Moles and Molar Mass
This is the value of Avogadro's number.
What is 6.022 x 1023?
This shows the lowest whole-number ratio of atoms present in a compound.
What is the empirical formula?
This is the number of moles of H2O produced from 8 moles of O2 according to the following reaction:
2 H2 + O2 --> 2 H2O
What is 16 moles?
This is the reactant present in a surplus amount.
What is the excess reactant?
This is the amount of product made when all of the limiting reactant is used up.
What is theoretical yield?
This is why we use moles in chemistry.
What is because we want to quantify number of particles on a realistic scale?
This is the mass percent of nitrogen in NH3.
What is 82.25%?
These are the three conversion factors needed to determine how many particles of C are produced from 100 g of A according to the following reaction: 3 A + 2 B --> C.
What are the molar mass of A, the mole ratio between A and C, and Avogadro's number?
This is the first step you should take when determining limiting and excess reactants.
What is calculate the number of moles of each reactant available?
This is the equation used to calculate percent yield.
What is Percent Yield = (Actual Yield / Theoretical Yield) x 100%?
This is the number of particles in 2.53 moles of a substance.
What is 1.52 x 1024 particles?
This is the molecular formula of a compound with the empirical formula P2O5 and a molar mass of 283.9 g/mol.
What is P4O10?
This is the mass in g of O2 produced from the complete reaction of 1.65 moles of KClO3 according to the following reaction:
2 KClO3 --> 2 KCl + 3 O2
What is 79.2 g O2?
This is the limiting reactant when 3.2 g Al and 5.4 g Cl2 react according to the following equation:
2 Al + 3 Cl2 --> 2 AlCl3
What is Cl2?
This is the percent yield if the theoretical yield was 47.89 g, but only 14.3 g were actually recovered.
What is 29.86%?
This is the molar mass of iron (II) phosphate.
What is 357.49 g/mol?
This is the empirical formula of a compound containing 4.151 g of Al and 3.692 g of O.
What is Al2O3?
This is the mass of water produced from the complete reaction of 32.5 g of C3H8 according to the following reaction:
C3H8 + 5 O2 --> 3 CO2 + 4 H2O
What is 53.13 g H2O?
This is the theoretical yield of XeF6 when 130.0 g Xe and 100.0 g F2 react according to the following equation:
Xe + 3 F2 --> XeF6
What is 215.04 g XeF6?
This is the mass of product actually produced when the theoretical yield is 3.5 g and the percent yield is 64.9%.
What is 2.27 g?
This is the mass in grams of 3.25 x 1024 oxygen molecules.
What is 172.7 g?
This is the empirical formula of a compound with the following percent composition: 65.02% Pt, 9.34% N, 2.02% H, and 23.63% Cl.
What is PtN2H6O2?
This is the mass in grams of Li2SO4 produced when 350 mg of LiCl react completely according to the following reaction:
2 LiCl + H2SO4 --> Li2SO4 + 2 HCl
What is 0.454 g Li2SO4?
This is the amount of excess reactant remaining when 1.00 x 103 g N2 and 2.50 x 103 g H2 react according to the following equation:
N2 + 3 H2 --> 2 NH3
What is 2284.15 g H2?
This is the percent yield when 68.5 g of CO and 8.60 g of H2 react according to the following equation:
CO + 2 H2 --> CH3OH
and 35.7 g of CH3OH is actually obtained.
What is 52.31%?