Photo AI

An electroplating process uses a solution of chromium(III) sulfate, Cr2(SO4)3, to deposit a thin layer of chromium on the surface of an object - VCE - SSCE Chemistry - Question 19 - 2016 - Paper 1

Question 19

An-electroplating-process-uses-a-solution-of-chromium(III)-sulfate,-Cr2(SO4)3,-to-deposit-a-thin-layer-of-chromium-on-the-surface-of-an-object-VCE-SSCE Chemistry-Question 19-2016-Paper 1.png

An electroplating process uses a solution of chromium(III) sulfate, Cr2(SO4)3, to deposit a thin layer of chromium on the surface of an object. A current of 5.00 A i... show full transcript

Worked Solution & Example Answer:An electroplating process uses a solution of chromium(III) sulfate, Cr2(SO4)3, to deposit a thin layer of chromium on the surface of an object - VCE - SSCE Chemistry - Question 19 - 2016 - Paper 1

Step 1

Calculate the total charge required

96%

114 rated

Answer

To find the total charge ( Q ), we can use the relation that the charge is equal to the number of moles of electrons multiplied by Faraday's constant:

Q = n imes F

Where:

$n$ is the number of moles of chromium, which is 0.0192 mol.
$F$ (Faraday's constant) = 96485 C/mol.

Thus:

Q = 0.0192 ext{ mol} imes 3 ext{ (for Cr)} imes 96485 ext{ C/mol} \ = 0.0192 imes 289955 ext{ C} \ = 5560.96 ext{ C}

Step 2

Determine the time using the current

99%

104 rated

Answer

Using the relation between current, charge, and time:

Q = I imes t

Where:

$I$ is the current (5.00 A),
$t$ is the time in seconds.

Rearranging the formula to find time gives:

t = \frac{Q}{I} = \frac{5560.96 ext{ C}}{5.00 ext{ A}} = 1112.19 ext{ seconds}

Thus, rounding to the nearest whole number, it takes approximately 1110 seconds.

Join the SSCE students using SimpleStudy...

97% of Students

Report Improved Results

98% of Students

Recommend to friends

100,000+

Students Supported

1 Million+

Questions answered

;