A major source of sodium metal is the electrolysis of molten so- dium chloride. What magnitude of current produces 1.0 kg of sodium metal in 1 hour?

Video transcript

Hello everyone today. We are being asked the following question. Magnesium can be acquired by the electoral isis or electrolysis of molten, magnesium chloride, calculate the required current to acquire 650 g of magnesium in a span of two hours. So first you want to write down what this equation where this reaction will look like. So we are going to have our liquid mercury and we're going to add two electrons to it. And in doing so we're going to produce our mercury are magnesium solid. Next we are going to write out the equation or solve for our current. So we're going to take that we have g of magnesium Over two hours and work backwards. So what we want to multiply this by first is the molar mass of magnesium and according to the periodic table, one mole of magnesium is equal to 24.305g. Next we want to multiply by the ratio of moles of magnesium to electrons. So we can say that in one mole Of Magnesium We have two moles of electrons. Next because we were dealing with current, we're gonna have to use Faraday's constant And that's to say that in one mole or one mole of an electron is equal to current. We then need to get rid of our hours and turn that into Minutes so that we can get our units. So we're gonna say that in one hour we have 60 minutes And then we're gonna finally multiply that by a conversion that in one minute we have 60 seconds. And so all of our units are going to cancel out our grams of magnesium, our moles of magnesium, our moles of electrons, Our minutes and our hours. And so we are going to be left with the current of 717 amps or amperes as our unit. And this is going to be our final answer. Overall, I hope that this helped, and until next time.