We appreciate your visit to In the electrolysis of aluminum chloride 10 A of electricity was passed for 96 5 seconds Calculate the mass in grams of aluminum deposited Given. This page offers clear insights and highlights the essential aspects of the topic. Our goal is to provide a helpful and engaging learning experience. Explore the content and find the answers you need!
Answer :
The mass in gram of aluminum deposited (c) 0.27 g.
Steps
The balanced chemical equation for the electrolysis of aluminum chloride is:
2 AlCl3 → 2 Al + 3 Cl2
From this equation, we can see that 2 moles of Al will be produced for every 2 moles of AlCl3 consumed. The molar mass of Al is 27 g/mol, so the mass of Al produced can be calculated using the following formula:
mass of Al = (current × time × molar mass of Al) / (3 × Faraday's constant)
where the current is in amperes, time is in seconds, Faraday's constant is in coulombs per mole of electrons (F = 96500 C), and the factor of 3 in the denominator comes from the stoichiometry of the reaction.
Plugging in the values given in the problem, we get:
mass of Al = (10 A × 96.5 s × 27 g/mol) / (3 × 96500 C/mol) = 0.27 g
Therefore, the answer is (c) 0.27 g.
learn more about electrolysis here
https://brainly.com/question/12994141
#SPJ1
Thanks for taking the time to read In the electrolysis of aluminum chloride 10 A of electricity was passed for 96 5 seconds Calculate the mass in grams of aluminum deposited Given. We hope the insights shared have been valuable and enhanced your understanding of the topic. Don�t hesitate to browse our website for more informative and engaging content!
- Why do Businesses Exist Why does Starbucks Exist What Service does Starbucks Provide Really what is their product.
- The pattern of numbers below is an arithmetic sequence tex 14 24 34 44 54 ldots tex Which statement describes the recursive function used to..
- Morgan felt the need to streamline Edison Electric What changes did Morgan make.
Rewritten by : Barada
