Are you ready for your Year 11 Chemistry Yearly Exam? Assess your exam-readiness with these commonly asked exam questions.
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The Matrix Year 11 Chemistry Yearly Exam Paper contains questions based on the new Year 11 Chemistry syllabus and covers the four modules of the Year 11 Chemistry course:
We have listed below some of the most popular exam questions for your quick reference. You can download the free Matrix Year 11 Chemistry Practice Paper:
Commonly asked exam questions on Module 1 Properties & Structures of Matter are:
Which VSEPR shape always results in a polar molecule?
(A) Linear
(B) Trigonal Planar
(C) Tetrahedral
(D) Bent
Write the full electronic configuration of a sodium atom.
Define the term “electronegativity’.
Explain why methane has a lower boiling point than water.
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Module 2: Introduction to Quantitative Chemistry
Commonly asked exam questions on Module 1 Properties & Structures of Matter are:
Which gas law describes the relationship between pressure and volume?
(A) Boyle’s Law
(B) Charles’ Law
(C) Avogadro’s Law
(D) Gay-Lussac’s Law
3.75 g of potassium carbonate was placed in 280 mL of 0.14 M hydrochloric acid. The following reaction occurs:
K2CO3(aq) + 2HCl(aq) → 2KCl(aq) + CO2(g) + H2O(l)
(A) Write the full ionic equation for this reaction.
(B) Write the net ionic equation for this reaction.
(C) What mass of potassium chloride will be produced?
Commonly asked exam questions on Module 3 Reactive Chemistry are:
A galvanic cell was constructed by connecting a graphite electrode in a solution of iron(II) nitrate and iron(III) nitrate, and a tine electrode in a solution of tin(II) chloride.
What is the cell potential under standard conditions?
(A) 0.91 V
(B) 0.63 V
(C) 030 V
(D) 1.68 V
2.37 g of aluminium was combusted in excess oxygen gas:
4Al(s) + 3O2(g) → 2Al2O3(s)
(a) How many moles of aluminium reacted?
(b) What mass of aluminium oxide was formed?
(c) How many atoms of oxygen reacted?
(d) Explain, with reference to collision theory, how heating up the reaction mixture would increase the rate of this reaction.
(e) Identify two other ways to increase the rate of this reaction.
Balance the following half-equations by adding coefficients and electrons, and combine them to form a balanced ionic equation.
| C2O42-(aq) | → | CO2(g) |
| Co3+(aq) | → | Co2+(aq) |
Commonly asked exam questions on Module 4 Drivers of Reactions are:
In a calorimetry experiment to determine the enthalpy of solution of lithium hydroxide, the following data were collected:
| Mass of lithium hydroxide | 5.73 g |
| Mass of water | 265.1 g |
| Initial temperature of water | 17.5 °C |
| Final temperature of water | 21.6 °C |
What is the experimentally determined value of ΔHsoln? The specific heat capacity of the solution is 4.18 x 103 J kg-1 K-1.
(a) − 4.54 kJ mol-1
(b) − 19.4 kJ mol-1
(c) − 4.64 kJ mol-1
(d) − 19.0 kJ mol-1
Given the following data:
| N2(g) + 3H2(g) | → | 2NH3(g) | ΔH = − 115 kJ mol-1 |
| 2NH3(g) + 4H2O(l) | → | 2NO2(g) + 7H2(g) | ΔH = − 142.5 kJ mol-1 |
| H2O(l) | → | H2(g) + ½O2(g) | ΔH = − 43.7 kJ mol-1 |
What is the enthalpy change for the following reaction?
N2(g) + 2O2(g) → 2NO2(g)
Written by Matrix Science Team
The Matrix Science Team are teachers and tutors with a passion for Science and a dedication to seeing Matrix Students achieving their academic goals.
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