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Station One

Station One. Determine the number of moles in 62.8g of barium acetate. Station Two. How many formula units are in a 61.8 g sample of potassium phosphite?. Station Three. Determine the number of atoms of nitrogen in 14.8 g of ammonium nitrate. Station Four.

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Station One

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  1. Station One Determine the number of moles in 62.8g of barium acetate.

  2. Station Two How many formula units are in a 61.8 g sample of potassium phosphite?

  3. Station Three Determine the number of atoms of nitrogen in 14.8 g of ammonium nitrate.

  4. Station Four Give the empirical formula of the compound C34H68O12.

  5. Station Five Find the mass of a sample of C6H6 gas that occupies 56.3 L at STP.

  6. Station Six At STP, a container is found to contain 54.2 L of CO2. How many moles of carbon dioxide are in the container?

  7. Station Seven Determine the mass in grams of 3.45x10-3 moles of titanium.

  8. Station Eight What mass of calcium metal contains the same number of atoms as 12.16g of magnesium?

  9. Station Nine Calculate the number of molecules present in 2.62x10-6 grams of water.

  10. Station Ten Calculate the number of atoms of Fe in 151 kg of Fe.

  11. Station Eleven Calculate the percentage of cation in ammonium chloride.

  12. Station Twelve Which of the following pairs of compounds have the same empirical formula? • C2H2 and C6H6 • C2H6 and C4H10 • NO2 and N2O4 • C12H10O and C6H5OH

  13. Station Thirteen A compound is known to have a molar mass of 391.5 g/mol. Find the molecular formula of the compound, given the results of analysis of a 310.8g sample that revealed that the sample contains only boron and iodine. The mass of the iodine in the sample is found to be 302.2g.

  14. Station Fourteen Determine the empirical formula of a compound containing 2.16g of Al, 3.85g of S, and 7.68g of O.

  15. Station Fifteen Octane, a compound of hydrogen and carbon, has a molar mass of 114.26g/mol. If one mole of the compound contains 18.17g of hydrogen, what is the molecular formula?

  16. Station Sixteen Find the percentage composition of a compound that contains 1.51g of chromium, 1.13g of K, and 1.62g of O, in a 4.26g sample of the compound.

  17. Station Seventeen A compound having an approximate molar mass of 165-170g has the following percentage composition by mass: carbon, 42.87%, hydrogen, 3.598%, oxygen, 28.55%, and nitrogen. Determine the empirical and molecular formulas of the compound.

  18. Station Eighteen The compound A2O is 63.7% A (a mystery element) and 36.3% oxygen. What is the identify of element A?

  19. Station Nineteen A compound with the empirical formula CH2O was found to have a molar mass between 89 and 91g. What is the molecular formula of the compound?

  20. Station Twenty Calculate the percent by mass of caffeine, C8H10N4O2.

  21. Station Twenty-One If cobalt metal is mixed with excess sulfur and heated strongly, a sulfide compound is produced that contains 55.06% cobalt by mass. Calculate the empirical formula of the sulfide compound.

  22. Station Twenty-Two Calculate the number of O atoms in 4.5L of carbon dioxide.

  23. Station Twenty-Three Give the percent composition of sodium dichromate.

  24. Station Twenty-Four Calculate the mass of 0.75 mol of lithium acetate.

  25. Station 25 Which weighs more - 0.5 mol of oxygen atoms or 4 mol of hydrogen atoms? 0.5 mol O2( 32 g ) = 16 g O2 1 mol 4 mol H2( 2 g ) = 8 g H2 1 mol

  26. Station 26 What mass of cobalt contains the same number of atoms as 57 g of fluorine? 57 g F2( 1 mol F2 ) = 38 g F2

  27. Station 27 Consider a 20.0 g sample of silver metal and a 20.0 g sample of another mystery metal. You are told there are exactly 4 times as many atoms of the mystery metal as of silver metal. Identify the mystery metal.

  28. Station 28 A single molecule of a particular compound has a mass of 4.65 x 10-23g. Which of the following could be this compound? CO H2O NO2 NH3

  29. Station 29 • Calculate the number of grams of iron that contain the same number of atoms as 2.24 g of cobalt.

  30. Station 30 • Consider a 5.0 gram sample of nickel and a 6.0 gram sample of an unknown metal. There are exactly 1/2 as many atoms of the unknown as in the 5.0 gram sample of Ni. What is the unknown metal?

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