<p>An electrolyte cell contains molten ZnCl2. The zinc chloride is electrolyzed by passing a current of 3.0 A through the cell for a certain length of time. During this process, 24.5g of Zn are deposited on the cathode.</p>
<p>How do you write the chemical equation for the reaction at the cathode?? And what weight of chlorine gas bubbles are released at the anode?</p>
<p>okay, nvm i found my answer :)))</p>
<p>just in case you need it:
At the cathode, the zinc (Zn++) ions in the melt each receive two electrons and are
reduced to elementary zinc (Zn°). The reaction equation is: Zn+2 + 2e- → Zn°.
Look at the overall equation for the electrolysis: ZnCl2 → Zn + Cl2
So for each atom of zinc we produce one molecule of chlorine gas (Cl2); thus, for
each mole of zinc we produce one mole of molecular chlorine, Cl2.
The atomic weight of zinc is 65.37 and if we produce 24.5 grams of zinc, that is
24.5 divided by 65.37, or 0.3747 mole of zinc. Then we also produce 0.3747 mole
of Cl2, with a molecular weight of 70.914. So we produce 0.3747 mole times 70.914
grams per mole, or 26.57 grams of chlorine gas.
Source(s):
college chemistry</p>