In class room , the teacher has explained the quantitative aspects of electrolysis by stating the Faraday's laws of electrolysis. Explain the term electrochemical equivalent.

In a classroom, the teacher has explained the quantitative aspects of electrolysis by stating the Faraday's laws of electrolysis. Explain the term electrochemical equivalent

State the Faraday's laws of electrolysis

In a classroom, the teacher has explained the quantitative aspects of electrolysis by stating the Faraday's laws of electrolysis. Calculate the quantity of electricity required to deposit 0.09 g of aluminium during the following electrode reaction: Al^3 + 3e^(-) to Al ( Al=27u)

Faraday's law of electrolysis are related to

How will you show that Faraday's second law of electrolysis is simply corollary of the first law.

Faraday's first law of electrolysis: Amount of a substance deposited or liberated on respective electrode is directly proportional to the quantity of electricity following through the circuit. W prop Q rArr W= ZQ W= Zit where Z= electrochemical equivalent of the substance. (i) In order to deposit or liberate 1 mole of substance, integeral no of Faradays are required. (ii) In order to deposit one gram equivalent of substance, 1 Faraday electricity is required. Current efficiency = ("Actual yield")/("Theoritical yield") xx 100% For the reaction, 2CH_(3)COO^(-) rarr C_(2)H_(6)(g) + 2CO_(2)(g) + 2e^(-) . If current of 20A is passed for 965sec, volume of liberated gases measured at NTP is found to be 3.36 lit, then calculate current efficiency of the reaction

Teacher explained crystal defects in class room. What are the different types of crystal defects?

State and explain law of multiple proportions with example.

Explain the method of obtaining pure aluminium from alumina by electrolysis. In this process the carbon rods are replaced from time to time. Why?