Which of the following sets of information allows you to obtain the molecular formula of a covalent compound? In each case that allows it, explain how you would proceed (draw a road map and write a Plan for a solution).(a) Number of moles of each type of atom in a given sample of the compound(b) Mass % of each element and the total number of atoms in a molecule of the compound(c) Mass % of each element and the number of atoms of one element in a molecule of the compound(d) Empirical formula and mass % of each element(e) Structural formula

What is the mass in grams of 5.0 * 1020 molecules of aspirin 1C9H8O42? (Hint: Using Avogadro’s number, convert the number of molecules to moles.)

Nitrogen dioxide (NO2) is a major component of urban air pollution. For a samplecontaining 4.000 g NO2, calculate (a) the number of moles of NO2 and (b) the number of molecules of NO2.

1. Explain the term empirical formula and a molecular formula and state how they two differ. 2. Write the empirical formulas of the following: (a) H₂O₂= ; (b) C¿H= ; (c) C6H₁2O6 = ; (d) H₂0 = (e) MgO 12 NaOH g of O 3. Calculate the formula mass (a) NaCl = (b) KOH of Cu 9 = 4. What is the percentage of Ag in AgNO3 5. What is the percentage of C in C12H22O11 (Sucrose, Cane Sugar) 6. Determine in g the mass of 2.5 moles of = 7. How many moles in 0.5 g of Mg; and 0.2 of C₂H₂O₂. ; 8. Determine the number of atoms in 0.8 g 9. A substance was found by analysis to contain 45.57 % of Sn and 54.43 % of Cl. What is the empirical formula of the substance. 10. Ethylene Glycol has a molecular formula (a) Determine its molar mass (b) The percentage compositions of its component's elements (c) The empirical formula of Ethylene Glycol

3) An organic compound contains only C, H, and O. Complete combustion of a 3.185 g sample in an excess of oxygen yields 8.846 g CO2 and 2.507 g H2O. (a) What is the percent composition, by mass, of this compound? (b) What is the empirical formula of the compound? (c) If the molar mass of this compound is 206 g/mol, what is the molecular formula? (C: 12.01 g/mol; H: 1.01 g/mol; O: 16.0 g/mol)

2. An excess of reagent A and 419.15 g of reagent B shown below are reacted together to give product C. (a) Using the full formulae, (NOT line structures), give the equation showing the formation of C. (b) What is the name of product C? (c) How many moles of C will be produced, assuming 98.9% of B is converted? (d) What is the mass of one molecule of C, in grams? HO. он A. B

a) Determine the empirical formula of a compound that contains sulfur and oxygen. It has been determined that 59.95% of the mass of this compound is oxygen. [   b) The molar mass of the compound is determined to be 240.189 g/mol. What is the molecular formula of the compound?

(a How many moles of ammonium ions are in 0.735 g of ammonium carbonate? mol (b) What is the mass, in grams, of 0.0295 mol of iron(III) phosphate? | 9 (c) What is the mass, in grams, of 5.20 x 1023 molecules of aspirin, C3H3O4? (d) What is the molar mass of a particular compound if 0.100 mol weighs 6.64 g? | g/mol

There are various methods for finding the composition of analloy (a metal-like mixture). Show that calculating the mass % of Mg in a magnesium-aluminum alloy (d=2.40 g/cm³) gives thesame answer (within rounding) using each of these methods: (a) a 0.263-g sample of alloy (d=of Mg 1.74 g/cm³; d=of Al 2.70 g/cm³); (b) an identical sample reacting with excess aque-ous HCl forms 1.38x10^-2mol of H₂; (c) an identical samplereacting with excess O₂ forms 0.483 g of oxide.

Determine the: (a) number of grams in 100 grams of calcium hydroxide (Ca=40, O=16, H=1) (b) number of particles in 5 moles of Ca. (Ca: 40 g/mol)