me right answer - Test - 3 In the following reaction, when the equation is correctly balanced, what is the correct coefficient for aluminum chloride?...
Question

1. In the following reaction, when the equation is correctly balanced, what is the correct coefficient for aluminum chloride?

Al( s) + Cl 2g) → AlCl 3s

• 1
• 2
• 3
• 4
• 5

2.In the kinetic molecular theory of gas behavior, the assumption is made that gas molecules

• are attracted to each other by strong forces.
• move with a kinetic energy equal to their centigrade temperature.
• move rapidly in random directions.
• occasionally come to rest.
• are close together in their container.

3.When 3.05 moles of CH 4 are mixed with 5.03 moles of O 2 the limiting reactant is __________.

CH 4 + 2O 2 → CO 2 + 2H 2

• CO2
• O2
• H2O
• CH4

4.The unit of 1 atmosphere used to describe the pressure of a gas is equal to

• 100 mmHg.
• 600 mmHg.
• 1 mmHg .
• 200 mmHg.
• 760 mmHg.

5.In a solution, the solvent

• is the substance present in the smallest concentration.
• can be a solid,
• liquid, or gas.
• is never a solid.is a liquid.
• can be a liquid or gas.

6.The volume of a gas with a pressure of 1.2 atm increases from 1.0 L to 4.0 L. What is the final pressure of the gas, assuming constant temperature?

• 1.2 atm
• 1.0 atm
• 4.8 atm
• 0.30 atm
• 3.3 atm

7.What is the coefficient of hydrogen, H 2, when the following equation is balanced?

Al + H 2SO 4 → Al 2(SO 4)  3 + ? H 2

• 1
• 2
• 3
• 4
• 5

8.An increase in the temperature of a solution usually

• decreases the solubility of a liquid solute in the solution.
• decreases the solubility of a solid solute in the solution.
• increases the solubility of a gas in the solution.
• increases the solubility of a solid solute in the solution.
• increases the boiling point.

9.At STP, what is the volume of 4.50 moles of nitrogen gas?

• 167 L
• 3420 L
• 1230 L
• 101 L
• 60.7 L

10.A 5.00-L tank contains helium gas at 1.50 atm. What is the pressure of the gas in mmHg?

• 7.5 mmHg
• 1140 mmHg
• 507 mmHg
• 1.50 mmHg
• 760 mmHg

11.What is the concentration, in mass percent, of a solution prepared from 50.0 g NaCl and 150.0 g of water?

• 40.0%
• 3.00%
• 33.3%
• 25.0%
• 0.250%

12.What is the molar mass of sodium phosphate, Na 3PO 4?

• 119.0 g
• 354.0 g
• 226.0 g
• 308.0 g
• 164.0 g

13.For the question(s) that follow, consider the following balanced equation.

Mg 32s) + 6H 2O( l) → 3Mg(OH) 2s) + 2NH 3g

What is the correct form of the conversion factor needed to convert the number of moles of H 2O to the number of moles of NH3 produced?

ans-

14.How many moles of water, H 2O, are present in 75.0 g of H 2O?

• 7.50 moles
• 4.41 moles
• 75.0 moles
• 4.17 moles
• 1.35 × 103 moles

15.Avogadro's number is the number of

• grams in 1 mole of a substance.
• amu in 1 mole of a substance.
• particles in 1 mole of a substance.
• moles in 6.02 × 1023 grams of an element.
• moles in 6.02 × 1023 amu of an element.

16.According to the kinetic-molecular theory, gas molecules have

• little distance between molecules.
• weak interactions between molecules.
• less energy than molecules of a solid.
• strong interactions between molecules.

17.A balloon is filled with helium gas. For the question(s) that follow, select the letter of the balloon diagram that corresponds to the given change in conditions.

The temperature is changed from 50 °C to -150 °C at constant pressure.

• A
• B
• C
• A and B
• B and C

18.The molarity (M) of a solution refers to

• moles of solute/100 mL of solution.
• grams of solute/L of solution.
• moles of solute/L of solvent.
• grams of solute/100 mL of solution.
• moles of solute/L of solution.

19.The molar mass of potassium is

• 39.1 g.
• 6.02 × 1023 grams.
• 15g.
• 31.0 g.
• 19 g.

20.What unit of temperature is used in gas law calculations?

• either degrees Celsius or degrees Fahrenheit
• degrees Celsius
• Kelvin
• degrees Fahrenheit
• either degrees Celsius or Kelvin

21.For a given amount of gas at a constant temperature, the volume of gas varies inversely with its pressure is a statement of ________ law.

• Charles's
• Boyle's
• Curie's

22.What is the molarity of a solution that contains 3.25 moles of NaNO 3 in 250. mL of solution?

• 0.0130 M
• 6.50 M
• 3.25 M
• 13.0 M
• 2.60 M

23.When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the solution is

• unsaturated.
• polar.
• dilute.
• saturated.
• nonpolar.

24.At STP, temperature and pressure have the values of

• 273 K and 1 mmHg.
• 0 K and 1 atm.
• 0 K and 760 mmHg.
• 760 K and 273 atm.
• 273 K and 760 mmHg.

25.In any balanced chemical equation, the number of each type of atom on both sides of the equation is

• decreased by one.
• dependent on the temperature.
• doubled.
• increased by one.
• the same.

26.What is the molarity of a KCl solution made by diluting 75.0 mL of a 0.200 M solution to a final volume of 100. mL?

• 0.267 M
• 0.200 M
• 0.100 M
• 0.150 M
• 6.67 M

27.In an oxidation-reduction reaction, the substance oxidized always

• shows a loss of electrons.
• shows a gain of electrons.
• gives up hydrogen atoms.
• takes on oxygen atoms.
• becomes a charged species.

28.Complete the following statement: In Charles's Law, the volume of a gas __________ when the __________ decreases.

• increases; quantity of gas
• increases; temperature
• decreases; temperature
• increases; pressure
• decreases; pressure

29.The mass percent concentration refers to

• grams of solvent in 100 g of solution.
• grams of solute in 1 kg of solution.
• grams of solute in 100 g of solution.
• grams of solute in 1 kg of solvent.
• grams of solute in 100 g of solvent.

30.Oil does not dissolve in water because

• water is saturated.
• water is nonpolar.
• oil is hydrated.
• oil is polar.
• oil is nonpolar.

31.What is the classification for this reaction?

SO 3 ( g) + H 2O ( l) → H 2SO 4l

• replacement
• combination
• decomposition
• oxidation reduction
• double replacement

32.In water, a substance that ionizes completely in solution is called a

• semiconductor.
• nonelectrolyte.
• weak electrolyte.
• nonconductor.
• strong electrolyte.

33.What is the classification for this unbalanced reaction?

Fe + HCl → FeCl 3 + H 2

• combination
• decomposition
• single replacement
• dehydration
• double replacement

Home work -4

1. What is the [OH -] in a solution that has a [H 3+] = 2.0 × 10 -4 M?
• 5.0 × 10-11 M
• 2.0 × 10-4 M
• 2.0 × 10-10 M
• 5.0 × 10-10 M
• 1.0 × 10-10 M

2.The name of Al(OH) 3 is

• aluminum(III) hydroxide.
• aluminum trihydroxide.
• aluminum hydroxide.
• monoaluminum trihydroxide.
• aluminum oxygen hydride.

3.In a neutralization reaction

• an acid and a salt react to form water and a base.
• an acid and a base react to form a salt and water.
• a base and a salt react to form water and an acid.
• water and a salt react to form an acid and a base.
• two acids react to form water.

4.In any chemical reaction, the rate of the reaction can be increased by

• adding product molecules to the reaction mixture.
• increasing the concentrations of the reactants.
• decreasing the temperature.
• changing the size of the container.
• adding water to the reaction.

5.Ammonium hydroxide is a weak base because

• it is only slightly soluble in water.
• it cannot hold on to its hydroxide ions.
• it is completely ionized in aqueous solution.
• it dissociates only slightly in water.
• it is a dilute solution.

6.The name given to an aqueous solution of HNO  is

• hydrogen nitrate.
• hyponitric acid.
• hydronitrogen acid.
• nitrous acid.
• nitric acid.

7.What is the name of  CH3

CH3 -CH-CH2-CH2-CH3 ?

• 2-methylpentane
• hexane
• 4-methylpentane
• pentane
• methylpentane

8.In the three-dimensional structure of methane, CH 4, the hydrogen atoms attached to a carbon atom are aligned

• at the corners of a tetrahedron.
• in a straight line.
• at the corners of a cube.
• at the corners of a square.
• at the corners of a rectangle.

9.Organic chemistry is the study of the chemistry of compounds of

• carbon.
• oxygen.
• polymers.
• living things.
• hydrogen.

10.The activation energy of a chemical reaction is the energy that

• must be released from the mixture.
• activates the catalyst.
• is the difference in the energies of the starting materials and products.
• must be removed from the mixture.
• initiates the reaction.

11.What is the pH of a solution with [H 3+] = 1 × 10 -9 M?

• -0.9
• 9.0
• -5.0
• 1.0 × 10-5 M
• 5.0

12.Which of the following statements correctly describes the hydronium-hydroxide balance in the given solution?

• In bases, [OH-] is greater than [H3O+].
• In bases, [OH-] = [H3O+].
• In acids, [OH-] is greater than [H3O+].
• In bases, [OH-] is less than [H3O+].
• In neutral solutions, [H3O+] = [H2O].

13.A formula that shows the arrangement of all bonds in a molecule is called a(n)

• complete structural formula.
• isomeric formula.
• condensed structural formula.
• condensed molecular formula.
• molecular formula.

14.For the following equilibrium reaction, which cause and effect are correctly matched?

CO( g) + 2H 2g) ⇌ CH 3OH( g) + heat

• remove heat, no change
• remove CH3OH,
• shift rightremove H2,
• shift left

15.Which one of the following is NOT an organic substance?

• nylon
• salt, sodium
• chloridecoalan
• antibiotic
• silk

16.An organic compound composed of carbon and hydrogen connected only by single bonds is an

• alkyne.
• alkane.
• aromatic compound.
• alcohol.
• alkene.

17.An acid and base react to form a salt and water in a(n) __________ reaction.

• neutralization
• oxidation
• ionization
• reduction
• dissociation

18.The simplest cycloalkane has

• five carbon atoms.
• one carbon atom.
• four carbon atoms
• three carbon atoms.
• two carbon atoms.

19.What is the IUPAC name of What is the IUPAC name of  ?

• 3-methyl-1,2-dichlorocyclopentane
• 1-methyl-2,3-dichlorocyclopentane1,
• 2-dichloro-3-methylcyclopentane1,
• 2-dichloro-3-methylpentane1,
• 2-dichloro-3-methylcyclobutane

20.The equilibrium constant for the production of carbon dioxide from carbon monoxide and oxygen is  KC=2 x 10(11) to the power . This means that the reaction mixture at equilibrium is likely to consist of

• an equal mixture of products and reactants.
• twice as much product as starting material.
• mostly starting materials.t
• wice as much starting material as product.
• mostly products.

21.In the following gas phase reaction, what is the effect on the direction of the reaction if more SO 3 is added to the reaction mixture?

2SO 2g) + O 2g) ⇌ 2SO 3g

• The equilibrium shifts to produce more reactants.
• The catalyst for the reaction is used up.
• The position of the equilibrium remains unchanged.
• The equilibrium shifts to produce more products.
• The rate of formation of products is increased.

22.What is the correct form of the equilibrium constant for the reaction of hydrogen and oxygen to form water? The equation is:

2H 2g) + O 2g) ⇌ H 2O( g

Ans-

23.Which of the following is correctly identified?

• NaOH, strong base
• HCl, weak acid
• NH3, strong acid
• H2CO3, strong acid
• Ca(OH)2, weak base

24.The reaction for the decomposition of PCl 5 to chlorine and PCl 3 is shown below.

PCl 5g) ⇌ PCl 3g) + Cl 2g

If the equilibrium concentrations are [PCl 5] = 1.0 M, [PCl 3] = 0.10 M, [Cl 2] = 0.10 M, what is the value of the equilibrium constant?

• 1.0 × 102
• 2.0 × 10-2
• 10 × 10-2
• 1.0 × 10-2
• 1.0 × 10-4

25.What is the condensed structural formula for an alkane with four carbon atoms?

• C - C - C - C

H H H H

• H ----- H
• CH3-CH2-CH2-CH3
• CH3-CH=CH-CH3
• C4H10

26.What is the name for a five-carbon continuous-chain alkane?

• ethane
• butane
• propane
• pentane
• methane

27.A chemical reaction has reached equilibrium when

• all reactants have been converted to products.
• the catalyst has been used up.
• the concentrations of reactants and products are equal.
• the rate of the forward reaction equals the rate of the reverse reaction.

28.According to the Arrhenius concept, if NaOH were dissolved in water, it would act as

• a base.
• an acid.
• a source of hydronium ions.
• a source of H- ions.
• a proton donor.

29.In which of the following are the pH values arranged from the most basic to the most acidic?

• 2, 5, 7, 9, 10, 11
• 7, 10, 14, 4, 3, 1
• 14, 10, 7, 4, 3, 1
• 14, 10, 7, 1, 3, 5
• 1, 3, 6, 8, 11, 14

30.What is the name of this compound?

CH 3- CH 2- CH 2- CH 2- CH 2- CH 2- CH 3

• heptane
• hexane
• pentane
• butane
• octane

31.A catalyst is

• a substance that decreases the energy of the products.
• a substance that increases the energy of the products.
• a substance that speeds up a reaction without being consumed in the reaction.
• a product in a chemical reaction.
• a reactant in a chemical reaction.

32.According to the Bronsted-Lowry definition,

• a base is a proton donor.
• a base produces H+ ions in aqueous solutions.
• a base is a proton acceptor.
• an acid is a proton acceptor.
• an acid acts as the solvent.

33.A reaction that can proceed in either the forward or the reverse direction as written is called a __________ reaction.

• reversible
• favored
• microscopic
• miniscule
• solid phase

Test 4

1.The equilibrium constant for the production of carbon dioxide from carbon monoxide and oxygen is

Kc = 2 × 10 11. This means that the reaction mixture at equilibrium is likely to consist of

• twice as much product as starting material.
• twice as much starting material as product.
• an equal mixture of products and reactants.
• mostly products.
• mostly starting materials.

2.Which of the following is correctly identified?

• NaOH, strong base
• Ca(OH)2, weak base
• H2CO3, strong acid
• HCl, weak acidNH3,
• strong acid

3.The activation energy of a chemical reaction is the energy that

• activates the catalyst.
• initiates the reaction.
• is the difference in the energies of the starting materials and products.
• must be released from the mixture.
• must be removed from the mixture.

4.In the three-dimensional structure of methane, CH 4, the hydrogen atoms attached to a carbon atom are aligned

• at the corners of a tetrahedron.
• at the corners of a cube.
• at the corners of a square.
• in a straight line.
• at the corners of a rectangle.

5.What is the pH of a solution with [ H 3+] = 1 × 10 -9 M?

• 1.0 × 10-5 M
• 9.0
• -5.0
• 5.0
• -9.0

6.The equilibrium for the reaction for the decomposition of PCl 5 to chlorine and PCl 3 is 0.042.

PCl 5g) ⇌ PCl 3g)+ Cl 2g

If the equilibrium concentrations are [PCl 3] = 0.010 M, [Cl 2] = 0.10 M, what is the value of [PCl 5]?

• 0.010 M
• 0.0020 M
• 0.0010 M
• 0.042 M
• 0.024 M

7.According to the Brønsted-Lowry definition,

• a base is a proton donor.
• a base is a proton acceptor.
• an acid is a proton acceptor.
• a base produces H+ ions in aqueous solutions.
• an acid acts as the solvent.

8.What is the molarity of a KOH solution if 25.0 mL neutralizes 35.0 mL of a 0.200 M HCl solution?

• 0.200 M
• 0.100 M
• 0.280 M
• 0.267 M
• 0.143 M

9.For the following equilibrium reaction, which cause and effect are correctly matched?

CO( g) + 2H 2g) ⇌ CH 3OH( g) + heat

• remove heat, no change
• remove CH3OH, shift left
• remove H2, shift left

10.The bond angles of tetravalent carbon are all approximately

• 90°.
• 60°.
• 109°
• 100°
• 45°.

11.An acid and base react to form a salt and water in a(n) ________ reaction.

• reduction
• oxidation
• ionization
• neutralization
• dissociation

12.In the following gas phase reaction, what is the effect of adding more NO 2 to the starting reaction mixture?

2NO 2g) ⇌ N 24g

• It would make the reaction more endothermic.
• It would slow the reaction down.
• It would increase the final quantity of products.
• It would make the reaction more exothermic.
• It would decrease the final quantity of products.

13.What is the correct form for the equilibrium constant expression for this reaction?

H 2g) + F 2g) ⇌ 2HF( g

Ans-

14.Which of the following statements correctly describes the hydronium-hydroxide balance in the given solution?

• In neutral solutions, [ H3O+] = [ H2O].
• In bases, [OH-] is less than [ H3O+].
• In bases, [OH-] = [ H3O+].
• In acids, [OH-] is greater than [ H3O+].
• In bases, [OH-] is greater than [ H3O+].

15.25.0 mL of 0.212 M NaOH is neutralized by 13.6 mL of an HCl solution. The molarity of the HCl solution is

• 0.115 M
• .0.137 M
• .0.390 M.
• 0.212 M
• .0.500 M.

16.In which of the following are the pH values arranged from the most basic to the most acidic?

• 1, 3, 6, 8, 11, 14
• 2, 5, 7, 9, 10, 11
• 14, 10, 7, 1, 3, 5
• 14, 10, 7, 4, 3, 1
• 7, 10, 14, 4, 3, 1

17.For the following reaction, the equilibrium concentration of NO 2 is 0.38 M and equilibrium concentration of N 2is 1.0M. What is the value of the equilibrium constant?

2NO 2g) ⇌ N 24g

• 0.14
• 1.0
• 0.38
• 6.9
• 2.6

18.Identify the Brønsted-Lowry acids in the following reaction.

2O + CO 3 2- → HCO 3 - + OH -

• CO32-/HCO3-
• OH-/HCO3-
• H2CO3/H2O
• H2O/HCO3-
• CO32-/OH-

19.What is the name for a nine-carbon continuous-chain alkane?

• hexane
• heptane
• octane
• nonane
• decane

20.What is the IUPAC name for the following?

CH 3

∣

CH 3-CH 2-CH 2-CH- CH 2-CH 3

• methylhexane
• 4-methylhexane
• heptane
• 2-methylhexane
• 3-methylhexane

21.Which of the following is the correctly balanced equation for the complete neutralization of H 3PO 4 with Ca(OH) 2?

• H3PO4 + Ca(OH)2 → Ca3(PO4)2+ H2O
• 2H3PO4 + 3Ca(OH)2 → Ca3(PO4)2 + 6H2O
• 3H3PO4 + Ca(OH)2 → Ca3(PO4)2 + 5H2O
• H3PO4 + Ca(OH)2 → CaHPO4 + 2H2O
• 4H3PO4 + 6Ca(OH)2 → 2Ca3(PO4)2 + 12H2O

22.A solution with a pH of 4 is

• neutral.
• extremely acidic.
• moderately acidic.
• slightly basic.
• extremely basic.

23.Which of the following is a neutralization reaction?

• KCl + NaNO3→ KNO3 + NaCl
• 4Na + O2 → 2Na2O
• 2NO2 → 2NO + O2
• HNO3+ KOH → H2O + KNO3
• H2O + SO3 → H2SO4

24.An organic compound composed of carbon and hydrogen connected only by single bonds is an

• alkane.
• aromatic compound.
• alkene.
• alkyne.
• alcohol.

25.A solution which has [OH -] = 4.6 × 10 -6 M is

• acidic.
• basic.
• neutral.

26.In a condensed structural formula, each carbon atom is

• written in lowercase letters.
• shown with only the other carbon atoms.
• shown with all individual atoms and bonds drawn.
• not explicitly shown.
• grouped with its bonded hydrogen atoms.

27.For the following reaction, the equilibrium constant  Kis 0.60 at a certain temperature. If the concentration of NO( g) and NOBr( g) are both 0.50 M,at equilibrium, what is the concentration of Br 2g)?

2NO( g) + Br 2g) ⇌ 2NOBr( g

• 2.8 M
• 0.36 M
• 0.60 M
• 1.0 M
• 1.7 M

28.What is the condensed structural formula for an alkane with four carbon atoms?

• CH3-CH=CH-CH3
• C4H10

H H H H

| | | |

• H - C - C - C - C - H

| | | |

H H H H

• CH3-CH2-CH2-CH3
• C - C - C - C

29.What is the IUPAC name for Cl-CH -CH 2 - CH 2-Cl?

• 1,1-dichloropropane
• dichloropropane
• 1,3-dichloropropane
• propane dichloride
• 1,3-dichlorobutane

30.Carbon atoms always have how many covalent bonds?

• one
• two
• three
• four
• five

31.In the following gas phase reaction, what is the effect on the direction of the reaction if more SO 3 is added to the reaction mixture?

2SO 2g) + O 2g) ⇌ 2SO 3g

• The position of the equilibrium remains unchanged.
• The catalyst for the reaction is used up.
• The equilibrium shifts to produce more products.
• The equilibrium shifts to produce more reactants.
• The rate of formation of products is increased.

32.The equation for the formation of ammonia from nitrogen and hydrogen is shown below. What is the form of the equilibrium constant?

3H 2g) + N 2g) ⇌ 2NH 3g

Ans-

33.What is the IUPAC name for the following?

CH 3

∣

CH 3-CH 2-CH 2-CH- CH 2-CH 3

• methylhexane
• 4-methylhexane
• heptane
• 2-methylhexane
• 3-methylhexane

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