Haven’t had much luck finding Unit 3 Chemistry practice questions for your IA1 Data Test?
Well today’s your lucky day, because we’ve got 25 practice questions you can use in preparation for your actual Unit 3 Chemistry Data Test!
You’ll also be able to check your answers after completing these practice questions with our downloadable solutions.
So what are you waiting for? Let’s get started!
Data Set 1
A closed reaction vessel contains nitrogen (0.5M), hydrogen (3.0M) and ammonia (2.0M) at equilibrium:
N2(g)+3H2(g) ⇌ 2NH3(g)
Image sourced fromSocratic Q&A
Question 1 (2 marks)
Deduce what has happened to the equilibrium position,with reference to Le Chatelier’s principle,at T1.
Question 2 (1 mark)
Deduce what has happened to the equilibrium position at T2.
Question 3 (4 marks)
(a) Describe the effect on the equilibrium position of all reactants and products, with reference to Le Chatelier’s principle, if the hydrogen concentration was increased.
(b)描述对平衡的影响状况n, with reference to Le Chatelier’s principle, if the ammonia concentration was increased.
Question 4 (1 mark)
Supposing that the enthalpy for the reaction in Question 1 is∆H= –91kJmol-1, determine whether it is an exothermic or endothermic reaction.
Question 5 (2 marks)
(a) Using the answer from Question 4 to justify, explain what would happen to the equilibrium position of the reactions if the temperature of the system wasincreased.
(b) Using the answer from Question 4 to justify, explain what would happen to the equilibrium position of the reactions if the temperature of the system wasdecreased.
Question 6 (4 marks)
(a) Explain what effectincreasing the pressureinside the system would have on the equilibrium position according to Le Chatelier’s principle.
(b) Explain what effectdecreasing the pressureinside the system would have on the equilibrium position according to Le Chatelier’s principle.
(c) Explain what effectincreasing the volumeinside the system would have on the equilibrium position according to Le Chatelier’s principle.
(d) Explain what effectdecreasing the volumeinside the system would have on the equilibrium position according to Le Chatelier’s principle.
Question 7 (1 mark)
Explain what effect adding a catalyst to the system would have on the equilibrium position according to Le Chatelier’s principle. Give a reason as to why.
Data Set 2
Image sourced fromUniversity of Wisconsin Pressbooks
Question 1 (1 mark)
Investigate Data Set 2 and determine what type of titration it represents (use the terms strong/weak and acid/base).
Question 2 (1 mark)
Determine the pH of the titrant and what number (1-4) on the graph it is represented by.
Question 3 (1 mark)
Determine the pH of the titrand and what number (1-4) on the graph it is represented by.
Question 4 (1 mark)
Determine the pH of the half-equivalence point and what number (1-4) on the graph it is represented by.
Question 5 (1 mark)
确定等效p的pH值oint and what number (1-4) on the graph it is represented by.
Question 6 (3 marks)
Distinguish between the half-equivalence point and equivalence point in terms of the pH and volume of the titrant.
Question 7 (3 marks)
Distinguish between the equivalence point and end point.
Question 8 (2 marks)
Determine the most appropriate pH indicator for this titration using your Formula and data book. Provide reasoning.
Data Set 3
| Strongest to weakest oxidising agent (1-8) |
Half-reaction | E°(V) |
|---|---|---|
| AuCl4-(aq) + 3e-⇌ Au(s) + 4Cl-(aq) | +1.00 | |
| F2(g) + 2e-⇌ 2F-(aq) | +2.89 | |
| NO3-(aq) + 4H+(aq) + 3e-⇌没有(g) + 2 h2O(l) | +0.96 | |
| Mg2+(aq) + 2e-⇌ Mg(s) | -2.36 | |
| Br2(l) + 2e-⇌ 2Br-(aq) | +1.08 | |
| Ni2+(aq) + 2e-⇌ Ni(s) | -0.24 | |
| Cu2+(aq) + 2e-⇌ Cu(s) | +0.34 | |
| Zn2+(aq) + 2e-⇌ Zn(s) | -0.76 |
Question 1 (2 marks)
According to the standard reduction potentials (E°)provided in Data Set 3, order the half-reactions from strongest to weakest oxidising agent (1-8).
Question 2 (2 marks)
Comparing the following half-reactions, determine which is the strongest oxidant and which is the strongest reductant. Use theE° values to support your answer.
- Half-reaction 1(a): F2(g) + 2e–⇌ 2F–(aq)
- Half-reaction 1(b): Ni2+(aq) + 2e–⇌ Ni(s)
Question 3 (2 marks)
Using theE°values provided, calculate the EMF of a fluoride-nickel galvanic cell.
Question 4 (2 marks)
Comparing the following half-reactions, determine which is the strongest oxidant and which is the strongest reductant. Use theE°values provided to support your answer.
- Half-reaction 2(a): Cu2+(aq) + 2e–⇌ Cu(s)
- Half-reaction 2(b): Zn2+(aq) + 2e–⇌ Zn(s)
Question 5 (2 marks)
Write the oxidation half-reaction for half reaction 2(a).
Question 6 (2 marks)
Determine, in a spontaneous redox reaction between half reaction 2(a) and half reaction 2(b), which of the chemical species will react.
Question 7 (3 marks)
Determine the equation for the balanced chemical reaction between half reaction 2(a) and half reaction 2(b).
Data Set 4
Image sourced fromLibreTexts
Question 1 (2 marks)
Label the buffer region(s).
Question 2 (1 mark)
Explain what the presence of two equivalence points suggests about the acid in this titration.
Question 3 (1 mark)
Provide an example of a common diprotic or polyprotic acid.
Unit 3 Chemistry Data Test Practice Solutions
Click here to download the solutions to the 25 practice questions above!
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