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Test your chemistry knowledge with questions about moles, atomic mass, formulas, percentage composition, limiting reactants, and percentage yield. Improve your understanding of fundamental concepts in Chemistry!

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Choose Your Category

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  1. Choose Your Category The Final Question

  2. The Mole - 100 • The SI base unit used to measure the amount of a substance whose number of particles equals the number of atoms of carbon in exactly 12 grams of carbon-12 The Answer is the mole Back

  3. The Mole - 200 • The number of atoms in a mole of any pure substance is called The Answer is the Avogadro's number Back

  4. The Mole - 300 • What can be said about the atoms in 1 mol Ag and 1 mol Au? The Answer is they contain the same number of atoms. Back

  5. The Mole - 400 • The _______________ in a chemical equation represent the relative number of moles of reactants and products. The Answer is coefficients. Back

  6. The Mole - 500 • In the reaction N2 + 3H2 2NH3, what is the mole ratio of nitrogen to ammonia? • The Answer is 1:2 (order in problem) • Or 2 mol NH3/1 mol N2 • (Moles of N2 were given) Back

  7. Average Atomic Mass and Molar Mass - 100 • Using a periodic table, what is the average atomic mass of zinc? The Answer is 65.4 amu. Back

  8. Average Atomic Mass and Molar Mass - 200 What is 120 g/mol in amu? The Answer is 120 amu. Back

  9. Average Atomic Mass and Molar Mass - 300 The atomic mass of hydrogen is 1.008 amu. This is because there is more than one ____________ of hydrogen. The Answer is isotope. Back

  10. Random Points 600 points

  11. Average Atomic Mass and Molar Mass - 400 • Calculate the molar mass of barium nitrate, Ba(NO3)2. The Answer is 261.35 g/mol. Back

  12. Average Atomic Mass and Molar Mass - 500 • Change 58 grams of water into moles. The Answer is 3.22 moles. (58g x 1mol/18 g) Back

  13. Formulas - 100 • A formula that shows the simplest whole-number ratio of the atoms in a compound is the ________________ ___________. The Answer is empirical formula. Back

  14. Formulas - 200 • The first step in finding the empirical formula from the percentage composition is to assume that you have this many grams? • The Answer is 100 g. Back

  15. Formulas - 300 A compound’s empirical formula is NO2. If the formula mass is 92 amu, what is the molecular formula? The Answer is N2O4 Back

  16. Random Points 500 points

  17. Formulas - 400 A compound contain 79.85% carbon and 20.15 % hydrogen. What is the empirical formula? The Answer is CH3 Back

  18. Formulas - 500 • A compound contains 9.1 % hydrogen, 54.5 % carbon and 36.4 % oxygen. What is the molecular formula if its molar mass is132 amu? The Answer is H12C6O3 Back

  19. Percentage Composition – 100 • The percentage of sulfur in SO2 is about 50%. What is the percentage of oxygen in this compound? The Answer is 50%. Back

  20. Percentage Composition – 200 • Calculate the percentage of sulfur in CuSO4. The Answer is 20.09%. Back

  21. Random Points 300 points

  22. Percentage Composition – 300 • What is the percentage composition of each element in CuCl2? The Answer is 47.3% Cu, 52.7% Cl. Back

  23. Percentage Composition – 400 What is the percentage composition of CF4? The Answer is 13.6% C, 86.4% F Back

  24. Daily Double

  25. Percentage Composition – 500 What is the percentage composition of each element in (NH4)2HPO4? The Answer is 21.2% N, 6.8 % H, 23.5% P, and 48.5% O Back

  26. Limiting Reactants - 100 To determine the limiting reactant in a chemical reaction, one must change each reactant into the ________ product with the ________ units. The Answer is same (and same). Back

  27. Limiting Reactants - 200 A chemical reaction involving substances A and B stops when B is completely used. B is the ___________________. The Answer is limiting reactant Back

  28. Limiting Reactants - 300 All the other reactants besides the limiting reactant are called ____________ reactants The Answer is excess. Back

  29. Limiting Reactants - 400 • The first step in most stoichiometry problems is to _____________. The Answer is convert given quantities to moles. Back

  30. Random Points 800 points

  31. Limiting Reactants - 500 • If 2 moles of each reactant are available for the reaction described by the following equation, SiO2(s) + 3C(s)  SiC(s) + 2CO(g), determine which substance is the limiting reactant by calculating the moles of SiC each of the reactants can produced. The Answer is carbon. Back

  32. Percentage Yield and Error - 100 • What is the ratio of the actual yield to the theoretical yield, multiplied by 100%? The Answer is percentage yield Back

  33. Percentage Yield and Error - 200 • Actual yield must be determined by __________________. The Answer is experiments. Back

  34. Random Points 400 points

  35. Percentage Yield and Error - 300 • For the reaction CH4(g) + 2O2(g)  CO2(g) + 2H2O(g), calculate the percentage yield of carbon dioxide if 1000 g of methane (needed to calculate theoretical) react with excess oxygen to produce 2300 g of carbon dioxide (experimental) . The Answer is 83.6%. Back

  36. Percentage Yield and Error - 400 • What is the percent of error in evaluating the molecular mass of a compound if the experimental value was 69.2 amu and the known value was 75.5 amu? The Answer is 8.3% Back

  37. Random Points 400 points

  38. Percentage Yield and Error - 500 • For the reaction CH4(g) + 2O2(g)  CO2(g) + 2H2O(g), calculate the percentage error of carbon dioxide if 1000 g of methane (needed to calculate theoretical) react with excess oxygen to produce 2300 g of carbon dioxide (experimental). The Answer is 16.4% Back

  39. Vocab - 100 • The proportional relationship between two or more substances during a chemical reaction The Answer is stoichiometry Back

  40. Vocab - 200 • The mass in grams of 1 mol of a substance The Answer is the molar mass Back

  41. Vocab - 300 • The percentage by mass of each element in a compound The Answer is the percentage composition Back

  42. Vocab - 400 • The measured amount of a product of a reaction The Answer is actual yield Back

  43. Vocab - 500 • A chemical formula that shows the number and kinds of atoms in a molecule, but not the arrangement of the atoms The Answer is the molecular formula Back

  44. The Final Question • The final question has to deal with: • Stoichiometry Make your wager and hand it to the teacher

  45. Stoichiometry • How many molecules of hydrogen are produced if 20.0 g of sodium metal react with excess water according to the chemical equation: 2 Na(s) + 2 H2O(l)  2 NaOH(aq) + H2(g)?

  46. And the Answer is: 20.0 x (1 mol/23 g) = 0.87 mol Na x (1 mol H2/2 mol Na) = 0.435 mol H2 x (6.02x1023 molecules/1 mol) = The Answer is 2.62 x 1023

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