganate, KMnO4 solution

15.5 mL

A 0.643-g sample of gas occupies 125 mL at 60. cm of Hg and 25°C. What is the molar mass of the gas?

160 g/mol

What is the average speed (actually the root-mean-square speed) of a radon atom at 27°C?

184 m/s

Determine the number of water molecules necessary to balance the reduction half reaction of _____ MnO4 -(aq) → _____ MnO2(s) that occurs in a basic solution.

2

In the unbalanced equation shown below how many moles of electrons are transferred per mole of reducing agent? C2O4 2- (aq) + MnO4 -(aq) → CO2(aq) + Mn2+(aq)

2

What is the oxidation half reaction in the following chemical reaction? Cr2O7 2-(aq) + 6 Cl-(aq) + 14 H+(aq) → 2 Cr3+(aq) + 3 Cl2(aq) + 7 H2O(l)

2 Cl-(aq) → Cl2(aq) + 2e-

Write a balanced net ionic equation for the reaction of H2SO4(aq) with Ba(OH)2(aq)

2 H+(aq) + SO4 2-(aq) + Ba2+(aq) + 2 OH-(aq) → BaSO4(s) + 2 H2O(l)

What are the coefficients in front of Fe(s) and O3(g) when the following equation is balanced in a basic solution? _____ Fe(s) + _____ O3(g) → _____ Fe2O3(s) + _____ O2(g)

2, 3

What are the coefficients in front of NO3 -(aq) and Ni(s) when the following redox equation is balanced in an acidic solution? _____ NO3 -(aq) + _____ Ni(s) → _____ NO(g) + _____ Ni2+(aq)

2, 3

What are the coefficients in front of NO3 -(aq) and Zn(s) when the following equation is balanced in a basic solution? _____ NO3 -(aq) + _____ Zn(s) → _____ Zn2+(aq) + _____ NO(g)

2, 3

What are the coefficients in front of NO3 -(aq) and Cu(s) when the following redox equation is balanced in an acidic solution: _____ NO3 -(aq) + _____ Cu(s) → _____ NO(g) + _____ Cu2+(aq)?

2,3

Automobile tires are typically inflated to about 30 pounds of pressure per square inch. What is the typical air pressure of a tire in kPa?

2.1 × 102 kPa

What is the molar concentration of sodium ions in a 0.750 M Na3PO4 solution

2.25 M

Determine the number of water molecules necessary to balance the reduction half reaction of _____ ClO3 -(aq) → _____ Cl-(aq) that occurs in an acidic solution

3

How many grams of O2 gas are there in a 5.00-L cylinder at 4.00 × 103 mm Hg and 23°C?

34.7 g

Based on the balanced chemical equation shown below, determine the mass percent of Fe3+ in a 0.6450 g sample of iron ore, if 22.40 mL of a 0.1000 M stannous chloride, SnCl2(aq), solution is required to completely react with the Fe3+ present in the ore sample. The chemical equation for the reaction is: 2 Fe3+(aq) + Sn2+(aq) → 2 Fe2+(aq) + Sn4+(aq).

38.79%

Determine the number of water molecules necessary to balance the reduction half reaction of _____ MnO4 -(aq) → _____ Mn2+(aq) that occurs in an acidic solution.

4

A 1.000 kg sample of nitroglycerine, C3H5N3O9, explodes and releases gases with a temperature of 1985°C at 1.400 atm. What is the volume of gas produced? 4 C3H5N3O9(s) → 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g)

4225 L

A 10.0-L flask containing He, 2.00 mole of Ar, and 3.00 mole of Ne has a total pressure of 24.5 atm at 25°C. How many moles of He are in the flask?

5.00 mol

When 15.0 g of zinc metal reacts with excess HCl, how many liters of H2 gas are produced at STP?

5.14 L

A 35.0-L steel tank at 20.0°C contains acetylene gas, C2H2, at a pressure of 1.39 atm. Assuming ideal behavior, how many grams of acetylene are in the tank?

52.7 g

What is the pressure in a gas container that is connected to an open-end U-tube manometer if the pressure of the atmosphere is 722 torr and the level of mercury in the arm connected to the container is 8.60 cm higher than the level of mercury open to the atmosphere?

636 mm Hg

Determine the number of water molecules necessary to balance the following chemical equation. Cr2O7 2-(aq) + Cl-(aq) + H+(aq) → Cr3+(aq) + Cl2(g) + _____ H2O(l)

7

How many molecules of N2 are in a 400.0 mL container at 780 mm Hg and 135°C?

7.38 × 1021 molecules

How many liters of oxygen are needed to exactly react with 27.8 g of methane at STP? CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l)

77.9 L

At STP how many liters of NH3 can be produced from the reaction of 6.00 mol of N2 with 6.00 mol of H2? N2(g) + 3 H2(g) → 2 NH3(g)

89.6 L

Write a balanced net ionic equation for the reaction of AgNO3(aq) with KBr(aq)

Ag+(aq) + Br-(aq) → AgBr(s)

Which elements will not react with liquid water or with aqueous H+ ions?

Ag, Au, Hg, Pt

When Na2CrO4(aq) and AgNO3(aq) are mixed, a red colored precipitate forms which is

Ag2CrO4

Predict the products of a reaction between AgNO3(aq) and KBr(aq

AgBr(s) and KNO3(aq)

What reagent could be used to separate I- from CH3CO2- when added to an aqueous solution containing both?

AgNO3 (aq)

What reagent could not be used to separate Cl- from CO32- when added to an aqueous solution containing both?

AgNO3 (aq)

What reagent could be used to separate Br- from NO3- when added to an aqueous solution containing both?

AgNO3(aq)

What reagent could not be used to separate Cl- from OH- when added to an aqueous solution containing both?

AgNO3(aq)

Which elements will not react with liquid water but will react with aqueous H+ ions?

Al, Cr, Mn, Zn

Three identical flasks contain three different gases at standard temperature and pressure. Flask A contains C2H6, flask B contains O2, and flask C contains NH3. Which flask contains the largest number of molecules

All contain same number of molecules

Three identical flasks contain three different gases at standard temperature and pressure. Flask A contains CH4, flask B contains CO2, flask C contains N2. Which flask contains the largest number of molecules?

All flasks contain the same number of molecule

Each of three identical 15.0-L gas cylinders contains 7.50 mol of gas at 295 K. Cylinder A contains Ar, cylinder B contains Cl2, and cylinder C contains N2. According to the kinetic molecular theory, which gas has the highest average kinetic energy?

All have identical average kinetic energies

Which of the compounds of HCO2H , Ba(OH)2, CsOH, and HBr, behave as bases when they are dissolved in water?

Ba(OH)2 and CsOH

Which elements will react rapidly with aqueous H+ ions and also with liquid H2O?

Ba, Ca, Li, K, Na

Which of the following compounds is not an Arrhenius acid?

C3H7NH2

Write a net ionic equation for the neutralization reaction of CH3CO2H(aq) with CsOH(aq).

CH3CO2H(aq) + OH-(aq) → CH3CO2 -(aq) + H2O(l)

Which one of the following compounds is soluble in water?

Co(NO3)2

Which species functions as the oxidizing agent in the following reduction-oxidation reaction? Zn(s) + Cu2+(aq) → Cu(s) + Zn2+(aq)

Cu2+(aq)

In the reaction AgNO3(aq) + HI(aq) → AgI(s) + HNO3(aq) the spectator ions are

H+ and NO3 -

When dissolved in water, of HClO4, Ca(OH)2, KOH, HI, which are acids?

HClO4 and HI

Using the following portion of the activity series for oxidation half reactions K(s) → K+(aq) + e- Al(s) → Al3+(aq) + 3e- Fe(s) → Fe2+(aq) + 2e- Sn(s) → Sn2+(aq) + 2e- determine which reaction will occur.

K(s) with Sn2+(aq)

Which pair of compounds is soluble in water?

LiI and Ca(NO3)2

In which compound is the oxidation state of hydrogen not +1?

NaH

Which one of the following compounds is soluble in water?

Pb(NO3)2

Which one of the following compounds is insoluble in water?

PbSO4 and Pb3(PO4)2

When dissolved in water, LiOH behaves as

a base that forms Li+ and OH- ions

Which law does the equation, V/n = k represent?

avogadros

What is the oxidation number of the chromium atom in HCr2O4-?

+3

A balloon contains 0.76 mol N2, 0.18 mol O2, 0.031 mol He, and 0.026 mol H2 at 739 mm Hg. What is the partial pressure of O2?

130 mm Hg

How many H+ ions can the acid, H2CO3, donate per molecule?

2

The reaction HNO3(aq) + KOH(aq) → KNO3(aq) + H2O(l) is best classified as a(n)

Acid-Base neutralization reaction

When dissolved in water, of HClO4, Ca(OH)2, KOH, HI, which are bases?

Ca(OH)2 and KOH

Write a balanced net ionic equation for the reaction of CdCl2(aq) with Na2S(aq)

Cd2+(aq) + S2-(aq) → CdS(s

What is the reduction half reaction for the following chemical reaction in a basic solution? ClO-(aq) + Cr(OH)4 -(aq) → CrO4 2-(aq) + Cl-(aq

ClO-(aq) + H2O(l) + 2e- → Cl-(aq) + 2 OH-(aq)

What is the reduction half reaction for the following chemical reaction in a basic solution? Mn2+(aq) + 2 ClO3 -(aq) + OH-(aq) → MnO2(s) + 2 ClO2(aq) + H2O(l)

ClO3 -(aq) + H2O(l) + e- → ClO2(aq) + 2 OH-(aq)

Based on the activity series, which metal dissolves in hydrochloric acid to produce hydrogen gas?

Co

The SI unit for pressure is the

pascal.

Which one of the following is not used to describe the condition of a gas?

polarity

The reaction Pb(NO3)2(aq) + K2SO4(aq) → PbSO4(s) + 2 KNO3(aq) is best classified as a(n)

precipitation reaction

The hydrogen ion, H+, is also referred to as a ________, and a hydrated hydrogen ion, H3O+, is called a ________ ion.

proton, hydronium

When temperature-volume measurements are made on 1.0 mol of gas at 1.0 atm, a plot V versus T results in a

straight line.

HBr, HCl, HClO4, KBr, and NaCl are all classified as

strong electrolytes

HCl, HI, H2SO4, LiCl, and KI are all classified as

strong electrolytes

By analogy with the oxoacids of sulfur, H2TeO3 would be named

tellurous acid.

According to the kinetic molecular theory, the pressure of a gas in a container will decrease if the

temperature of the gas decreases

What is the molar concentration of sulfate ions in a 0.150 M Na2SO4 solution

0.150 M

What is the molarity of a potassium triiodide solution, KI3(aq), if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.600 M thiosulfate solution, K2S2O3(aq)? The chemical equation for the reaction is: 2 S2O3 2-(aq) + I3 -(aq) → S4O6 2-(aq) + 3 I-(aq).

0.250

According to the balanced equation shown below, 1.00 mole of oxalic acid, H2C2O4, reacts with ________ moles of permanganate ion, MnO4 -. 5 H2C2O4(aq) + 2 MnO4 -(aq) + 6 H+(aq) → 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l)

0.400

Based on the balanced chemical equation shown below, determine the molarity of a solution containing Fe2+(aq), if 40.00 mL of the Fe2+(aq) solution is required to completely react with 30.00 mL of a 0.125 M potassium bromate, KBrO3(aq), solution. The chemical equation for the reaction is: 6Fe2+(aq) + BrO3 -(aq) + 6H+(aq) → 6Fe3+(aq) + Br-(aq) + 3H2O(l).

0.563 M

How many H+ ions can the acid CH3CO2H donate per molecule

1

What is the molar concentration of sodium ions in a 0.350 M Na3PO4 solution?

1.05 M in Na

What is the oxidation number of the chromium atom in K2Cr2O7?

+6

What is the oxidation number of the sulfur atom in H2SO4?

+6

What is the oxidation number of the oxygen atom in H2O2?

-1

The volume of 350. mL of gas at 25°C is decreased to 155 mL at constant pressure. What is the final temperature of the gas?

-141°C

The volume of 350. mL of gas at 25°C is decreased to 125 mL at constant pressure. What is the final temperature of the gas?

-167°C

What is the oxidation number change for the chromium atom in the following unbalanced reduction half reaction? Cr2O72-(aq) + H+(aq) → Cr3+(aq) + H2O(l)

-3

What is the oxidation number change for the iron atom in the following reaction? 2 Fe2O3(s) + 3 C(s) → 4 Fe(s) + 3 CO2(g)

-3

What is the oxidation number change for the manganese atom in the following unbalanced reduction half reaction? MnO4 -(aq) + H+(aq) → Mn2+(aq) + H2O(l)

-5

What is the oxidation number of the sulfur atom in S8?

0

According to the balanced chemical equation 5 H2C2O4(aq) + 2 MnO4 -(aq) + 6 H+(aq) → 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l) 0.3500 grams of oxalic acid, H2C2O4 will react with ________ moles of permanganate, MnO4 -.

0.001554

At STP how many grams of Mg are required to produce 35 mL of H2 in the reaction shown below? Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq)

0.038 g

A 5.00-L flask contains nitrogen gas at 25°C and 1.00 atm pressure. What is the final pressure in the flask if an additional 2.00 g of N2 gas is added to the flask and the flask cooled to -55°C?

0.987 atm

Which is the smallest quantity of pressure?

1 pascal

What are the coefficients in front of BrO3 -(aq) and Br-(aq) when the following equation is balanced in an acidic solution? _____ BrO3 -(aq) + _____ Br-(aq) → _____ Br2(aq)

1, 5

Write a net ionic equation for the neutralization reaction of H3PO4(aq) with Ba(OH)2(aq).

2 H3PO4(aq) + 3 Ba2+(aq) + 6 OH-(aq) → Ba3(PO4)2(s) + 6 H2O(l)

An "empty" aerosol can at 25°C still contains gas at 1.00 atmosphere pressure. If an "empty" can is thrown into a 475°C fire, what is the final pressure in the heated can?

2.51 atm

What is the Celsius temperature of 100.0 g of chlorine gas in a 55.0-L container at 800 mm Hg?

228°C

An unknown gas effuses 1.73 times faster than krypton. What is the molar mass of the gas?

28.0 g/mol

How many grams of N2 gas are there in a 5.00-L cylinder at 4.00 × 103 mm Hg and 23°C?

29.9 g

Write a balanced net ionic equation for the reaction of AgNO3(aq) with Cu(s)

2Ag+(aq) + Cu(s) → 2 Ag(s) + Cu2+(aq)

The action of some commercial drain cleaners is based on the following reaction: 2 NaOH(s) + 2 Al(s) + 6 H2O(l) → 2 NaAl(OH)4(s) + 3 H2(g) What is the volume of H2 gas formed at STP when 7.32 g of Al reacts with excess NaOH?

9.12 L

How many molecules of N2 are in a 500.0 mL container at 780 mm Hg and 135°C?

9.23 × 1021

Some assumptions from the kinetic molecular theory are listed below. Which one is most frequently cited to explain diffusion of a gas?

A gas consist of tiny particles moving in random straight line motion.

One mole of which gas has the greatest density at STP?

Ar

"Equal volumes of different gases at the same temperature and pressure contain the same molar amounts" is another way of stating

Avogadro's law.

Predict the products of a reaction between Ba(NO3)2(aq) and K2SO4(aq)

BaSO4(s) and KNO3(aq)

Which species functions as the reducing agent in the following reduction-oxidation reaction? ZnO(s) + C(s) → Zn(s) + CO(g

C(s)

Which of the following gases has the highest average speed at 400K?

CO2

The mixing of which pair of reactants will result in a precipitation reaction?

Cu(NO3)2(aq) + Na2CO3(aq)

Using the following portion of the activity series for oxidation half reactions K(s) → K+(aq) + e- Al(s) → Al3+(aq) + 3e- Fe(s) → Fe2+(aq) + 2e- Sn(s) → Sn2+(aq) + 2e- determine which pairs of reactions will occur.

Fe(s) with Sn2+(aq) and Al(s) with Sn2+(aq)

The chemical formula for sulfurous acid is

H2SO3(aq).

Which of the compounds of H3PO4 , Mg(OH)2, LiOH, and HCl, behave as acids when they are dissolved in water?

H3PO4 and HCl

Write a net ionic equation for the neutralization reaction of HCN(aq) with NaOH(aq).

HCN(aq) + OH-(aq) → CN-(aq) + H2O(l)

Which pair of reactants will produce a precipitate when mixed together?

HCl(aq) and Pb(NO3)2(aq)

The chemical formula for chlorous acid is

HClO2(aq).

Which of the following is not a strong acid?

HF

Which one of the following compounds behaves as an acid when dissolved in water?

HI

The mixing of which pair of reactants will result in a precipitation reaction?

K 2SO4(aq) + Pb(NO3)2(aq)

Coinage metals are metals that are not easily oxidized. Based on the activity series, which metal would be least desirable as a coinage metal?

Mg

The mixing of which pair of reactants will result in a precipitation reaction?

Mg(NO3)2(aq) + Na2CO3(aq)

Using the following portion of the activity series for oxidation half reactions Mg(s) → Mg2+(aq) + 2e- Zn(s) → Zn2+(aq) + 2e- Cu(s) â→ Cu2+(aq) + 2e- indicate which pairs of reactions will occur.

Mg(s) with Zn2+(aq) and Zn(s) with Cu2+(aq)

Which species functions as the oxidizing agent in the following reduction-oxidation reaction? 5 Fe2+(aq) + MnO4 -(aq) + 8 H+(aq) → Mn2+(aq) + 5 Fe3+(aq) + 4 H2O(l)

MnO4 -(aq)

An unknown gas effuses 2.3 times faster than N2O4 at the same temperature. What is the identity of the unknown gas?

NH3

Which of the following compounds is an Arrhenius base in water?

NH3

Using the following portion of the activity series for oxidation half reactions, determine which combination of reactants will result in a reaction. Na(s) → Na+(aq) + e- Cr(s) → Cr3+(aq) + 3e-

Na(s) with Cr3+(aq)

Using the following portion of the activity series for oxidation half-reactions, determine which combination of reactants will result in a reaction. Na(s) → Na+(aq) + e- Cr(s) → Cr3+(aq) + 3e-

Na(s) with Cr3+(aq)

Write a balanced net ionic equation for the reaction of Na2CO3(s) and HCl(aq)

Na2CO3(s) + 2 H+(aq) → 2 Na+(aq) + H2O(l) + CO2(g)

In which compound is the oxidation state of oxygen not -2?

Na2O2

What reagent would distinguish between Ba2+ and Pb2+?

NaCl

What reagent would distinguish between Ag+ and Fe3+?

NaI

What is true when the following equation is balanced in basic solution? P(s) + PO4 3-(aq) → HPO3 2-(aq)

OH- appears on the left side of the equation

Which species functions as the reducing agent in the following reduction-oxidation reaction? 2 P(s) + 3 Br2(l) → 2 PBr3(l)

P(s)

Which of the following equations represents "Boyle's law"?

PV = k

Write a balanced net ionic equation for the reaction of Pb(NO3)2(aq) with NaI(aq)

Pb2+(aq) + 2 I-(aq) → PbI2(s)

When K2SO4(aq) and Pb(NO3)2(aq) are mixed, a white colored precipitate forms which is

PbSO4

Which one of the following compounds is insoluble in water?

PbSO4

Some assumptions from the kinetic molecular theory are listed below. Which one is most frequently cited to explain compressibility of a gas?

The volume of the particles is negligible compared to the volume of the gas.

Using the following portion of the activity series for oxidation half reactions Ca(s) → Ca2+(aq) + 2e- Mg(s) → Mg2+(aq) + 2e- Zn(s) → Zn2+(aq) + 2e- Cu(s) → Cu2+(aq) + 2e- determine which reaction will not occur.

Zn(s) with Mg2+(aq)

What is the oxidation half reaction in the following chemical reaction? Zn(s) + 2 H+(aq) → Zn2+(aq) + H2(g)

Zn(s) → Zn2+(aq) + 2e

The mixing of different gases by random molecular motion with frequent collisions is called

diffusion

Pressure is defined as

force divided by unit area.

An aqueous solution of HI is named

hydriodic acid

An aqueous solution of H2S is named

hydrosulfuric acid.

Water (H2O), methyl alcohol (CH3OH), ethyl alcohol (CH3CH2OH), ethylene glycol (HOCH2CH2OH), and sucrose (C12H22O11) are commonly classified as

nonelectrolytes

Acetic acid (CH3CO2H), formic acid (HCO2H), hydrofluoric acid (HF), ammonia (NH3), and methylamine (CH3NH2) are commonly classified as

weak electrolytes