I have a lab due where it asks for the chemical reaction which is : Cu(s)+4HNO3(aq)->Cu(NO3)2(aq)+2NO2(g)+2H2O(l)

Question

then theres a chart and it asks for the mass or volume to be used or produced (g or mL) , Molar mass(g/mol) Molarity and diluent (if a solution) and moles used or produced. IDK where to get these answers from ??

Answer 1

The lab is basically asking you to do stoichiometry. You should be able to determine the molar masses by adding the corresponding atomic masses (periodic table) of each element. For instance,

(molecular mass HNO3) = 1(atomic mass H) + 1(atomic mass N) + 3(atomic mass O)

notice that the coefficients in front are simply the subscripts in the molecular formula. I will let you do this for the rest of the molecules involved in the equation.

Now, determine the number of moles of your two reagents:

moles Cu = (0.100 g) / [atomic mass Cu]
moles HNO3 = (6 moles/L)(0.002 L) = 0.012 moles HNO3

Determine which is the limiting reagent by calculating how many moles of HNO3 are needed to react COMPLETELY with all the moles of Cu:

(moles Cu) x [(4 moles HNO3)/(1 mole Cu)] = moles HNO3

If (moles HNO3) > 0.012, HNO3 = limiting reagent
If (moles HNO3) < 0.012, Cu = limiting reagent

Finally, use the limiting reagent and stoichiometry to calculate all the other values. The density of water at STP is 1.00 g/mL.