Copper wire reacts with silver nitrate to form silver and copper (1) nitrate. This reaction is performed in a beaker in the lab. When the reaction is complete, the chemist pulls the remaining copper wire out of the solution and scrapes off the newly formed silver. Use the
reaction below to determine the limiting reactant.
Cu + AgNO3 → CuNO3 + Aq

See Explanation

Explanation:

From the data given an argument for either reactant as limiting can be presented. The Limiting Reactant is that reactant which when consumed the reaction stops as the remaining reactant does not have any reagent to react with.    

Based on this definition, if one adds a small quantity of AgNO₃ solution to a large quantity of copper wire the interaction will spontaneously react with copper metal undergoing oxidation forming CuNO₃ followed by formation of the reduced form of silver precipitate until all of the AgNO₃ is consumed and the reaction stops. In this case, the AgNO₃ is the limiting reactant and the copper will remain in excess.      

On the other hand and based on this definition of limiting reactant, one can add a small amount of copper wire to a concentrated solution of AgNO₃ and the same reaction will spontaneously occur. However, in this reaction system the reaction would proceed until all of the copper wire is consumed (dissolved) and the reaction stops leaving an excess of unreacted AgNO₃ in solution with CuNO₃ and reduced Ag.

Problems dealing with limiting reactants require specifying the  quantities of each reactant from which identification for the limiting reactant can be specified. One simple way to ID the limiting reactant is to convert all given reactant quantities to moles followed by dividing each by its respective coefficient from the balanced rxn equation. The smaller value will be the limiting reactant.  

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be