লক্ষ্য করুন: এই এন্ট্রির অনুবাদ বর্তমানে মান পর্যালোচনার অধীনে রয়েছে, তাই কিছু বিষয়বস্তু সাময়িকভাবে শুধুমাত্র ইংরেজিতে প্রদর্শিত হচ্ছে।
এই এন্ট্রিটি এখনও আপনার ভাষায় অনুবাদ করা হয়নি, তাই নিচে মূল লেখাটি দেখানো হচ্ছে।
faraday
This term is a specialized unit of measurement used primarily in electrochemistry to quantify the amount of electricity required to react one mole of a monovalent ion. It is named after Michael Faraday, the pioneer of electrolysis, and serves as a constant that bridges the gap between macroscopic electrical measurements and microscopic chemical quantities.
As a unit of measurement, it is typically used in technical, academic, or laboratory settings. While it functions as a countable noun when referring to specific quantities of charge, it is almost exclusively encountered in scientific formulas or formal reports regarding electrochemical cells and Faraday's laws of electrolysis.
Meanings
Examples
One faraday is the amount of electric charge per mole of electrons.
The total charge transferred during the reaction is exactly one faraday.
The constant is often referred to as one faraday in electrochemistry textbooks.
I wonder if the calculation requires the value of one faraday to be precise.
The experiment demonstrated that the charge was equivalent to one faraday.
The experiment demonstrated that the charge was equivalent to one faraday.
We need to calculate the mass of the deposit using one faraday per mole.
The value of one faraday is approximately ninety six thousand four hundred eighty five coulombs.