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Year 11 Chemistry Practice Questions for Yearly Exam (Free Chemistry Paper Download)

Are you ready for your Year 11 Chemistry Yearly Exam? Assess your exam-readiness with these commonly asked exam questions.

Year 11 Chemistry Practice Paper for Yearly Exam

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:

  • Module 1: Properties & Structures of Matter
  • Module 2: Introduction to Quantitative Chemistry
  • Module 3: Reactive Chemistry
  • Module 4: Drivers of Reactions

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 at the bottom of this article.

 

Module 1: Properties & Structure of Matter

Commonly asked exam questions on Module 1 Properties & Structures of Matter are:

  • Writing the electron configuration of elements and ions in spdf notation
  • Explaining the physical properties of substances (metallic, ionic, covalent network, covalent molecular)
  • Recalling and explaining periodic trends

 

Question 1  (1 mark)

Which VSEPR shape always results in a polar molecule?

(A) Linear

(B) Trigonal Planar

(C) Tetrahedral

(D) Bent

 

Question 2  (1 mark)

Write the full electronic configuration of a sodium atom.

 

Question 3  (1 mark)

Define the term “electronegativity’.

 

Question 4  (3 marks)

Explain why methane has a lower boiling point than water.

 

 

Module 2: Introduction to Quantitative Chemistry

Commonly asked exam questions on Module 1 Properties & Structures of Matter are:

  • Completing mole calculations
  • Completing limiting reactant calculations
  • Recalling and applying gas laws

 

Question 5  (1 mark)

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 

 

Question 6   (5 marks)

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?

 

 

Module 3: Reactive Chemistry

Commonly asked exam questions on Module 3 Reactive Chemistry are:

  • Classifying and writing equations for different reaction types
  • Selecting and combining half-equations for redox reactions
  • Calculating cell potentials
  • Explaining changes in reaction rates using collision theory

 

 

Question 7  (1 mark)

What is the cell potential under standard conditions?

(A) 0.91 V 

(B) 0.63 V 

(C) 030 V 

(D) 1.68 V 

 

Question 8  (6 marks)

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.

 

Question 9  (2 marks)

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) 

 

 

Module 4: Drivers of Reactions

Commonly asked exam questions on Module 4 Drivers of Reactions are:

  • Calculating reaction enthalpies from calorimetric data
  • Applying Hess’s Law to energy cycles
  • Explaining reaction spontaneity with reference to Gibbs free energy, enthalpy and entropy

 

 

Question 10  (1 mark)

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 

 

Question 11  (1 mark)

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) 

 

Are your ready for your upcoming Year 11 Chemistry Yearly Exam?

Test your depth of knowledge and understanding with our 2-hour Year 11 Chemistry Yearly Exam Practice Paper. Click here to download the Matrix Year 11 Chemistry Practice Paper.

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Written by Michelle Wong

Michelle is the Senior Chemistry Teacher at Matrix Education, and has been tutoring Chemistry and Mathematics for over 15 years.

 

© Matrix Education and www.matrix.edu.au, 2018. Unauthorised use and/or duplication of this material without express and written permission from this site’s author and/or owner is strictly prohibited. Excerpts and links may be used, provided that full and clear credit is given to Matrix Education and www.matrix.edu.au with appropriate and specific direction to the original content.

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