Title | Exam questions kerboodle redox answers |
---|---|
Author | Najma Hussein |
Course | Introduction to Chemistry |
Institution | University of Central Lancashire |
Pages | 3 |
File Size | 235.2 KB |
File Type | |
Total Downloads | 75 |
Total Views | 175 |
a level exam questions kerboodle redox mark scheme....
7 Oxidation, reduction, and redox reactions Exam-style mark scheme
AQA Chemistry Question number
Answer
Marks
1a
3CuS(s) + 8HNO3(aq) → 3CuSO4(aq) + 8NO(g) + 4H2O(l)
1
1b
(+) 5 (+) 2
1
1c
Guidance
1 −
−
4H+ + NO3 + 3e → 2H2O + NO
1
Ignore state symbols. Credit multiples of this equation only. Ignore absence of charge on the electron
1d
S
2−
+ 4H2O → SO4
2−
−
+ 8e + 8H+
1
Ignore state symbols. Credit multiples of this equation only. Ignore absence of charge on the electron.
2ai
–
H2O2 + 2H+ + 2e → 2H2O –
1
–
2 a ii
2I → I 2 +2e
2 a iii
H2O2 + 2H+ + 2I → I2 + 2H2O
2bi
Cl2 + 2e → 2Cl
2 b ii
+1
2 b iii
Cl2 + 2H2O → 2HClO + 2H+ + 2e
1
3ai
MnO2 (+) 4
1
3 a ii
MnO2 + 4H+ + 2e → Mn + 2H2O
1 –
1
–
1
–
1 –
–
2+
1
–
Allow ‘2HI’ in place of 2H+ + 2I
Allow 1 / 1+ / Cl+
Or multiples Ignore state symbols Credit electrons subtracted from RHS Ignore absence of charge on e
3 a iii
Iodide ion(s) is / are oxidised because they have lost electron(s)
3b
2Br → Br2 + 2e
–
+
4H + SO4
2–
– –
+ 2e → SO2 + 2H2O
1
Do not penalise reference to iodine; the mark is for electron loss
1
NOT multiples
1
Ignore state symbols Credit electrons subtracted from incorrect side
OR +
–
2H + H2SO4 + 2e → SO 2 + 2H2O 4a
Oxidation
Ignore absence of charge on e 1
OR Oxidised ONLY 4b
NO2
© Oxford University Press 2015
(+) 4
1
www.oxfordsecondary.co.uk/acknowledgements
This resource sheet may have been changed from the original
1
7 Oxidation, reduction, and redox reactions Exam-style mark scheme
AQA Chemistry Question number
Answer NO3
–
HNO2
Marks
(+) 5
1
(+) 3
1
5ai
Loss (of electrons)
1
5 a ii
Oxidation state of nitrogen is NO is +2
1
Oxidation state of nitrogen in NH4 + is –3
1
I2
1
5 a iii 5bi
–
Cl2 + 2e → 2Cl
–
1
Guidance
Ignore state symbols Allow multiples
5 b ii
SO 2 + 2H2O → SO4
2–
+
–
1
+ 4H + 2e
Ignore state symbols Allow multiples
5 b iii
SO 2 + 2H2O + Cl2 → SO4
2–
–
+ 2Cl + 4H
+
1
Ignore state symbols Allow multiples
5c
Use small quantities of solutions e.g. , 2–5 cm
3
Use a fume cupboard since chlorine and SO2 are toxic 6a
–
2+
1 1
MnO2 + 4H+ + 2e → Mn + 2H 2O
1
OR multiples
An oxidising agent is an electron acceptor OR receives / accepts / gains electrons
1
Ignore state symbols
1
NOT an ‘electron pair acceptor’
MnO2 is the oxidising agent 6b
Formation of SO2 and Br2 (could be in an equation) Balanced equation (several possible equations) 2KBr + 3H2SO 4 → 2KHSO4 + Br2 + SO2 + 2H2O OR
Ignore ‘takes electrons’ or ‘takes away electrons’ 1 1 1
–
1 1
2KBr + 2H2SO 4 → K2SO4 + Br2 + SO 2 + 2H2O 2KBr + Cl2 → 2KCl + Br2 % atom economy of bromine
Br2 = ×100 2KBr + CI2 =
=
2 × 79.9 × 100 238.0 + 71.0
159.8 309.0
Could be ionic equation with or without K+
× 100 = 51.72% OR 51.7% OR 52%
2Br + 6H+ + 3SO4 + SO2 + 2H2O
2–
–
→ Br2 + 2HSO4
(3H2SO4) –
2Br + 4H+ + SO4 2H2O
2–
→ Br2 + SO2 +
(2HBr + H2SO4) Accept HBr and H2SO4 in these equations as shown or mixed variants that balance. Ignore equations for KBr reacting to produce HBr Could be ionic equation with or without K+ –
–
2Br + Cl2 → 2Cl + Br2
One from:
Ignore greater number of significant © Oxford University Press 2015
www.oxfordsecondary.co.uk/acknowledgements
This resource sheet may have been changed from the original
2
7 Oxidation, reduction, and redox reactions Exam-style mark scheme
AQA Chemistry Question number
6c
Answer
Marks
Guidance
•
High atom economy
figures
•
Less waste products
Ignore reference to cost
•
Cl2 is available on a large scale
Ignore reference to yield
•
No SO2 produced
•
Does not use concentrated H 2SO4
•
(Aqueous) KBr or bromide (ion) in seawater
•
Process 3 is simple(st) or easiest to carry out
HBr
–1
1
HBrO
+1
1
Equilibrium will shift to the right
1
OR Favours forward reaction OR Produces more HBrO To oppose the loss of HBrO
1
OR Replaces (or implied) the HBrO (that has been used up)
© Oxford University Press 2015
www.oxfordsecondary.co.uk/acknowledgements
This resource sheet may have been changed from the original
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