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.

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

To calculate the volume of 16M nitric acid required to fully react with the copper, we'll need to use stoichiometry.

First, let's start by balancing the chemical equation:

Cu(s) + 2HNO3(aq) → Cu(NO3)2(aq) + NO2(g) + H2O(l)

According to the balanced equation, for every 1 mole of copper (Cu), we require 2 moles of nitric acid (HNO3) for a complete reaction.

To determine the moles of copper, we can use the molar mass of copper, which is 63.55 g/mol:

moles of copper = mass of copper / molar mass of copper
= 1.5120 g / 63.55 g/mol
≈ 0.02379 mol

Since the reaction requires 2 moles of nitric acid per mole of copper, we can calculate the moles of nitric acid required:

moles of nitric acid required = 2 * moles of copper
= 2 * 0.02379 mol
= 0.04758 mol

Now, to find the volume of 16M nitric acid required, we need to use the concentration and the molarity equation:

molarity (M) = moles / volume (L)

We can rearrange the equation to solve for volume:

volume (L) = moles / molarity (M)

volume of 16M nitric acid required = 0.04758 mol / 16 mol/L
= 0.002974 L
≈ 2.974 mL

Therefore, approximately 2.974 mL of 16M nitric acid is required to fully react with the copper.

To compare the calculated volume to the original used in the experiment, you need to check the initial volume of nitric acid used and compare it to the calculated volume. If there is a significant deviation between the two volumes, it could indicate errors in the experimental setup or procedure.