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Chemistry B Quizzes

Chemistry B Quizzes. The number of atoms or molecules in exactly 1.000 mole of a substance, and is equal to 6.022 x 10 23. The number of atoms or molecules in exactly 1.000 mole of a substance, and is equal to 6.022 x 10 23. Avogrado’s Number.

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Chemistry B Quizzes

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  1. Chemistry B Quizzes

  2. The number of atoms or molecules in exactly 1.000 mole of a substance, and is equal to 6.022 x 1023

  3. The number of atoms or molecules in exactly 1.000 mole of a substance, and is equal to 6.022 x 1023 Avogrado’s Number

  4. atoms of the same element that have different numbers of neutrons, which means that atoms of the same element can have different masses

  5. Atoms of the same element that have different numbers of neutrons, which means that atoms of the same element can have different masses • Isotope

  6. The SI unit for amount of a substance.

  7. The SI unit for amount of a substance. Mole

  8. a chemical formula that shows the simplest ratio of atoms in a compound

  9. a chemical formula that shows the simplest ratio of atoms in a compound Emperical Formula

  10. Which will have the greater number of ions, 1 mol of nickel (II) or 1 mol of copper (I)?

  11. Which will have the greater number of ions, 1 mol of nickel (II) or 1 mol of copper (I)? They will be the same they both are 1 mole, so each would have 6.022 x 1023 ions

  12. Without making a calculation,is 1.11 mol Pt more of less than 6.022 x 1023 atoms?

  13. Without making a calculation,is 1.11 mol Pt more of less than 6.022 x 1023 atoms? It would be more because 1 mole would = 6.022 x 1023, and there are 1.11 moles Pt, so it would be larger than avogadro’s number

  14. Find the mass in grams in 4.30 x 1016 atoms of He, 4.00 g/mol

  15. Find the mass in grams in 4.30 x1016 atoms of He, 4.00 g/mol 4.30 x 1016 atomsHe 1 mol 4.00 g = 2.86 x 10 -7 6.022 x 1023 atoms 1 mol grams He

  16. How many atoms are in two moles of mercury? • 1.204 x 1022 • 1.204 x 1023 • 1.204 x 1024 • 6.022 x 1023

  17. How many atoms are in two moles of mercury? 1.204 x 1024

  18. How many atoms are in a mole of barium chloride, BaCl2? • 6.022 x 1026 • 1.806 x 1024 • 1.204 x 1024 • 6.022 x 1023

  19. How many molecules are in a mole of barium chloride, BaCl2? • 6.022 x 1023

  20. How many grams of cobalt (58.9332 g/mol) are in 4.76 mol of the element?

  21. An element has one isotope with an atomic mass of 27.94 amu. Another isotope has an atomic mass of 28.96 amu. The average atomic mass of the element is 28.02 amu. The isotope that makes up the larger percent of a sample of the element is the isotope with a mass of 27.94 amu 28.96 amu 28.02 amu

  22. An element has one isotope with an atomic mass of 27.94 amu. Another isotope has an atomic mass of 28.96 amu. The average atomic mass of the element is 28.02 amu. The isotope that makes up the larger percent of a sample of the element is the isotope with a mass of 27.94 amu, because it is closes to averageatomic mass of 28.02 amu

  23. What is the molar mass of C6H12O6?

  24. What is the molar mass of C6H12O6? 180.16 g Simply add up the masses from the periodic table

  25. Boron has an isotope with a mass of 10.013 amu that makes up 19.8% of all boron. Its other isotope has a mass of 11.009 amu and makes up 80.2%. What is the average atomic mass of boron.

  26. Boron has an isotope with a mass of 10.013 amu that makes up 19.8% of all boron. Its other isotope has a mass of 11.009 amu and makes up 80.2%. What is the average atomic mass of boron. Boron -10 = (.198) x 10.013 = 1.983 Boron – 11 = (.802) x 11.009 = 8.83 1.983+8.83 =10.81 amu

  27. How many moles of hydrogen are in one mole of C2H6?

  28. How many moles of hydrogen are in one mole of C2H6? 6

  29. How many hydrogen atoms are present in one formula unit of ammonium hydrogen phosphate, (NH4)2HPO4?

  30. How many hydrogen atoms are present in one formula unit of ammonium hydrogen phosphate, (NH4)2HPO4? 8

  31. A compound is 5.94% H and 94.06% O. What is its empirical formula?

  32. A compound is 5.94% H and 94.06% O. What is its empirical formula? 5.94% = 5.94 g H 94.06% = 94.06 g O 5.94g H 1 mol = 5.89 mol H 1.0079g 5.88 94.06g O 1 mole =5.88 mol O 15.999 g 5.88 HO

  33. The first set of calculations in determining an empirical formula from masses of elements produces the subscripts of 1.67 and 1.00. What do you need to do to find the actual subscripts? • Round of both numbers • Round off 1.67, and use 1.00 as it is • Multiply both subscipts by 3 • Multiply both subsripts by 6

  34. The first set of calculations in determining an empirical formula from masses of elements produces the subscripts of 1.67 and 1.00. What do you need to do to find the actual subscripts? • Round off 1.67, and use 1.00 as it is

  35. A compound’s empirical formula is CH. If the formula mass is 79.12 g/mol, what is the molecular formula?

  36. A compound’s empirical formula is CH. If the molar mass is 79.12 g/mol, what is the molecular formula? Formula mass of compound = 79.12 g Molar mass of CH = 13.019 Molar mass of compound = 79.12 =6.07 Molar mass of CH 13.019 Multiply each by 6 to find the molecular formula = C6H6

  37. What is the percentage of chlorine in NaCl?

  38. What is the percentage of chlorine in NaCl? Molar mass of Na = 22.990g Molar mass of Cl = 35.453 g Molar mass of NaCl = 58.443g % of sodium = 22.990/58.443 x 100 = 39% % of chlorine = 35.453/583443 x 100 = 61%

  39. Match each equation with the correct type of reaction. • Ca(ClO3)2 CaCl2 +O2 • CaO + H2O  Ca(OH)2 • C8H18 + O2  CO2 + H2O • Decomposition • Combustion • Synthesis

  40. Match each equation with the correct type of reaction. • Ca(ClO3)2 CaCl2 +O2 • CaO + H2O  Ca(OH)2 • C8H18 + O2  CO2 + H2O • Decomposition (1) • Combustion(3) • Synthesis ( 2)

  41. Balance the following equation: ZnS + O2 ZnO + SO2

  42. Balance the following equation: 2ZnS + 3O2 2ZnO + 2SO2

  43. Match each equation with the correct type of reaction. • AgNO3 + AlCl3 AgCl + Al(NO3)2 • C8H18 + O2  CO2 + H2O • Ca(ClO3)2 CaCl2 +O2 • NaOH + HCl  NaCl + HOH • CaO + H2O  Ca(OH)2 • Ni(ClO3)2  NiCl2 + O2 • Decomposition • Combustion • Synthesis • Single Replacement • Double Replacement – Precipitation • Double Replacement – Acid/Base

  44. Match each equation with the correct type of reaction. • AgNO3 + AlCl3 AgCl + Al(NO3)2 • C8H18 + O2  CO2 + H2O • Ca(ClO3)2 CaCl2 +O2 • NaOH + HCl  NaCl + HOH • CaO + H2O  Ca(OH)2 • Ni(ClO3)2  NiCl2 + O2 • Decomposition (6), (3) • Combustion ( 2) • Synthesis (5) • Single Replacement • Double Replacement – Precipitation (1) • Double Replacement – Acid/Base (4)

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