Stoich

1.

B

What amount of oxygen, O2, (in moles) contains 1.8×10^22 molecules?

A. 0.0030

B. 0.030

C. 0.30

D. 3.0

2.

B

Which compound has the empirical formula with the greatest mass?

A. C2H6

B. C4H10

C. C5H10

D. C6H6

3.

D

__C2H2(g) + __O2(g) → __ CO2(g) + __ H2O(g)

When the equation above is balanced, what is the coefficient for oxygen?

A. 2

B. 3

C. 4

D. 5

4.

C

3.0 dm3 of sulfur dioxide is reacted with 2.0 dm3 of oxygen according to the equation below. 2SO2(g) + O2(g) → 2SO3(g)

What volume of sulfur trioxide (in dm3) is formed? (Assume the reaction goes to completion and all gases are measured at the same temperature and pressure.)

A. 5.0

B. 4.0

C. 3.0

D. 2.0

5.

A

What will happen to the volume of a fixed mass of gas when its pressure and temperature (in Kelvin) are both doubled?

A. It will not change.

B. It will increase.

C. It will decrease.

D. The change cannot be predicted.

6.

B

What volume (in dm3) of 0.30 mol dm–3 NaCl solution can be prepared from 0.060 mol of solute?

A. 0.018

B. 0.2

C. 0.50

D. 5.0

7.

D

Ag(s) + NO3–(aq) + H+(aq) Ag+(aq) + NO(g) + H2O(l)

When the oxidation-reduction equation above is balanced, what is the coefficient for H+(aq)?

A.1

B. 2

C.3

D.4

8.

A

What amount (in moles) is present in 2.0 g of sodium hydroxide, NaOH?

A. 0.050

B. 0.10

C. 20

D. 80

9.

B

A hydrocarbon contains 90% by mass of carbon. What is its empirical formula?

A. CH2

B. C3H4

C. C7H10

D. C9H10

10.

C

Copper can react with nitric acid as follows.

3Cu +_HNO3 _Cu(NO3)2 +_H2O + _NO

What is the coefficient for HNO3 when the equation is balanced?

A. 4

B. 6

C. 8

D. 10

11.

B

Lithium hydroxide reacts with carbon dioxide as follows. 2LiOH + CO2 → Li2 CO3 + H2O

What mass (in grams) of lithium hydroxide is needed to react with 11 g of carbon dioxide?

A. 6

B. 12

C. 24

D. 48

12.

D

Which change in conditions would increase the volume of a fixed mass of gas?

13.

A

Which solution contains the smallest amount of H+ ions?

A. 10.0 cm3 of 0.250 mol dm–3 HCl

B. 20.0 cm3 of 0.250 mol dm–3 HCl

C. 10.0 cm3 of 0.500 mol dm–3 HCl

D. 10.0 cm3 of 0.250 mol dm–3 H2SO4

14.

D

How many hydrogen atoms are contained in one mole of ethanol, C2H5OH?

A. 5

B. 6

C. 1.0×10^23

D. 3.6×10^24

15.

B

The percentage by mass of the elements in a compound is

C = 72%, H = 12%, O = 16%.

What is the mole ratio of C:H in the empirical formula of this compound?

A. 1 : 1

B. 1 : 2

C. 1 : 6

D. 6 : 1

16.

C

What is the coefficient for O2(g) when the equation below is balanced? __C3H8(g) + __O2(g) → __CO2(g) + __H2O(g)

A. 2

B. 3

C. 5

D. 7

17.

D

What amount of NaCl (in moles) is required to prepare 250 cm3 of a 0.200 mol dm–3 solution?

A. 50.0

B. 1.25

C. 0.800

D. 0.0500

18.

D

For which set of conditions does a fixed mass of an ideal gas have the greatest volume?

19.

A

Which of the following contains the greatest number of molecules?

A. 1 g of CH3Cl

B. 1 g of CH2Cl2

C. 1 g of CHCl3

D. 1 g of CCl4

20.

C

Which of the following compounds has/have the empirical formula CH2O? I. CH3COOH II. C6H12O6 III. C12H22O11

A. II only

B. III only

C. I and II only

D. II and III only

21.

C

Assuming complete reaction, what volume of 0.200 mol dm–3 HCl(aq) is required to neutralize 25.0 cm3 of 0.200 mol dm–3 Ba(OH)2(aq)?

A. 12.5 cm3

B. 25.0 cm3

C. 50.0 cm3

D. 75.0 cm3

22.

B

Under what conditions would one mole of methane gas, CH4, occupy the smallest volume?

A. 273 K and 1.01×105 Pa

B. 273 K and 2.02×105 Pa

C. 546 K and 1.01×105 Pa

D. 546 K and 2.02×105 Pa

23.

A

The temperature in Kelvin of 2.0 dm3 of an ideal gas is doubled and its pressure is increased by a factor of four. What is the final volume of the gas?

A. 1.0 dm3

B. 2.0 dm3

C. 3.0 dm3

D. 4.0 dm3

24.

A

Consider the following equation.

2C4H10(g) + 13O2(g) 8CO2(g) + 10H2O(1)

How many moles of CO2(g) are produced by the complete combustion of 58 g of butane,

C4H10(g)?

A.4

B.8

C.12

D.16

25.

D

6.0 moles of Fe2O3(s) reacts with 9.0 moles of carbon in a blast furnace according to the equation below.

Fe2O3(s) + 3C(s) → 2Fe(s) + 3CO(g)

What is the limiting reagent and hence the theoretical yield of iron?

26.

D

What volume of 0.500 mol dm–3 HCl(aq) is required to react completely with 10.0 g of calcium carbonate according to the equation below?

CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g)

A. 100 cm3

B. 200 cm3

C. 300 cm3

D.400 cm3

27.

D

Which is a correct definition of the term empirical formula?

A. formula showing the numbers of atoms present in a compound

B. formula showing the numbers of elements present in a compound

C. formula showing the actual numbers of atoms of each element in a compound

D. formula showing the simplest ratio of numbers of atoms of each element in a compound

28.

C

The reaction of ethanal and oxygen can be represented by the unbalanced equation below. __ CH3CHO + __ O2 → __ CO2 + __ H2O

When the equation is balanced using the smallest possible integers, what is the coefficient for O2?

A. 3

B. 4

C. 5

D. 6

29.

C

The equation for the complete combustion of butane is

2C4H10 + 13O2 → 8CO2 + 10H2O

What is the amount (in mol) of carbon dioxide formed by the complete combustion of three moles of butane?

A. 4

B. 8

C. 12

D. 24

30.

C

Which solution contains the greatest amount (in mol) of solute?

A. 10.0 cm3 of 0.500 mol dm–3 NaCl

B. 20.0 cm3 of 0.400 mol dm–3 NaCl

C. 30.0 cm3 of 0.300 mol dm–3 NaCl

D. 40.0 cm3 of 0.200 mol dm–3 NaCl

31.

B

A fixed mass of an ideal gas has a volume of 800 cm3 under certain conditions. The pressure (in kPa) and temperature (in K) are both doubled. What is the volume of the gas after these changes with other conditions remaining the same?

A. 200 cm3

B. 800 cm3

C. 1600 cm3

D. 3200 cm3

32.

B

How many oxygen atoms are present in 0.0500 mol carbon dioxide?

A. 3.01×10^22

B. 6.02×10^22

C. 6.02×10^23

D. 1.20×10^24

33.

B

The complete oxidation of propane produces carbon dioxide and water as shown below.

C3H8 + __O2 __CO2 + __H2O

What is the total of the coefficients for the products in the balanced equation for 1 mole of

propane?

A. 6

B. 7

C. 12

D.13

34.

C

The relative molecular mass (Mr) of a compound is 60. Which formulas are possible for this compound?

I. CH3CH2CH2NH2 II. CH3CH2CH2OH III.CH3CH(OH)CH3

A. I and II only

B. I and III only

C. II and III only

D. I, II, and III

35.

A

35. Which sample has the least number of atoms?

A. 1 mol of H2SO4

B. 1 mol of CH3COOH

C. 2 mol of H2O2

D. 2 mol of NH3

36.

A

Avogadro’s constant has the same value as the number of

A. molecules in 1 mol of solid iodine.

B. atoms in 1 mol of chlorine gas.

C. ions in 1 mol of solid potassium bromide.

D. protons in 1 mol of helium gas.

37.

A

Which aqueous solution contains the most hydrogen ions?

A. 20 cm3 of 2 mol dm–3 sulfuric acid

B. 10 cm3 of 4 mol dm–3 nitric acid

C. 80 cm3 of 0.5 mol dm–3 hydrochloric acid

D. 40 cm3 of 0.5 mol dm–3 sulfuric acid

38.

D

What is the total of all the coefficients in the balanced equation for the reduction of 1 mol of MnO4–?

__ MnO4– +__H+ + __ e– __Mn2+ + __H2O

A. 5

B. 9

C. 17

D. 19

39.

A

Which contains the same number of ions as the value of Avogadro’s constant?

A. 0.5 mol NaCl

B. 0.5 mol MgCl2

C. 1.0 mol Na2O

D. 1.0 mol MgO

40.

C

A reaction occurring in the extraction of lead from its ore can be represented by this unbalanced equation:

__ PbS + __O2 __ PbO + __ SO2

When the equation is balanced using the smallest possible whole numbers, what is the

coefficient for O2?

A. 1

B. 2

C.3

D.4

41.

A

The equation for a reaction occurring in the synthesis of methanol is

CO2 + 3H2 CH3OH + H2O

What is the maximum amount of methanol that can be formed from 2 mol of carbon dioxide and

3 mol of hydrogen?

A. 1 mol

B. 2 mol

C. 3 mol

D. 5 mol

42.

C

Which solution contains 0.1 mol of sodium hydroxide?

A. 1 cm3 of 0.1 mol dm–3 NaOH

B. 10 cm3 of 0.1 mol dm–3 NaOH

C. 100 cm3 of 1.0 mol dm–3 NaOH

D. 1000 cm3 of 1.0 mol dm–3 NaOH

43.

C

A cylinder of gas is at a pressure of 40 kPa. The volume and temperature (in K) are both doubled. What is the pressure of the gas after these changes?

A. 10 kPa

B. 20 kPa

C. 40 kPa

D. 80 kPa

44.

C

Which of the following quantities has units?

A. Relative atomic mass

B. Relative molecular mass

C. Molar mass

D. Mass number

45.

A

What is the purpose of the beam of high energy electrons used in a mass spectrometer?

A. To ionize atoms

B. To accelerate ions

C. To deflect ions

D. To detect ions

46.

C

The empirical formula of a compound is C2H4O. Which molecular formulas are possible for this compound?

I. CH3COOH II. CH3CH2CH2COOH III. CH3COOCH2CH3

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

47.

B

Calcium carbonate decomposes on heating as shown below. CaCO3 CaO + CO2

When 50 g of calcium carbonate are decomposed, 7 g of calcium oxide are formed. What is the percentage yield of calcium oxide?

A. 7%

B. 25%

C. 50%

D. 75%

48.

D

Sodium reacts with water as shown below.

__ Na + __ H2O __ NaOH + __ H2

What is the total of all the coefficients when the equation is balanced using the smallest possible

whole numbers?

A. 3

B. 4

C. 6

D. 7

49.

C

What is the total number of ions present in the formula, Al2(SO4)3?

A. 2

B. 3

C. 5

D. 6

50.

B

A 4 g sample of sodium hydroxide, NaOH, is dissolved in water and made up to 500 cm3 of aqueous solution. What is the concentration of the resulting solution?

A. 0.1 mol dm–3

B. 0.2 mol dm–3

C. 0.5 mol dm–3

D. 1.0 mol dm–3

51.

B

Methane, CH4, burns in oxygen gas to form carbon dioxide and water. How many moles of carbon dioxide will be formed from 8.0 g of methane?

A. 0.25

B. 0.50

C. 1.0

D. 2.0

52.

D

What is the empirical formula of a compound containing 50% by mass of element X (Ar = 20)

and 50% by mass of element Y (Ar = 25)?

A. XY

B. X3Y2

C. X4Y5

D. X5Y4

53.

C

Assuming complete reaction, what volume of 0.200 mol dm–3 potassium hydroxide solution (KOH(aq)), is required to neutralize 25.0 cm3 of 0.200 mol dm–3 aqueous sulfuric acid,

(H2SO4(aq))?

A. 12.5 cm3

B. 25.0 cm3

C. 50.0 cm3

D. 75.0 cm3

54.

A

Consider the following reaction.

N2(g) + 3H2(g) 2NH3(g)

If the reaction is made to go to completion, what volume of ammonia (in dm3) can be prepared

from 25 dm3 of nitrogen and 60 dm3 of hydrogen? All volumes are measured at the same temperature and pressure.

A. 40

B. 50

C. 85

D. 120

55.

B

The temperature in Kelvin of 1.0 dm3 of an ideal gas is doubled and its pressure is tripled. What is the final volume of the gas in dm3?

A.1/3

B.2/3

C.3/2

D.1/6

56.

D

On complete combustion, a sample of a hydrocarbon compound produces 1.5 mol of carbon

dioxide and 2.0 mol of water. What is the molecular formula of this hydrocarbon?

A. C2H2

B. C2H4

C. C3H4

D. C3H8

57.

A

When excess BaCl2(aq) was added to a sample of Fe(NH4)2(SO4)2(aq) to determine the amount in moles of sulfate present, 5.02×10–3 mol of BaSO4 was obtained. How many moles of sulfate

ions and iron ions were in the sample of Fe(NH4)2(SO4)2?

58.

B

What volume of 0.500 mol dm–3 sulfuric acid solution is required to react completely with 10.0 g of calcium carbonate according to the equation below?

￼￼￼CaCO3(s) + H2SO4(aq) CaSO4(aq) + H2O(l) + CO2(g)

A. 100 cm3

B. 200 cm3

C. 300 cm3

D. 400 cm3

59.

A

Which expression gives the amount (in mol) of a substance, if the mass is given in grams?

60.

C

What is the total number of atoms in 0.20 mol of propanone, CH3COCH3?

A. 1.2×10^22

B. 6.0×10^23

C. 1.2×10^24

D. 6.0×10^24

61.

C

When the equation below is balanced for 1 mol of C3H4, what is the coefficient for O2?

C3C4 + _O2 -> _CO2 + _H2O

A.2

B.3

C.4

D.5

62.

C

Ethyne, C2H2, reacts with oxygen according to the equation below. What volume of oxygen (in dm3) reacts with 0.40 dm3 of C2H2?

2C2H2(g) + 5O2(g) 4CO2(g) + 2H2O(g)

A. 0.40

B. 0.80

C. 1.0

D. 2.0

63.

C

Ethyne, C2H2, reacts with oxygen according to the equation below. What volume of oxygen (in dm3) reacts with 0.40 dm3 of C2H2?

2C2H2(g) + 5O2(g) 4CO2(g) + 2H2O(g)

A. 0.40

B. 0.80

C. 1.0

D. 2.0

64.

D

What is the coefficient for H+ when the redox equation below is balanced?

_Ag(s) + _NO3–(aq) +_H+(aq) -> _Ag+(aq) + _NO(g) + _H2O(l)

A.1

B.2

C.3

D.4

65.

B

How many hydrogen atoms are in one mole of ethanol, C2H5OH?

A. 1.00×10^23

B. 3.61×10^24

C. 5.00

D. 6.00

66.

C

What is the coefficient for H2SO4(aq) when the following equation is balanced, using the smallest possible integers?

__Mg3N2(s) + __H2SO4(aq) → __MgSO4(aq) + __(NH4)2SO4(aq)

A.1

B.3

C.4

D.7

67.

C

Air bags in cars inflate when sodium azide decomposes to form sodium and nitrogen: 2NaN3(s) → 2Na(s) + 3N2(g)

Calculate the amount, in moles, of nitrogen gas produced by the decomposition of 2.52 mol of NaN3(s).

￼￼A. 1.68

B. 2.52

C. 3.78

D. 7.56

68.

C

What volume, in cm3, of 0.200 mol dm–3 HCl(aq) is required to neutralize 25.0 cm3 of 0.200 mol dm–3 Ba(OH)2(aq)?

A. 12.5

B. 25.0

C. 50.0

D. 75.0

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