Problem: A metal forms the salt MCl 3. Electrolysis of the molten salt with a current of 0.700 A for 6.63 h produced 3.00 g of the metal. What is the molar mass of the metal?

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We’re being asked to determine the molar mass of the metal in MCl3. The problem states that the electrolysis of the molten salt with a current of 0.700 A for 6.63 h produced 3.00 g of the metal.


Recall that the molar mass of a compound is expressed as grams per mole:


Molar Mass = massmole=gmol


We know the mass of the metal, 3.00 g. All we need is to find the moles of the metal from the given electrolysis. The flow for this problem will be like this:


Duration of electrolysis (current applied)  Charge applied (Faraday’s constant)  Moles of electrons (mole-to-mole comparison)  Moles of metal


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Problem Details

A metal forms the salt MCl 3. Electrolysis of the molten salt with a current of 0.700 A for 6.63 h produced 3.00 g of the metal. What is the molar mass of the metal?

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Our tutors have indicated that to solve this problem you will need to apply the Electrolysis of Water & Mixture of Ions concept. If you need more Electrolysis of Water & Mixture of Ions practice, you can also practice Electrolysis of Water & Mixture of Ions practice problems.

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Based on our data, we think this problem is relevant for Professor Grant's class at HUNTER.