A 0.2500 g sample of a compound known to contain carbon, hydrogen and oxygen undergoes complete combustion to produce 0.3664 g of CO2 and 0.1500 g of H2O. What is the empirical formula of this compound?   a. Calculate the· percentage composition of the compound.   b. Determine the empirical formula.

Which of the following is true about finding the molar mass of potassium sulfate, K₂SO4? A. The molar mass is found by adding the molar mass of potassium (K) to the molar mass of sulfate (SO4). B. The molar mass is found by using Avogadro's number divided by 22.4. C. The molar mass is found by taking 2x the molar mass of potassium (K) plus 1x the molar mass of sulfur (S) plus 4x the molar mass of oxygen (O). D. The molar mass of potassium sulfate is a number between 1 and 10.

III. Molecular Formula 1. A hydrocarbon found in crude oil has an empirical formula of C,H, and an experimentally determined molecular weight of 121 g/mol. What is its molecular formula?

Moles and Chemical Formulas A. Finding the Simplest Formula 43.58 Oi 23 43.81 43.95 1. Mass of empty crucible + cover g 2. Initial appearance of the magnesium 3. Mass of crucible + cover + magnesium 4. Mass of crucible + cover + oxide product Calculations 5. Mass of magnesium 23.43 6. Mass of magnesium compound 7. Mass of oxygen in the product 8. Moles of Mg mole (Show calculations.) 9. Moles of O mole (Show calculations.) 10. Which number of moles (Mg or O) is smaller moles of Mg moles of Mg (rounded to a whole numbe moles O moles of O (rounded to a whole number Formula: Mg subscripts

For the following reaction: N2(g) + H2(g) -------> NH3(g) a. Balance the reaction. b. Determine the number of moles of H2 required to react with 8.50 grams of N2 c. How many moles of NH3 can be formed from 8.50g of N2?

A flask contains 0.200 mol of liquid bromine. Br2. Determine the number of bromine molecules present in the flask

A. Enter the balanced chemical equation for the reaction of solid tin(II) oxide with aqueous hydrogen fluoride to produce aqueous tin(II) fluoride and water.  Express your answer as a chemical equation including phases.   B. Use your balanced chemical equation to calculate the number of moles of HFHF needed to react with 0.600 mole of SnOSnO. Express the number of moles to three significant figures.   C.Use the balanced chemical equation to calculate the grams of HFHF that need to react with 4.30 gg of SnF2SnF2. Express the mass in grams to three significant figures.   D. If 5.00 gg of HFHF completely reacts, what is the theoretical yield of SnF2SnF2? Express the mass in grams to three significant figures.

1. Calculate the Molar Mass (in grams per mole) of: then calculate the number of atoms (or molecules) given moles of moles given molecules. Formula 0₂ HCIO3 Ag₂SO4 C12H22O11 Barium nitrate Molar Mass 16.0 x 2 = 32.0 g/mole moles Given 0.50 mole 1.00 mole 2.50 moles 0.10 moles Molecules .50 x NA 3.01 x 1023 molecules = 1.51 x 1023 molecules

N2(g) + 3 H2(g) → 2 NH3(g) If 0.17 g N2 reacts with 2.5 g H2 in ideal conditions, which statement is true? a. N2 is in excess.b. H2 is in excess.c. Both reactants are completely consumed.d. Not enough information is given to answer the question.

1. A combustion reaction wherein 15.0 g of propane (C3H8) is burned with 75.0 g of oxygen (O2).             a. Determine the limiting reactant.             b. What is the maximum amount of CO2 can you produce?