Calculate the mass of a divalent metal produced at the cathode by passing $5 \ A$ current through its salt solution for $100 \ minutes$. (Molar mass of metal $= x \ g/mol$)
- A$\frac{193}{30} x \ g$
- B$\frac{193}{15} x \ g$
- C$\frac{15}{193} x \ g$
- D$\frac{30}{193} x \ g$
Explore More
Similar Questions
The current flowing in a copper voltameter is $3.2 \ A$. The number of copper ions $(Cu^{2+})$ deposited at the cathode per minute is
Easy
View SolutionWhich equation represents Faraday's first law of electrolysis? ($m \rightarrow$ mass,$c \rightarrow$ current,$t \rightarrow$ time,$z \rightarrow$ electrochemical equivalent)
Easy
View SolutionWhat is the $SI$ unit for electrochemical equivalent?
The quantity of electricity in Faraday needed to reduce $1 \ mol$ of $Cr_{2}O_{7}^{2-}$ to $Cr^{3+}$ is ....
The cost of energy required to deposit $1 \ g$ of $Mg$ is $5.00$ rupees. What is the cost to deposit $10 \ g$ of $Al$? (Atomic mass of $Al = 27, Mg = 24$)
Medium
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo