IB Chemistry Topic R2.1 How Much? the Amount of Chemical Change Questionbank (SL/HL)

IB Chemistry Topic R2.1 How Much? the Amount of Chemical Change Questionbank (SL/HL) | RevisionDojo

Practice IB Chemistry Topic R2.1 How Much? the Amount of Chemical Change with authentic exam-style questions for both SL and HL students. This question bank focuses on the exact syllabus content for R2.1 How Much? the Amount of Chemical Change and mirrors Paper 1A, 1B, 2 style where relevant.

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Paper

Level

Question 1

SLPaper 2

Zinc reacts with dilute sulfuric acid according to the following equation:

$Zn (s) + H_{2} S O_{4} (aq) \to ZnS O_{4} (aq) + H_{2} (g)$

A student reacts $3.00 g$ of zinc with $25.0 c m^{3}$ of $1.00 mol d m^{- 3}$ sulfuric acid.

Determine the limiting reactant in this reaction.

[2]

Calculate the volume of hydrogen gas produced at STP.

[2]

If the experiment yields 85% of the expected hydrogen gas, calculate the actual volume collected.

[1]

Question 2

SLPaper 2

A gaseous hydrocarbon is found to have an empirical formula of $C H_{2}$ . At standard temperature and pressure (STP), the density of this gas is $1.85 g dm^{- 3}$ .

Calculate the molar mass of the hydrocarbon and determine its molecular formula, using $22.7 dm^{3} mol^{- 1}$ as the molar volume of an ideal gas at STP.

Molar mass:

Molecular formula:

[3]

Silver metal can be recovered from a solution of silver nitrate by a displacement reaction with copper.

$C u (s) + 2 A g N O_{3} (a q) \to C u (N O_{3})_{2} (a q) + 2 A g (s)$

A $1.27 g$ sample of copper is added to $50.0 cm^{3}$ of $0.400 mol dm^{- 3}$ silver nitrate solution. Determine the limiting reactant and calculate the maximum mass of silver, in grams, that can be produced.

[4]

Question 3

SLPaper 1A

A student recorded the following burette readings during a titration:

Initial volume: $5.00 \pm 0.05 c m^{3}$

Final volume: $15.00 \pm 0.05 c m^{3}$

What is the percentage uncertainty in the volume of solution delivered?

Question 4

HLPaper 2

A reaction vessel is charged with aluminum and chlorine gas to synthesize aluminum chloride ( $A l C l_{3}$ ). The initial quantities of the reactants are provided in the table below.

Reactant	Initial amount / mol
Aluminum ( $Al$ )	$0.500$
Chlorine ( $Cl_2$ )	$0.600$

Using the balanced equation $2 Al(s) + 3 Cl_{2} (g) \to 2 AlCl_{3} (s)$ , deduce the maximum amount, in mol, of aluminum chloride that can be produced from this mixture.

[1]

Determine the mass, in g, of the reactant that remains in excess at the end of the reaction. ( $A_{r} (A l) = 26.98$ )

[2]

Question 5

SL & HLPaper 1A

Methane, $CH_{4}$ , undergoes complete combustion when oxygen is in excess, as represented by the equation below:

$CH_{4} (g) + 2 O_{2} (g) \to CO_{2} (g) + 2 H_{2} O(l)$

When $12.0 g$ of methane is fully burned, what is the greatest mass of carbon dioxide that could be produced?

IB Chemistry R2.1 How Much? the Amount of Chemical Change Questionbank

IB Chemistry R2.1 How Much? the Amount of Chemical Change Questionbank

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