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For a question of this nature http://puu.sh/dgvcw/7cb432e4ce.png , would you use the formula F=ma, or the formula F = T(Thurst) - mg(rocket)?

Just to clarify. This is the exact experiment we did. It was a prac exam, so I don't have the results with me. http://puu.sh/d9GSa/3e3e7c3e6e.png

Nope, we didn't notice any bubbling, or metal depositing on the graphite (but then again, we weren't really paying attention to that).

The only observations we were told to take was the reading on the voltmeter. If it helps, we used different metals in the same solution, the higher reading we got was from Magnesium (considering we used Mg, Cu, Zn and Nickel)

In our prac, we also performed an experiment where we used the same metal but different concentrations of the NaCl (0.1 Mol, 1.00 Mol, 0.001 Mol), and we got higher readings the more concentrated the solution was. Would that help with anything?

Is it a possibility that the Zinc was the one being oxidised and chlorine being reduced? Our teacher didn't really tell us much about this experiment

When we did our experiment, we got a positive reading. The graphite was connected to the positive terminal and the zinc to the negative terminal.

Can a non-spontaneous reaction be read off the voltmeter?

If the experiment was like this, with an inert conductor http://community.boredofstudies.org/attachments/239/production-materials/29198d1384568000-galvanic-cell-chem2.4.11.png And one of the electrodes was zinc and the other graphite, and the electrolyte was NaCl (Sodium Chloride), what is...