Well, zinc loses two moles of electrons, and this guy gains two moles of electrons. That means we're dealing with two moles of electrons times our Faradays constant 96,500 approximately Coulombs per mole of electron times our cell voltage or electromotive force 1.1 volt. We see that these guys cancel out and our units are left Coulombs times voltage, which is simply joules. So in the end we get 212,300 joules of work. It's produced is released in the form of moving electrons or moving charge from the anode to the capital from this battery. And this amount of energy can be used to do useful work.