3) Based upon your initial mass of Cu, calculate the theoretical mass of Cu,S you could produce

[Tutorial: Empirical formula) This question will walk you through the process of calculating the empirical formula of a 100.0 g sample of an unknown compound from its elemental percent compositions. This problem will be solved via the following sequence of conversions: mass % mass → moles mole ratio → empirical formula. a) Step 1a: When percentages are given, assume that the total mass is 100 grams to determine the mass of each element in grams. (mass % = mass). Then, using the molar masses of each element, convert grams to moles (mass → moles). The unknown compound is 66.6% N by mass. What quantity in moles of nitrogen does a 100.0 gram sample of the unknown compound contain? b) The unknown compound is 28.6% C by mass. What quantity in moles of carbon does a 100.0 gram sample of the unknown compound contain? c) The unknown compound is 4.8% H by mass. What quantity in moles of hydrogen does a 100.0 gram sample of the unknown compound contain

What mass of hydrogen peroxide (H2O2) must decompose to produce 65.88 g of H2O?

Balance these chemical equations. (Use the lowest possible whole number coefficients.) (a)    S8 + O2 → SO3   chemPad Help                   (b)    NaNO3 → NaNO2 + O2   chemPad Help                   (c)    C4H10 + O2 → CO2 + H2O   chemPad Help                   (d)    AgCl2 + H2 → Ag + HCl   chemPad Help                   (e)    Ga + H2SO4 → Ga2(SO4)3 + H2   chemPad Help                   (f)    N2H4 + O2 → H2O2 + N2    chemPad Help