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WorksheetsExam 4 Review
Total questions: 26
Worksheet time: 13mins
Using solubility rules, select the compound that is least soluble in water.
Pb(NO3)2
(NH4)2CO3
K2SO4
Ca3(PO4)2
Predict the identity of the precipitate formed when solutions of Na2CO3 and CaCl2 are mixed.
Na2CO3
CaCl2
CaCO3
NaCl
Which of the following statements regarding a strong monoprotic acid is NOT correct?
The acid ionizes completely in water
The acid ionizes in water to produce hydronium ions
HNO2 is an example
HCl is an example
Which of the following is a weak acid?
HBr
HI
HF
HCl
Which of the following is a strong base?
Al(OH)3
NH3
Fe(OH)3
RbOH
Which of the following is the conjugate acid of the hydrogen phosphate ion, HPO42– ?
H3PO4
H2PO4 –
HPO42–
PO43–
H3O+
Which one of the following is not a conjugate acid–base pair?
NH3 and NH4+
H3O+ and OH–
H2PO4– and HPO42–
HS– and H2S
Identify the base in the following acid-base reaction:
C5H5N (aq) + HCO3- (aq) → C5H5NH+ (aq) + CO32- (aq) ?
C5H5N (aq)
HCO3- (aq)
C5H5NH+ (aq)
CO32- (aq)
Identify the conjugate base in the following acid-base reaction:
C5H5N (aq) + HCO3- (aq) → C5H5NH+ (aq) + CO32- (aq) ?
C5H5N (aq)
HCO3- (aq)
C5H5NH+ (aq)
CO32- (aq)
What is the oxidation number of phosphorus in the phosphate ion?
-5
-3
+3
+5
Which species is the oxidizing agent in the reaction below?
Cr2O72−(aq) + C2H5OH(aq) → Cr3+(aq) + CO2(g) + H2O(ℓ)?
Cr3+(aq)
Cr2O72−(aq)
CO2(g)
H2O(ℓ)
The following reaction occurs in basic solution:
Zn(s) + NO3−(aq) → Zn(OH)42−(aq) + NH3(aq)
The reducing agent is:
Zn(s)
NO3−(aq)
Zn(OH)42−(aq)
NH3(aq)
How many electrons are being transferred in the net redox reaction?
Zn (s) + 2 MnO2 (s) ⟶ ZnO (s) + Mn2O3 (s)
0
1
2
4
How many electrons are being transferred each time the reaction below happens?
2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)
2
7
14
28
Which of the following is a true statement about this combustion reaction?
2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)
Oxygen is being oxidized and carbon is being reduced.
Hydrogen is being oxidized and carbon is being reduced
Carbon is being oxidized and oxygen is being reduced
Hydrogen is being oxidized and oxygen is being reduced
It is not a redox reaction
Which of these is a redox reaction?
2 NaOH + H2SO4 → Na2SO4 + 2 H2O
2 AgNO3 + Cu → Cu(NO3)2 + 2 Ag
Pb(NO3)2 + 2 KI → PbI2 + 2 KNO3
CaCO3 + 2 HCl → CaCl2 + CO2 + H2O
Dichromate ion in acidic solution converts ethanol, C2H5OH, to CO2 according to the unbalanced equation:
Cr2O72−(aq) + C2H5OH(aq) → Cr3+(aq) + CO2(g) + H2O(ℓ)
The coefficient for H+ in the balanced equation using the smallest integer coefficient is...
8
10
13
16
Rust (mostly Fe2O3) forms on old cars through a series of reactions between iron in the car and oxygen in the atmosphere. Which is the balanced chemical equation showing the formation of Fe2O3 from its elements?
2 Fe + 3 O → Fe2O3
2 Fe + 3 O2 → Fe2O3
4 Fe + 3 O2 → 2 Fe2O3
2 Fe + 3 O → 2 Fe2O3
Rust (mostly Fe2O3) forms on old cars through a series of reactions between iron in the car and oxygen in the atmosphere.
Which element is oxidized and which is reduced during this reaction?
4 Fe + 3 O2 → 2 Fe2O3
Fe is reduced and O2 is oxidized.
Fe is oxidized and O2 is reduced.
Which statement about voltaic cells is not true?
Reduction occurs at the cathode.
Anions move in the salt bridge toward the electrode where oxidation is occurring.
The anode loses mass.
Electrons flow in the external circuit from cathode to anode.
As time passes, what happens to the cathode in a voltaic cell?
Metal ions dissolve into solution.
Metal atoms precipitate (plate) onto it.
Nothing—it stays the same size.
What will the anode be when two half-cells represented by the following half-reactions are combined to make a voltaic cell?
Li+ (aq) + e- → Li (s) ; E° red = -3.05 V
Cu+ (aq) + e- → Cu (s) ; E° red = +0.521 V
Li(s)
Cu(s)
Li+(aq)
Cu+(aq)
What is the standard cell potential for a voltaic cell given the cell potentials for the following two half-reactions?
Cu3+ (aq) + e- →Cu2+ (aq) ; E° red = +2.40 V
Au3+ (aq) + 3e- → Au (s) ; E° red = +1.40 V
1.00 V
3.80 V
1.80 V
-1.00 V
If the standard hydrogen electrode (SHE) is a better oxidizing agent than a zinc electrode, which way will the electrons flow in a voltaic cell made from these electrodes?
Toward the zinc electrode through the salt bridge
Toward the SHE through the salt bridge
Toward the zinc electrode through the wire
Toward the SHE through the wire
An electrolytic cell is composed of silver and zinc half-cells. Determine which electrode is the cathode.
Ag+ (aq) + e- → Ag (s) ; E° red = +0.80 V
Zn2+ (aq) + e- → Zn (s) ; E° red = -0.44 V
zinc
silver
Which type of electrochemical cell has a negative change in Gibbs free energy (ΔG°)?
a voltaic cell
an electrolytic cell
Either one can have a negative ΔG°.
Neither one has a negative ΔG°.
