Hi there! Could anyone help me out with this question? Which steps should I take in solving this question?(adsbygoogle = window.adsbygoogle || []).push({});

Chemical cells can produce quite large charge flows for substantial times before their chemicals have all reacted. If zinc is the metal losing electrons under chemical attack, what mass of zinc is reacting per second to produce this current of 0.2A? (remember that each zinc atom loses 1 electrons to become a [tex]Zn^2+[/tex] ion.

2. Relevant equations

- [tex]Current = \frac{Charge}{time}[/tex]

3. The attempt at a solution

So far this is what I have done:

I know that 0.2A = 0.2C/sec. If we divide this by 1.6[tex]\times 10^{-19}[/tex], we obtain the number of electrons being discharged.

What else should I do next?

:shy:

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# Homework Help: Ions in chemical cells

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