Calculating Charge Flows in Chemical Cells: How Much Zinc Reacts per Second?

[pizza1512]

Hi there! Could anyone help me out with this question? Which steps should I take in solving this question?

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 $$Zn^2+$$ ion.

Homework Equations

1. $$Current = \frac{Charge}{time}$$

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$$\times 10^{-19}$$, we obtain the number of electrons being discharged.

What else should I do next?
:shy:

 

[chemisttree]

Hi there! Could anyone help me out with this question? Which steps should I take in solving this question?

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 $$Zn^2+$$ ion.

Homework Equations

1. $$Current = \frac{Charge}{time}$$

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$$\times 10^{-19}$$, we obtain the number of electrons being discharged.

What else should I do next?
:shy:

That would be electrons per second. What would half of that be?

 

[Blueshift5]

your first step in solving this question would be to gather all the necessary information and understand the problem. In this case, you are given the current (0.2A) and the fact that zinc is losing electrons. From this, you can infer that the current is being produced by the flow of electrons from the zinc atoms.

Next, you can use the equation for current (I = Q/t) to calculate the charge flow per second. In this case, the charge flow is 0.2C per second.

Then, you can use the fact that each zinc atom loses 1 electron to become a Zn^2+ ion to determine the number of electrons being discharged per second. This can be done by dividing the charge flow (0.2C) by the charge of one electron (1.6 x 10^-19 C). This will give you the number of electrons being discharged per second.

Finally, to calculate the mass of zinc reacting per second, you can use the molar mass of zinc (65.38 g/mol) and the Avogadro's number (6.022 x 10^23 mol^-1) to convert the number of electrons into moles of zinc per second. Then, you can use the molar mass to convert the moles of zinc into grams of zinc.

In summary, the steps to solve this question would be:
1. Understand the problem and gather all the necessary information
2. Use the equation for current (I = Q/t) to calculate the charge flow per second
3. Determine the number of electrons being discharged per second
4. Use the molar mass of zinc and Avogadro's number to convert the number of electrons into grams of zinc per second.

I hope this helps! Let me know if you have any further questions.