In anticipation to the building of a permanent colony on the moon, scientists are planning to provide a self-sustaining source of oxygen by extracting it out of lunar rocks (which are composed primarily of silica). Thus, both silicon (Si(s)) and oxygen gas (O2(g)) can be produced by the electrolysis of molten silica (SiO2(l)). (Note: in the liquid state, SiO2 can be considered as a mixture of Si4+ and 2 O2- ions) Hint: O2 + 4e- → 2O2-
a. Write both half-reactions involved in this process, identifying the oxidation and reduction half reactions. Also, write the balanced equation describing the global reaction.
Is the overall reaction Si4++2O2- ----> Si + O2?
Si4+ is gaining electrons so it's the cathode and O2 is losing it so it's the anode.
b. How many hours are required to convert 1.00 x 103 kg of SiO2(l) by passing a constant current of 5.00 x 104 A through the melt?
Why are they putting '1.00x103' and '5.00x104', why don't they use a single number? Is there something I am missing here?