Free Printable Topic 1 SL Chemistry Stoichiometry

1.

What is the sum of the coefficients when the equation is balanced with whole numbers?

__MnO₂ (s) + __HCl (aq) → __MnCl₂ (aq) + __H₂O (l) + __Cl₂ (g)

a)

6

b)

7

c)

8

d)

9

2.

Which is correct?

a)

Mixtures are either homogeneous or heterogeneous and their chemical properties are an average of the individual component properties.

b)

Mixtures are never heterogeneous and their chemical properties are an average of the individual component properties.

c)

Mixtures are either homogeneous or heterogeneous and the components retain their individual chemical properties.

d)

Mixtures are never homogeneous and the components retain their individual chemical properties.

3.

What is the sum of the coefficients when the equation is balanced with the smallest whole numbers?

__BaCl₂ (aq) + __Fe₂(SO₄)₃ (aq) → __FeCl₃ (aq) + __BaSO₄ (s)

a)

4

b)

6

c)

8

d)

9

4.

What is the sum of the integer coefficients when propene undergoes complete combustion?

__C₃H₆ (g) + __O₂ (g) → __CO₂ (g) + __H₂O (l)

a)

11

b)

17

c)

21

d)

23

5.

Which diagram represents a heterogeneous mixture?

a)

b)

c)

d)

6.

Which is a homogeneous mixture?

a)

Oil and water

b)

Sand and water

c)

Ethanol and water

d)

Chalk and sand

7.

What is the sum of the coefficients when the equation is balanced with the lowest whole number ratio?

__Na₂S₂O₃(aq) + __HCl(aq) → __S(s) + __SO₂(g) + __NaCl(aq) + __H₂O(l)

a)

6

b)

7

c)

8

d)

9

8.

What is the sum of the coefficients when the following equation is balanced using the smallest whole numbers?

__C₆H₁₂O₆ (aq) → __C₂H₅OH (aq) + __CO₂ (g)

a)

4

b)

5

c)

9

d)

10

9.

Which statements about mixtures are correct?

I.The components may be elements or compounds.

II.All components must be in the same phase.

III.The components retain their individual properties.

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

10.

What is the sum of the coefficients when the equation is balanced with whole numbers?

_—C₈H₁₈(g) + _—O₂(g) → _—CO(g) + _—H₂O(l)

a)

26.5

b)

30

c)

53

d)

61

11.

Which equation represents sublimation?

a)

2Al(s)+3I₂(g)→2AlI₃(s)

b)

HgCl₂(s)→HgCl₂(g)

c)

I₂(g)→I₂(s)

d)

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

12.

Some sodium chloride is dissolved in water. Which term describes the role of sodium chloride in this process?

a)

Solute

b)

Solvent

c)

Solution

d)

Saturated

13.

Nitroglycerine, C₃H₅N₃O₉, can be used in the manufacture of explosives.

What is the coefficient of C₃H₅N₃O₉(l) when the equation for its decomposition reaction is balanced using the lowest whole numbers?

__ C₃H₅N₃O₉(l)→__ CO₂(g)+ __ H₂O(l)+ __ N₂(g)+ __ O₂(g)

a)

2

b)

4

c)

20

d)

33

14.

Which statements about solutions are correct?
I. A solute dissolves in a solvent to form a solution.
II. A solution is a homogeneous mixture of two or more substances.
III. Concentrations of solutions can be expressed in gdm−3
.

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

15.

What is the sum of the coefficients when the following equation is balanced using whole numbers?

___ Fe₂O₃(s)+___ CO(g)→ ___ Fe(s)+ ___ CO₂(g)

a)

5

b)

6

c)

8

d)

9

16.

What is the sum of all coefficients when the following equation is balanced using the smallest possible whole numbers?

__ C₂H₂+ __ O₂→ __ CO₂+ __ H₂

a)

4

b)

5

c)

6

d)

7

17.

What is the sum of the coefficients for the equation when balanced using the smallest possible whole numbers?

__ N₂H₄(g)+ __ O₂(g)→ __ NO₂(g)+ __ H₂

a)

5

b)

6

c)

7

d)

8

18.

Which contains the greatest number of moles of oxygen atoms?

a)

0.05 mol Mg(NO₃)₂

b)

0.05 mol C₆H₄(NO₂)₂

c)

0.1 mol H₂O

d)

0.1 mol NO₂

19.

What is the empirical formula of a hydrocarbon with 75 % carbon and 25 % hydrogen by mass?

a)

C₃H

b)

CH₂

c)

C₂H₆

d)

CH₄

20.

How many moles of magnesium hydroxide are produced with 0.50 mol of ammonia?

Mg₃N₂ (s) + 6H₂O (l) → 3Mg(OH)₂ (aq) + 2NH₃ (aq)

a)

0.25

b)

0.33

c)

0.75

d)

1.5

21.

How many moles of FeS₂ are required to produce 32 g of SO₂? (A_r: S = 32, O = 16)

4FeS₂ (s) + 11O₂ (g) → 2Fe₂O₃ (s) + 8SO₂ (g)

a)

0.25

b)

0.50

c)

1.0

d)

2.0

22.

16 g of bromine react with 5.2 g of metal, M, to form MBr₂. What is the relative atomic mass of the metal M? (A_r: Br = 80)

a)

13

b)

26

c)

52

d)

104

23.

What is the molecular formula of a hydrocarbon containing 84.6% carbon by mass with a molar mass of 142.3 g mol⁻¹?

a)

C₂₀H₄₄

b)

C₁₁H₁₀

c)

C₁₀H₂₂

d)

C₅H₁₁

24.

What is the number of atoms of oxygen in 2.0 mol of hydrated sodium carbonate, Na₂CO₃•10H₂O?

Avogadro’s constant, L or N_A: 6.02 × 10²³ mol^–1

a)

6

b)

26

c)

3.6 × 10²⁴

d)

1.6 × 10²⁵

25.

What is the number of atoms of oxygen in 2.0 mol of hydrated sodium carbonate, Na₂CO₃•10H₂O?

Avogadro’s constant, L or N_A: 6.02 × 10²³ mol^–1

a)

6

b)

26

c)

3.6 × 10²⁴

d)

1.6 × 10²⁵

26.

How many atoms of nitrogen are there in 0.50 mol of (NH₄)₂CO₃?

a)

1

b)

2

c)

3.01 × 10²³

d)

6.02 × 10²³

27.

What is the value of x when 32.2 g of Na₂SO₄•xH₂O are heated leaving 14.2 g of anhydrous Na₂SO₄?

M_r(H₂O) = 18;

M_r(Na₂SO₄) = 142.

Na₂SO_4•xH₂O (s) → Na₂SO₄ (s) + xH₂O (g)

a)

0.1

b)

1

c)

5

d)

10

28.

How many grams of sodium azide, NaN₃, are needed to produce 68.1 dm³ of N₂ (g) at STP?

Molar volume at STP = 22.7 dm³ mol^–1

M_r(NaN₃) = 65.0

2NaN₃ (s) → 3N₂ (g) + 2Na (s)

a)

32.5

b)

65.0

c)

130.0

d)

195.0

29.

Which compound has the greatest percentage by mass of nitrogen atoms?

a)

N₂H₄

b)

NH₃

c)

N₂O₄

d)

NaNO₃

30.

How many moles of oxygen atoms are there in 0.500 mol of hydrated iron(II) ammonium sulfate, (NH₄)₂Fe(SO₄)₂•6H₂O(s)?

a)

4.00

b)

7.00

c)

8.00

d)

14.00

31.

Which solution neutralizes 50.0 cm³ of 0.120 mol dm^–3 NaOH (aq)?

a)

12.5 cm³ of 0.080 mol dm^–3 H₃PO₄

b)

25.0 cm³ of 0.120 mol dm^–3 CH₃COOH

c)

25.0 cm³ of 0.120 mol dm^–3 H₂SO₄

d)

50.0 cm³ of 0.060 mol dm^–3 HNO₃

32.

A compound with M_r = 102 contains 58.8 % carbon, 9.80 % hydrogen and 31 % oxygen by mass.

What is its molecular formula?

A_r: C = 12.0; H = 1.0; O = 16.0

a)

C₂H₁₄O₄

b)

C₃H₄O₄

c)

C₅H₁₀O₂

d)

C₆H₁₄O

33.

Which sample contains the largest amount, in mol, of oxygen atoms?

a)

$0.20\ mol\ P_2O_5$

b)

$0.3\ mol\ O_3$

c)

$0.4\ mol\ CH_3COOH$

d)

$0.8\ mol\ H_2O$

34.

Which compound has the highest percentage of carbon by mass?

a)

$CH_4$

b)

$C_2H_4$

c)

$C_4H_{10}$

d)

$C_6H_6$

35.

What is the total number of protons and electrons in one mole of hydrogen gas?

a)

2

b)

4

c)

$1.2\ x\ 10^{24}$

d)

$2.4\ x\ 10^{24}$

36.

A hydrocarbon contains 85.7 % carbon by mass. What is the empirical formula of the hydrocarbon?

a)

$C_2H_3$

b)

$CH_2$

c)

$C_2H_5$

d)

$CH_3$

37.

How many atoms are present in 0.500 mol of NH₃?

a)

1.20×10²³

b)

3.01×10²³

c)

6.02×10²³

d)

1.20×10²⁴

38.

The structural formula of a dioxin is shown below. What is its empirical formula?

a)

$C_6O$

b)

$C_6H_4O$

c)

$C_6H_6O$

d)

$C_{12}H_8O$

39.

What is the mass, in g, of one mole of hydrated copper(II) sulfate, CuSO₄∙5H2O, given the following relative atomic mass values?

a)

169

b)

178

c)

186

d)

250

40.

For which compounds is the empirical formula the same as the molecular formula?

I. Methane

II. Ethene

III. Ethanol

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

41.

Which represents an empirical formula?

a)

$C_2H_4$

b)

$B_2H_6$

c)

$Al_2O_3$

d)

$C_6H_6$

42.

Which statements are correct about Avogadro’s constant?

I. It is the number of ions in 12 g of sodium hydride, NaH.

II. It is the number of molecules in 22.4 dm³ of hydrogen gas at 0 °C and 1 atm.

III. It is the number of atoms in 12 g of 12C.

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

43.

What is the molar mass, in gmol^−1, of a substance if 0.30 mol of the substance has a mass of 18 g?

a)

5.4

b)

6.0

c)

30

d)

60

44.

Which contains the largest number of ions?

a)

$1\ mole\ of\ Al_2\left(SO_4\right)_3$

b)

$1\ mole\ of\ Mg_3\left(PO_4\right)_2$

c)

$2\ moles\ of\ K_3PO_4$

d)

$3\ moles\ of\ NaNO$

45.

Which is the best description of relative atomic mass, A_r?

a)

The number of neutrons and protons present in the nucleus of an atom

b)

The average number of neutrons and protons in all isotopes of an element

c)

The weighted mean mass of naturally occurring isotopes of an element compared to the mass of an atom of carbon-12

d)

The weighted mean mass of naturally occurring isotopes of an element compared to 1/12^thof the mass of an atom of carbon-12

46.

What is the number of ions in 0.20 moles of (NH₄)₃PO₄?

a)

$8.0\ x\ 10^{-1}$

b)

$1.2\ x\ 10^{23}$

c)

$4.8\ x\ 10^{23}$

d)

$2.4\ x\ 10^{24}$

47.

What is the molar mass, in gmol^-1, of Na₂CO₃•H₂O?

a)

105.99

b)

124.00

c)

263.15

d)

286.19

48.

What is the total number of atoms in 0.100 mol of Pt(NH₃)₂Cl₂?

a)

11

b)

$6.02\ x\ 10^{22}$

c)

$3.01\ x\ 10^{23}$

d)

$6.62\ x\ 10^{23}$

49.

How many molecules are present in a drop of ethanol, C₂H₅OH, with a mass of 2.3×10⁻³ g?

a)

$3.0\ x\ 10^{19}$

b)

$3.0\ x\ 10^{20}$

c)

$6.0\ x\ 10^{20}$

d)

$6.0\ x\ 10^{26}$

50.

Which sample has the greatest mass?

a)

$1\ mol\ of\ SO_2$

b)

$2\ mol\ of\ N_2O$

c)

$2\ mol\ of\ Ar$

d)

$4\ mol\ of\ NH_3$

51.

The relative molecular mass of a gas is 56 and its empirical formula is CH₂. What is the molecular formula of the gas?

a)

$CH_2$

b)

$C_2H_4$

c)

$C_3H_6$

d)

$C_4H_8$

52.

What is the total number of nitrogen atoms in two moles of NH₄NO₃?

a)

$4$

b)

$6.02\ x\ 10^{23}$

c)

$1.20\ x\ 10^{24}$

d)

$2.41\ x\ 10^{24}$

53.

Which molecular formula is also an empirical formula?

a)

$PCl_3$

b)

$C_2H_4$

c)

$H_2O_2$

d)

$C_6H_{12}O_6$

54.

300cm³ of water is added to a solution of 200cm³ of 0.5moldm^-3 of sodium chloride. What is the concentration of sodium chloride in the new solution?

a)

$0.05\ mol\ dm^{-3}$

b)

$0.1\ mol\ dm^{-3}$

c)

$0.2\ mol\ dm^{-3}$

d)

$0.3\ mol\ dm^{-3}$

55.

Which non-metal forms an oxide XO₂with a relative molecular mass of 60?

a)

C

b)

N

c)

Si

d)

S

56.

4.00 mol of a hydrocarbon with an empirical formula of CH₂ has a mass of 280 g. What is the molecular formula of this compound?

a)

$C_2H_4$

b)

$C_3H_6$

c)

$C_4H_8$

d)

$C_5H_{10}$

57.

The molar mass of a compound is approximately 56 gmol^-1. Which formula is possible for this compound?

a)

NaNO₃

b)

AgOH

c)

MgO

d)

KOH

58.

Which compound has the empirical formula with the largest mass?

a)

$C_2H_6$

b)

$C_2H_4$

c)

$CH_2$

d)

$C_3H_6$

59.

0.10 mol of hydrochloric acid is mixed with 0.10 mol of calcium carbonate.

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

Which is correct?

a)

A

b)

B

c)

C

d)

D

60.

What is the volume of gas when the pressure on 100 cm³ of gas is changed from 400 kPa to 200 kPa at constant temperature?

a)

50.0 cm³

b)

100 cm³

c)

200 cm³

d)

800 cm³

61.

What is the concentration, in mol dm⁻³, of 20.0 g of NaOH (M_r = 40.0) in 500.0 cm³?

a)

0.250

b)

0.500

c)

1.00

d)

4.00

62.

What volume of carbon dioxide, CO₂ (g), can be obtained by reacting 1 dm³ of methane, CH₄ (g), with 1 dm³ of oxygen, O₂ (g)?

CH₄ (g) + 2O₂ (g) → CO₂ (g) + 2H₂O (l)

a)

0.5 dm³

b)

1 dm³

c)

2 dm³

d)

6 dm³

63.

What is the volume of gas when the pressure on 100 cm³ of gas is changed from 400 kPa to 200 kPa at constant temperature?

a)

50.0 cm³

b)

100 cm³

c)

200 cm³

d)

800 cm³

64.

The volume of a sample of gas measured at 27 °C is 10.0 dm³. What is the temperature when the volume is reduced to 9.0 dm³ at the same pressure?

a)

−3.0 °C

b)

24.3 °C

c)

29.7 °C

d)

57.0 °C

65.

An antacid tablet containing 0.50 g of NaHCO₃ (M_r = 84) is dissolved in water to give a volume of 250 cm³. What is the concentration, in mol dm⁻³, of HCO₃⁻ in this solution?

a)

$\frac{\text{0.250 }x\ 84}{\text{0.50}}$

b)

$\frac{\text{0.50 }}{\text{84 x 0.250}}$

c)

$\frac{\text{250 x 84}}{\text{0.50}}$

d)

$\frac{\text{0.50}}{\text{84 x 250}}$

66.

Which graph shows the relationship between the volume and pressure of a fixed mass of an ideal gas?

a)

A

b)

B

c)

C

d)

D

67.

What is the percentage yield when 7 g of ethene produces 6 g of ethanol?

M_r(ethene) = 28 and M_r(ethanol) = 46

C₂H₄(g) + H₂O(g) → C₂H₅OH(g)

a)

$\frac{6\ x\ 7\ x\ 100}{28\ x\ 46}$

b)

$\frac{6\ x\ 46\ x\ 100}{7\ x\ 28}$

c)

$\frac{6\ x\ 28}{7\ x\ 46\ x\ 100}$

d)

$\frac{6\ x\ 28\ x\ 100}{7\ x\ 46}$

68.

Which volume, in cm³, of 0.20 mol dm^-3 NaOH (aq) is needed to neutralize 0.050 mol of H₂S(g)?

H₂S(g) + 2NaOH(aq) → Na₂S(aq) + 2H₂O(l)

a)

0.25

b)

0.50

c)

250

d)

500

69.

In which mixture is NaOH the limiting reagent?

a)

0.20mol NaOH + 0.10mol H₂SO₄

b)

0.10mol NaOH + 0.10mol H₂SO₄

c)

0.20mol NaOH + 0.10mol HNO₃

d)

0.10mol NaOH + 0.10mol HNO₃

70.

The complete combustion of 15.0cm³ of a gaseous hydrocarbon X produces 60.0 cm³ of carbon dioxide gas and 75.0 cm³ of water vapour. What is the molecular formula of X? (All volumes are measured at the same temperature and pressure.)

A. C₄H₆

B. C₄H₈

C. C₄H₁₀

D. C₆H₁₀

a)

$C_4H_6$

b)

$C_4H_8$

c)

$C_4H_{10}$

d)

$C_6H_{10}$

71.

Why do gases deviate from the ideal gas law at high pressures?

a)

Molecules have finite volume.

b)

Cohesive forces increase the volume from the ideal.

c)

Increasing pressure increases the temperature of the gas.

d)

Collisions between molecules occur more frequently as pressure increases.

72.

Combustion of ethanol takes place according to the following unbalanced equation.

__ C₂H₅OH(l) + __ O₂(g) → __ CO₂(g) + __ H₂O(l)

What is the mole ratio of ethanol to oxygen in the balanced equation?

a)

1:1

b)

2:1

c)

1:3

d)

2:7

73.

Which solution contains the biggest amount, in mol, of chloride ions?

a)

20cm³ of 0.50mol dm^-3 of NH₄Cl

b)

60cm³ of 0.20mol dm^-3 of MgCl₂

c)

70cm³ of 0.30mol dm^-3 of NaCl

d)

100cm³ of 0.30mol dm^-3 of ClCH₂COOH

74.

4.0 g of solid sodium hydroxide is added to 0.10 dm3 of 1.0 mol dm⁻³ aqueous sulfuric acid. 2NaOH(s) + H₂SO₄(aq) → Na₂SO₄(aq) + 2H₂O(l) Which statement is correct?

a)

Neither reactant is in excess.

b)

0.10 mol Na₂SO₄ is formed

c)

Excess H₂SO₄ remains in solution

d)

Excess NaOH remains in solution.

75.

0.040 mol of (NH₄)₂Ni(SO₄)₂•6H₂O is dissolved in water to give 200 cm³ of aqueous solution. What is the concentration, in mol dm^-3, of ammonium ions?

a)

0.00040

b)

0.0080

c)

0.20

d)

0.40

76.

When sodium bromate(V), NaBrO₃, is heated, it reacts according to this equation.

2NaBrO₃(s)→2NaBr(s)+3O₂(g)

What amount, in mol, of NaBrO₃ produces 2.4 dm³ of oxygen gas, measured at room temperature and pressure? (Molar volume of gas =24 dm³mol⁻¹ at room temperature and pressure.)

a)

0.017

b)

0.067

c)

0.10

d)

0.15

77.

Aluminium carbide reacts with water according to the equation below. What is the sum of all the coefficients when the equation is balanced?

__Al₄C₃(s) + __ H₂O(l) → __ Al(OH)₃(s) + __ CH₄(g)

a)

13

b)

14

c)

19

d)

20

78.

At which temperature, in K, assuming constant pressure, is the volume of a fixed mass of gas at 127 °C doubled?

a)

200 K

b)

254 K

c)

400 K

d)

800 K

79.

100.0 cm³ of a 0.50M solution of BaCl₂ is added to 50.0 cm³ of a 0.10M solution of Na₂SO₄. A precipitate of BaSO₄ is formed according to the equation below.

BaCl₂(aq) + Na₂SO₄(aq) → BaSO₄(s) + 2NaCl(aq)

What is the amount, in mol, of BaSO₄produced?

a)

0.0050

b)

0.10

c)

0.50

d)

0.10

80.

Which volumes of gases at standard temperature and pressure have the same mass as 100 cm³ of O₂?

I. 50 cm³ of SO₂

II. 100 cm³ of CH₄

III. 100 cm³ of SiH₄

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

81.

What is the pressure, in Pa, if 3 moles of gas occupies 500 cm³ at 25 °C?

Given: R = 8.31JK^-1mol^-1

a)

$\frac{3\ x\ 8.31\ x\ 298}{500}$

b)

$\frac{3\ x\ 8.31\ x\ 25}{0.0005}$

c)

$\frac{3\ x\ 8.31\ x\ 25}{500}$

d)

$\frac{3\ x\ 8.31\ x\ 298}{0.0005}$

82.

7.102 g of Na₂SO₄ (M=142.04 gmol⁻¹) is dissolved in water to prepare 0.5000 dm³ of solution. What is the concentration of Na₂SO₄ in mol/L?

a)

$2.500\ x\ 10^{-2}$

b)

$1.000\ x\ 10^{-1}$

c)

$1.000\ x\ 10$

d)

$1.000\ x\ 10^2$

83.

When 50 cm³ of a hydrocarbon, CxHy, was burned in excess oxygen, 200 cm³ of carbon dioxide and 250 cm³ of steam were produced (all volumes were measured under the same conditions).

What is the molecular formula of the hydrocarbon?

a)

$C_2H_4$

b)

$C_3H_8$

c)

$C_4H_8$

d)

$C_4H_{10}$

84.

What is the pressure, in Pa, in a 100 cm3container containing 1.8 g of steam at a temperature of 727 °C?
$R\ =\ 8.31\ JK^{-1}mol^{-1}$

a)

$\frac{1.8\ x\ 8.31\ x\ 727}{18\ x\ 100}$

b)

$\frac{18\ x\ 100}{1.8\ x\ 8.31\ x\ 727}$

c)

$\frac{1.8\ x\ 8.31\ x\ 1000}{18\ x\ 10^{-4}}$

d)

$\frac{1.8\ x\ 8.31}{1.8\ x\ 10^{-4}\ x\ 1000}$

85.

What mass of carbon dioxide, CO₂(g), in g, is produced when 5.0 g of calcium carbonate, CaCO₃(s), reacts completely with hydrochloric acid, HCl(aq)?

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

a)

0.050

b)

2.2

c)

4.4

d)

5.0

86.

What volume of carbon dioxide, CO₂(g), in dm³, is produced when 1 dm³of octane, C₈H₁₈(g), undergoes complete combustion?

2C₈H₁₈(g) + 25O₂(g) → 16CO₂(g) + 18H₂O(g)

a)

1

b)

4

c)

8

d)

9

87.

7.102 g of Na₂SO₄ (M = 142.04 g mol^–1) is dissolved in water to prepare 0.5000 dm³ of solution. What is the concentration of Na₂SO₄ in M?

a)

$2.500\ x\ 10^{-2}$

b)

$1.000\ x\ 10^{-1}$

c)

$1.000\ x\ 10$

d)

$1.000\ x\ 10^2$

88.

Which graph represents the relationship between volume and pressure for a fixed mass of gas at constant temperature?A

a)

A

b)

B

c)

C

d)

D

89.

The equation for the reduction of iron(III) oxide is:

Fe₂O₃(s) + 3CO(g) → 2Fe(s) + 3CO₂(g)

What mass of carbon dioxide, in g, is produced by the complete reduction of 80 g of iron(III) oxide?

a)

44

b)

68

c)

88

d)

132

90.

3.0 dm³ of ethyne, C₂H₂, is mixed with 3.0 dm³

of hydrogen and ignited. The equation for the reaction that occurs is shown below.

C₂H₂(g) + 2H₂(g) → C₂H₆(g)

Assuming the reaction goes to completion and all gas volumes are measured at the same temperature and pressure, what volume of ethane, C₂H₆, in dm³, is formed?

a)

1.5

b)

2.0

c)

3.0

d)

6.0

91.

What is the amount, in moles, of sulfate ions in 100 cm³ of 0.020 mol/L FeSO₄(aq)?

a)

$2.0\ x\ 10^{-3}$

b)

$2.0\ x\ 10^{-2}$

c)

$2.0\ x\ 10^{-1}$

d)

$2$

92.

1.7 g of NaNO₃ (Mr=85) is dissolved in water to prepare 0.20 dm³ of solution. What is the concentration of the resulting solution in mol/L?

a)

0.01

b)

0.1

c)

0.2

d)

1.0

93.

Chloroethene, C₂H₃Cl, reacts with oxygen according to the equation below.

2C₂H₃Cl(g) + 5O₂(g) → 4CO₂(g) + 2H₂O(g) + 2HCl(g)

What is the amount, in mol, of H₂O produced when 10.0 mol of C₂H₃Cl and 10.0 mol of O₂ are mixed together, and the above reaction goes to completion?

a)

4.00

b)

8.00

c)

10.0

d)

20.0

94.

A fixed mass of gas has a certain volume at a temperature of 50 °C. What temperature is required to double its volume while keeping the pressure constant?

a)

100K

b)

323K

c)

373K

d)

646K

95.

What is the concentration of NaCl, in mol/L, when 10.0 cm³ of 0.200 mol/L NaCl solution is added to 30.0 cm³ of 0.600 mol/L NaCl solution?

a)

0.450

b)

0.300

c)

0.500

d)

0.800

96.

Four identical containers under the same conditions are filled with gases as shown below. Which container and contents will have the highest mass?

a)

A

b)

B

c)

C

d)

D

97.

What mass, in g, of hydrogen is formed when 3 mol of aluminium react with excess hydrochloric acid according to the following equation?

2Al(s) + 6HCl(aq) → 2AlCl₃(aq) + 3H₂(g)

a)

3.0

b)

4.5

c)

6.0

d)

9.0

Topic 1 SL Chemistry Stoichiometry

Total questions: 97

Worksheet time: 9hrs 17mins

Similar Resources on Wayground