Respuesta :
Answer: Option (c) is the correct answer.
Explanation:
It is known that relation between charge, current and time is as follows.
Total charge passed = current (A) x time (s)
= [tex]3.86 \times 16.2 \times 60[/tex]
= 3751.92 C
Moles of electrons passed = [tex]\frac{\text{total charge}}{F} [/tex]
= [tex]\frac{3751.92}{96485}[/tex]
= 0.03889 mol
As, the given metal salt is MCl. Therefore, the reduction reaction is as follows.
[tex]M^{+} + e^{-} \rightarrow M [/tex]
Thus, moles of M = moles of electrons = 0.03889 mol
As we known that molar mass is calculated using the formula:
Molar mass of M = [tex]\frac{mass}{moles}[/tex]
= [tex]\frac{1.52}{0.03889}[/tex]
= 39.1 g/mol
We know that potassium is the metal which has molar mass as 39 g/mol.
Thus, we can conclude that the metal is identified as K (potassium).
The current passed for cell in the unit time gives the charge passes to the cell. The metal deposited in the electrolysis is Potassium.
What is electrolysis?
The electrolysis is given as the breaking of the salt for the formation of the ions under the influence of the electric current.
The charge transferred ([tex]Q[/tex]) to the cell in the given time is calculated as:
[tex]Q=\rm current\;\times\;time\\\\\textit Q=3.86\;amp\;\times\;16.2\;\times\;60\;sec\\\\\textit Q=3751.92\;C[/tex]
The moles of sample is given as:
[tex]\rm Moles=\dfrac{Charge}{Faraday} \\\\Moles=\dfrac{3751.92}{96,485} \\\\Moles=0.03889\;mol[/tex]
The mass of sample deposited is 1.5 grams, the molar mass of the sample is calculated as:
[tex]\rm Molar\;mass=\dfrac{mass}{moles} \\\\Molar\;mass=\dfrac{1.52}{0.03889}\\\\ Molar\;mass=39.1\;g/mol[/tex]
The molar mass of the compound is 39.1 g/mol. The element with molar mass 39.1 g/mol is Potassium.
Learn more about electrolysis, here:
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