Question

Cu(s)+HNo3(aq)- Cu(NO3)2(aq)+NO2(g)+H2O 1. which chemical species is the limiting reaggent? 2.which chemical spcies is the non-limiting reagent? 3.Theoretical Volume amount of nitric acid needed used. 4Experimental Volume amount of nitc acid used. 5.Experimental Volume amount of nitric acid remaining.

Answer 1

In order to do this I need the following information:

Amount of any reactant (Cu or acid).

Part 4 and 5, it's data you obtained in experimental, you need to provide that.

Now for the first part, you need to balance the reaction first:

Cu + 4HNO₃ ------> Cu(NO₃)₂ + 2NO₂ + 2H₂O

Now, how you will obtain the limitant reactant?

1. Calculate the number of moles of both Cu and HNO3, using ithe mass of the compound and it's molecular weight:

n = m/MW

In the case of acid, you need the density to change volume to mass:

V = m/d

then conver to moles.

2. Once that you have the moles, look the balance reaction, and see the coefficients of the reactants. That's the theorical moles of both reactants. and do a relation between then:

if 1 mole Cu -----> 4 mole HNO3

then X ---------> Y moles

and solve for Y. If the moles obtained are lower than the moles you previosly calculate, then the Cu would be the limitant reactant and the acid the excess.

and the theorical volume of acid used, you may calculate it if you have the density and mass.

Hope this helps. Post again the question, with the data I said.