Test
Practical Test: Faraday's Law
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Preguntas del test (20)
1Which electrode are connected at anode?
- Acopper
- Bcarbon
- Coxygen
- Dsulphur
2What is the use of the sand paper?
- Ato clean the beaker
- Bto clean up spilled electrolyte
- Cto remove oxide layer on the electrode
- Dto remove dust on the electrode
3Arrange the most applicable steps when weighing the copper.
A) Close the door of analytical balance
B) Record the weight to four decimal places
C) Use TARE button
D) Clean the copper before weighing- AD, C, A, B
- BC, A, B, D
- CC, A, D, B
- DD, B, C, A
4Arrange the following steps in conducting the experiment (Faraday's Law)
A) Set up the electrolytic cell
B) Remove oxide layer on electrode
C) Dry the copper after electrolysis and record the final mass.
D) Start the stopwatch and disconnect the circuit immediately- AD, C, B, A
- BD, C, A, B
- CB, A, C, D
- DB, A, D, C
5If the electrolyte used is CuSO4, carbon is the anode and copper is the electrode, which of the following would be the expected observation?
- Abubble gas evolved at the cathode
- Bbubble gas evolved at the anode
- Ccarbon electrode becomes thicker
- Dbrown solid deposited at anode
6If an ammeter in an electrolytic cell does not shows any reading, what could be wrong?
- AThe wires is not connected properly
- BThe power button is switched on
- CThe analytical balance is not functioning properly
- DThe stopwatch stop ticking
7In the experiment to determine Faraday's Law, electrolytic cell is used. Which of the following is not a relevant precaution steps in this experiment?
- AThe cathode electrode need to dry properly before the final mass is weighed
- BWhen running the electrolysis, both electrodes should not be in contact with each other.
- CThe electrodes used should be cleaned with sand paper properly.
- DThe electrodes need to immerse in the electrolyte fully.
8The theoretical value of Faraday's Law is 96500 C. Choose the correct source of errors at which the experimental value is far from the theoretical value.
I. Inaccuracy in weighing
II. Size of the electrodes
III. Fluctuations in electric current
IV. Colour of the electrolyte- AII & IV
- BI, II, & III
- CI & III
- DAll of the above
9The following statement is true about the experiment to determine Faraday's Law except:
- AThe electrolytic cell is set up using ammeter and power supply.
- BThe electrolyte must be filled to 3/4 volume of the beaker
- CThe time taken for the electrolysis should be recorded using a stopwatch
- DThe electrode used at the cathode should be weighed immediately after the electrolysis is stopped
10All experiment should be conducted with a noble manner. Which of the following is not a good noble value while conducting an experiment to determine Faraday's Law?
- AClean up workplace after the experiment is done
- BIf a hair dryer is used, make sure it was used at appropriate distance to the electrode
- CPut all used sand papers left in the dustbin
- DPour back the electrolyte used in their original flask to avoid wasting
11Why does the ammeter reading fluctuate during electrolysis?
- AThe wires are not connected properly
- BBoth electrodes touch each other
- CBoth electrodes are not immerse in the electrolyte
- DThe negative terminal is connected to anode and the positive terminal is connected to cathode
12What is the function of TARE button on the analytical balance?
- ATo stabilize the reading
- BTo reset the reading to zero display
- CTo hold the mass of the substances displayed
- DTo remove the weight of the door of the analytical balance.
13The following cause could affect the mass of electrode after electrolysis except?
- AThe solid deposited at the bottom of the beaker is not collected
- BThe analytical balance are closed while weighing.
- CThe TARE button is not used.
- DThe electrodes are weighed immediately after electrolysis stopped.
14The following statement is correct for electrolysis involving copper electrode at cathode and carbon electrode at anode in CuSO4 solution
- Acarbon electrode is connected to the positive terminal of the power supply
- Bcarbon electrode is connected to the negative terminal of the power supply
- Ccarbon electrode is connected to the ammeter
- Dcopper electrode is connected to the positive terminal of the power supply
15What should we do if a small amount of copper deposited fell to the bottom of the beaker?
- AIf it is a small amount, we can ignore as the small amount will not affect the final mass.
- BTry to collect the solid using filter paper, dry and add the mass with the mass of the electrode.
- CTry to collect the solid using filter paper, if the mass does not exceed 0.5 g, we should ignore the mass.
- DTry to collect the solid using filter paper, dry and add the mass with mass of the electrode only if it weighs more than 0.5 g.
16Which of the following is the source of errors that could happen in the experiment of electrolytic cell
i. The volume of the electrolyte are not at appropriate meniscus level.
ii. The volume of the electrolytes is not the same as instructed in the procedure.
iii. The electrodes are not cleaned properly
iv. The electrodes are left in contact with each other- Aii. iii and iv
- Bi, iii and iv
- Ciii and iv
- DAll of the above
17During the experiment using CuSO4 solution, copper cathode and carbon anode, how many electrons are gained to deposit 1 mol of solid copper?
- A1
- B2
- C3
- D4
18If 0.0316 g of copper is deposited, the no of moles of copper is [blank_start]0.000497[blank_end] moles. (6 d.p)
- A0.000497
19If 0.00048 moles produced by 90 C of current, calculate the Faradays constant.
Faradays's constant is [blank_start]93 750[blank_end] C.- A93 750
20What is the value of Q if the current is 0.15 A and the time used for the electrolysis is 10 minutes.
Q = [blank_start]90[blank_end] C- A90
Información
- Descripción
- Chemistry Test sobre Practical Test: Faraday's Law, creado por Afiqah Rosali el 18/02/2019.
- Autor
- Afiqah Rosali
- Idioma
- English
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