How many hydrogen atoms are contained in a molecular

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Reference no: EM131061613

General Chemistry Lec II

Problem 1

All of the following are clues that a chemical reaction has taken place except

The reactant is smaller.

a.A flame occurs.

b.A color change occurs.

c. A solid forms.

Problem 2

Balance the following equation in standard form and determine the sum of the coefficients.

a.6

b.4

c.3

d.14

e.7

Problem 3

Balance this equation using the smallest possible integers, S + HNO3→ H2SO4 + NO2 + H2O. What is the coefficient of water.

a.2

b.6

c.8

d. 1

Problem 4

When the following equation is balanced using the smallest possible integers, what is the coefficient of oxygen gas?

C7H16(g) + O2(g) → CO2(g) + H2O(g)

a.5   

b.11

c.2

d.14

e.8

Problem 5

True or false? The equation N2 + 3H2→ 2NH3 means that 1 g of N2 reacts with 3 g of H2 to form 2 g of NH3.

Problem 6

Which of the following statements is not true of balancing a chemical equation?

a.Subscripts in the reactants must be conserved in the products.

b.The law of conservation of matter must be followed.

c.Phases are often shown for each compound but are not critical to balancing an equation.

d.All of the above statements (a-d) are true.

e.Coefficients are used to balance the atoms on both sides.

Problem 7

CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)

a.oxidation-reduction

b.two of these

c.synthesis

d. decomposition

e.combustion

Problem 8

Classify the following reaction:

2Mg(s) + O2(g) → 2MgO(s)

a.synthesis

b.oxidation-reduction

c. a-c are all correct.

d.combustion

e.two of the above

Problem 9

The equation 2Ag2O(s) → 4Ag(s) + O2(g) is a(n) ______________ reaction.

a.synthesis

b.two of these

c. oxidation-reduction

d.decomposition

e.combustion

Problem 10

The reaction 2K(s) + Br2(l) → 2KBr(s) is a(n) ______________ reaction.

a.acid-base

b.oxidation-reduction

c.precipitation

d. single-replacement

e.double-displacement

Problem 11

When the following equation is balanced in standard form, what is the coefficient in front of the H2O?

C8H18(g) + O2(g) CO2(g) + H2O(g)

a.8

b.18

c.16

d.25

e.1

Problem 12

Which of the following is a strong acid?

a.phosphoric acid

b.acetic acid

c.hydrofluoric acid

d.lactic acid

e.hydrochloric acid

Problem 13

Which of the following statements is not true?

a.Two nonmetals can undergo an oxidation-reduction reaction.

b.A metal-nonmetal reaction involves electron transfer.

c.When two nonmetals react, the compound formed is ionic.

d.A metal-nonmetal reaction can always be assumed to be an oxidation-reduction reaction.

e.When a metal reacts with a nonmetal, an ionic compound is formed.

Problem 14

17.7 g of Mg represents how many moles?

a.none of these

b.1.37 mol

c.42.0 mol

d.4.30 × 102 mol

e.0.728 mol

Problem 15

21.2 g of oxygen contains

a.none of the above

b.1.28 × 1025 oxygen molecules

c.7.98 × 1023 oxygen atoms

d.42 amu

e.1.33 mol of oxygen molecules

Problem 16

45 atoms of calcium weigh

a.1.804 × 103 g

b.900 amu

c.900 g

d.1.804 × 103 amu

e.2.71 × 1025 amu

Problem 17

8.55 x 10-3 moles of an unknown compound has a mass of 0.257 g. The compound could be:

a.C5H12

b.CH4

c.C3H8

d.C2H6

e.C4H10

Problem 18

A 1.73-mole sample of H2O2 weighs

a. 31.2 amu

b. 31.2 g

c. 1.73 g

d. 58.8 g

e 35.7 g

Problem 19

A certain compound has an empirical formula of NH2O. Its molar mass is between 55 and 65 g/mol. Its molecular formula is

a N2H4O2

b N2H2O2

c NH2O

d not calculable

Problem 20

A certain compound is found to have the percent composition (by mass) of 85.63% C and 14.37% H. The molecular formula contains 3 carbon atoms. How many hydrogen atoms are contained in a molecular of this compound?

A 8

b3

c 2

d 4

 e 6

Problem 21

A compound is composed of element X and hydrogen. Analysis shows the compound to be 80% X by mass, with three times as many hydrogen atoms as X atoms per molecule. Which element is element X?

A F

b none of these

c He

d S

e C

Problem 22

Calculate the mass of 5.333 moles of silver nitrate.

a.none of these

b.906.1 g

c.820.8 g

d.31.9 g

e.3.139 × 10-2 g

Problem 23

Convert: 3.577 mol K2O = _____________ g K2O

a.26.33

b 3.577

 c.337.0

d 3.797 × 10-2

e 2.154 × 1024

Problem 24

Convert: 9.41 mol Cu(NO3)2 = ____________ g Cu(NO3)2

a. none of these

b 1.77 × 103

c 1.61 × 103

d 5.02 × 10-2

e 19.9

Problem 25

Determine the percentage composition (by mass) of tin in SnCl2.

a.62.6 %

b.77.0 %

c 38.5 %

d 61.5 %

e 18.7 %

Problem 26

The empirical formula of styrene is CH; its molar mass is 104.1 g/mol. What is the molecular formula of styrene?

a.C8H8

b.C2H4

c C6H6

d C10H12

Problem 27

What is the molar mass of Li3PO4?

a 83.79 g/mol

b 115.79 g/mol

c 108.85 g/mol

d 6.02 × 1023 g/mol

e 84.82 g/mol

Problem 28

Which represents the greatest mass?

a.1.0 mol P

b.1.0 mol K

c. all the same

d.1.0 mol Al

e.1.0 mol I

Problem 29

True or false? One atomic mass unit (amu) is the mass (in grams) of one mole of the substance.

Problem 30

True or false? The empirical formula and the molecular formula for a compound cannot be the same.

Problem 31

True or false? The mole can be defined as the number equal to the number of oxygen atoms in 32.00 g of oxygen.

Problem 32

An excess of Al and 9.7 mol of Br2 are reacted according to the equation

How many moles of AlBr3 will be formed assuming 100% yield?

a.4.9 mol

b.6.5 mol

c.9.7 mol

d.14.6 mol

e.3.2 mol

Problem 33

Calculate the mass of water produced when 6.25 g of methane, CH4, reacts with an excess of oxygen in the following unbalanced reaction.

a. 7.02 g H2O

b 0.78 g H2O

c. 14.0 g H2O

d.2.25 × 102 g H2O

e.0.347 g H2O

Problem 34

Consider the equation: . The molar mass of B is 50.0 g/mol. Which of the following statements is true when equal masses of A and B are reacted?

a.If the molar mass of A is less than the molar mass of B, then B must determine how much C is produced.

b. If the molar mass of A is greater than the molar mass of B, then B must determine how much C is produced.

c.If the molar mass of A is greater than the molar mass of B, then A must determine how much C is produced.

d.If the molar mass of A is less than the molar mass of B, then A must determine how much C is produced.

e If the molar mass of A is the same as the molar mass of B, then A and B react in a perfect stoichiometric ratio and both determine how much C is produced.

Problem 35

Consider the following unbalanced equation: 

How many moles of water are needed to react with 232. g of Al4C3?

a.0.620 mol

b.0.134 mol

c 19.3 mol

d 1.61 mol

e 348. mol

Problem 36

Tin(II) fluoride is added to some dental products to help prevent cavities. Manufacturers have to make the tin(II) fluoride first, though, before they can add it to their products.

How many grams of tin(II) fluoride can be made from 58.0 g of hydrogen fluoride if there is plenty of tin available to react?

a. 908. g

B 227. g

c 116. g

d 454. g

e 1.45 g

Problem 37

What mass of carbon dioxide will be produced when 12.9 g of butane reacts with an excess of oxygen in the following reaction?

a. none of these

b 39.1 g CO2

c 4.88 g CO2

d 78.1 g CO2

e 51.6 g CO2

Problem 38

True or false? A balanced chemical equation is one that has the same number of moles of molecules on each side of the equation.

Problem 39

True or false? A mole ratio is used to convert the moles of a starting substance to the moles of a desired substance.

Problem 40

True or false? The equation can be interpreted by saying that 1 mol of N2 reacts with 3 mol of H2 to form 2 mol of NH3.

Problem 41

A hydrogen balloon is at 25oC, 1.00 atm and has a volume of 1.00 L. How many grams of argon gas must be added to the hydrogen balloon to achieve a volume of 3.84 L at constant temperature and pressure?

a 4.64 g

b 93.9 g

c none of these

d 6.27 g

e 7.91 g

Problem 42

A sample of an ideal gas containing 0.918 mol is collected at 742 torr pressure and 31°C. Calculate the volume.

aL

b 23.5 L

cL

d none of these

e 2.39 L

Problem 43

A sample of oxygen gas (O2) has a volume of 7.86 L at a temperature of 19oC and a pressure of 1.38 atm. Calculate the moles of O2 molecules present in this gas sample.

A none of these

B 0.226 mol

C 6.96 mol

D 0.905 mol

E 0.453 mol

Problem 44

An oxygen sample has a volume of 9.77 L at 27°C and 800.0 torr. How many oxygen molecules does it contain?

Problem 45

Avogadro's law states that:

a The volume of a fixed amount of gas is indirectly proportional to its temperature in Kelvin at constant pressure.

b The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.

c The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.

d Equal amounts of gases occupy the same volume at constant temperature and pressure.

e The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.

Problem 46

Boyle's law states that:

a Equal amounts of gases occupy the same volume at constant temperature and pressure.

b The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.

c The volume of a fixed amount of gas is proportional to its pressure at constant temperature.

d The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.

e The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.

Problem 47

Charles's law states that:

a.The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.

b. The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.

C The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.

D The volume of a fixed amount of gas is indirectly proportional to its temperature in Kelvin at constant pressure.

E Equal amounts of gases occupy the same volume at constant temperature and pressure.

Problem 48

A solution has [H+] = 4.7 × 10-8M. The pH of this solution is

a.9.80

b.7.33

c.6.01

d. none of these

e.6.67

Problem 49

A solution has a pH of 3.66. The pOH of this solution is

a.10.34

b.none of these

c.10.24

d.3.76

e. 3.66

Problem 50

A solution where [H+] = 10-13M is ______________.

Select one:

A acidic

B basic

C strongly acidic

d.neutral

e.two of these

Problem 51

Calculate the [H+] in a solution that has a pH of 2.39.

aM

b none of these

c 11.61 M

d 2.39 M

eM

Problem 52

What is the pH of a 3.6 M solution of HClO4?

a. 0.56

b.13.44

c.-0.56

d. 14.56

e. minus infinity

Problem 53

What is the pH of a solution that has [OH-] = .

a.3.84 M

b.1.92 M

c. none of these

d. 10.16 M

e.6.90 M

Problem 54

Which of the following is not a strong acid?

a. HClO4

b.H2SO4

c.CH3COOH

d.HCl

e.HNO3

Problem 55

Which of the following statements is/are correct?

a.None of the above statements (a-c) are correct.

b.In a basic solution, [OH-] > [H+].

c.All of the above statements (a-c) are correct.

d.In an acidic solution, [H+] > [OH-].

e.In a neutral solution, [H+] = [OH-].

Problem 58

How many lone pairs of electrons are in the Lewis structure for compound, HF?

a.3

b.4

c.1

d.0

e.none of these

Problem 59

How many of the following will have Lewis structures with multiple bonds?

CO, CO2, CO32-, N2, O2

a.2

b.1

c.3

d.5

e.4

Problem 60

The number of polar covalent bonds in SF4 is

a.none of these

b.3

c.2

d.4

e.1

Problem 61

Which has a bent structure?

a.NH3

b.CO2

c.CaCl2

d.O2

e.H2O

Problem 62

Which has a linear structure?

a.SCl2

b.OF2

c.CO2

d.CaCl2

e.SO2

Problem 63

Which has a planar structure?

a.CO32-

b.H3O+

c.CH4

d.NF3

e.SO32-

Problem 64

Which has a tetrahedral structure?

a.CO32-

b.NH3

c.SO3

d.CH4

e.SO32-

Problem 65

Which has a trigonal pyramid structure?

a.NO3-

b.SO32-

c.CO32-

d.CH4

e.SO3

Problem 66

Which of the following bonds does not have a dipole moment?

a.C-H

b.B-F

c.Br-H

d.F-F

e.F-H

Problem 67

Which of these has more than one reasonable resonance structure?

a.SiCl4

b.BH4-

c.NO3-

d.N2H4

e.PH3

Problem 68

True or false? A bond is a force that holds groups of two or more atoms together and makes them function as a unit.

True

False

Problem 69

True or false? CH4 has ionic bonds.

True

False

Problem 70

True or false? Covalent bonding occurs when a metal reacts with a nonmetal.

True

False.

Reference no: EM131061613

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