Question

I was doing a lab and stared off with 10mL of HNO3 and the mass of copper which was 1.5120g. The question now is:
With initial mass of copper wire being 1.5120g, calculate the volume of (16M) nitric acid that is required to fully react with the copper.
Cu(s)+2HNO3(aq) --> Cu(NO3)2(aq)+NO2(g)+H2O(l)
And to make any deviations between the original that was used in the experiment and what we calculated now.

Answer 1

calculate the moles of copper in 1.51grams. You need twice the moles of acid as moles of copper.
Volume acid in liters=molesacid/molarityacid
= 2*molesCu/molarityacid