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Molar Relationships

Molar Relationships. The pH of a 0.1 molar aqueous solution of HCl would equal —. A -1 B 1 C 11 D 13. If 3.50 g of H 2 S are used in the above reaction, what will be the theoretical yield of water in grams?. A 0.102 g B 0.185 g C 1.85 g D 185 g.

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Molar Relationships

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  1. Molar Relationships

  2. The pH of a 0.1 molar aqueous solution of HCl would equal — A -1 B 1 C 11 D 13

  3. If 3.50 g of H2S are used in the above reaction, what will be the theoretical yield of water in grams? A 0.102 g B 0.185 g C 1.85 g D 185 g

  4. If 3.50 g of H2S are used in the above reaction, what will be the theoretical yield of water in grams?

  5. If 3.50 g of H2S are used in the above reaction, what will be the theoretical yield of water in grams? A 0.102 g B 0.185 g C 1.85 g D 185g

  6. Which of the following aqueous solutions will cause litmus paper to turn red? A NaOH B NaCl C HCl D H2O

  7. Which of the following substances is a weakelectrolyte?

  8. A solution contains 225 g of glucose, C6H12O6, dissolved in enough water to make 0.825 L of solution. What is the molarity of the solution? A 0.66 M B 0.97 M C 1.03 M D 1.52 M

  9. A solution contains 225 g of glucose, C6H12O6, dissolved in enough water to make 0.825 L of solution. What is the molarity of the solution?

  10. A solution contains 225 g of glucose, C6H12O6, dissolved in enough water to make 0.825 L of solution. What is the molarity of the solution? A 0.66 M B 0.97 M C 1.03 M D 1.52 M

  11. Carbon disulfide is prepared industrially by reacting carbon with sulfur dioxide according to the above equation. If 5.9 moles of carbon react, how many moles of CS2 are produced? A 0.077 moles B 1.2 moles C 1.5 moles D 30 moles

  12. Carbon disulfide is prepared industrially by reacting carbon with sulfur dioxide according to the above equation. If 5.9 moles of carbon react, how many moles of CS2 are produced?

  13. Carbon disulfide is prepared industrially by reacting carbon with sulfur dioxide according to the above equation. If 5.9 moles of carbon react, how many moles of CS2 are produced? A 0.077 moles B 1.2 moles C 1.5 moles D 30 moles

  14. A solution which has a concentration that exceeds its predicted solubility at a certain temperature and pressure would be — A unsaturated B saturated C supersaturated D dilute

  15. How many milliliters of 2.00 M H2SO4 are needed to provide 0.250 mole of H2SO4? A 125 mL B 1.25 x 101 mL C 8.00 x 103 mL D 8.00 mL

  16. How many milliliters of 2.00 M H2SO4 are needed to provide 0.250 mole of H2SO4?

  17. How many milliliters of 2.00 M H2SO4 are needed to provide 0.250 mole of H2SO4? A 125 mL B 1.25 x 101 mL C 8.00 x 103 mL D 8.00 mL

  18. What is the molarity of a solution prepared by dissolving 27.2 g of sodium chloride in enough water to prepare 500.0 mL of solution? A 0.186 M B 0.465 M C 0.930 M D 1.860 M

  19. What is the molarity of a solution prepared by dissolving 27.2 g of sodium chloride in enough water to prepare 500.0 mL of solution?

  20. What is the molarity of a solution prepared by dissolving 27.2 g of sodium chloride in enough water to prepare 500.0 mL of solution? A 0.186 M B 0.465 M C 0.930 M D 1.860 M

  21. When copper reacts with silver nitrate according to the equation, the number of grams of copper required to produce 432 grams of silver is — A 31.5 g B 127 g C 216 g D 252 g

  22. When copper reacts with silver nitrate according to the equation, the number of grams of copper required to produce 432 grams of silver is —

  23. When copper reacts with silver nitrate according to the equation, the number of grams of copper required to produce 432 grams of silver is — A 31.5 g B 127 g C 216 g D 252 g

  24. What is the final concentration if 50.0 mL of a 2.00 M solution are diluted to 500.0 mL? A 0.100 M B 0.200 M C 0.400 M D 1.00 M

  25. What is the final concentration if 50.0 mL of a 2.00 M solution are diluted to 500.0 mL?

  26. What is the final concentration if 50.0 mL of a 2.00 M solution are diluted to 500.0 mL?

  27. What is the final concentration if 50.0 mL of a 2.00 M solution are diluted to 500.0 mL? A 0.100 M B 0.200 M C 0.400 M D 1.00 M

  28. The number of grams of oxygen required for the complete combustion of 4.00 grams of methane (CH4) is — A 4.00 g B 8.00 g C 16.0 g D 32.0 g

  29. The number of grams of oxygen required for the complete combustion of 4.00 grams of methane (CH4) is —

  30. The number of grams of oxygen required for the complete combustion of 4.00 grams of methane (CH4) is — A 4.00 g B 8.00 g C 16.0 g D 32.0 g

  31. Zn + 2HCl → ZnCl2 + H2If 0.600 gram of zinc is used, what is the amount of zinc chloride that is produced in the above reaction? A 0.125 gram B 1.25 grams C 12.5 grams D 0.018 gram

  32. Zn + 2HCl → ZnCl2 + H2If 0.600 gram of zinc is used, what is the amount of zinc chloride that is produced in the above reaction?

  33. Zn + 2HCl → ZnCl2 + H2If 0.600 gram of zinc is used, what is the amount of zinc chloride that is produced in the above reaction? A 0.125 gram B 1.25 grams C 12.5 grams D 0.018 gram

  34. Four aqueous solutions and their concentrations are shown in the above illustration. Which of the solutions is most likely to be the strongest conductor of electricity? A. I B. II C. III D. IV

  35. I 2 x .5 or 1M II 2 x 1.5 or 3M III 1 x .5 or .5M IV 1 x 1.5 or 1.5 M

  36. Four aqueous solutions and their concentrations are shown in the above illustration. Which of the solutions is most likely to be the strongest conductor of electricity? A. I B. II C. III D. IV

  37. In the reaction 2SO2 (g) + O2 (g) 2SO3 (g), which change would cause the greatest increase in the concentration of SO3? A Decrease the concentration of SO2 B Decrease the concentration of O2 C Increase the concentration of SO2 D Increase the concentration of O2

  38. 2H2(g) + 02(g)  2H2O(g)How many liters of oxygen are requiredto produce 2 liters of water at STP? A 1 B 2 C 3 D 4

  39. 2H2(g) + 02(g)  2H2O(g)How many liters of oxygen are requiredto produce 2 liters of water at STP?

  40. 2H2(g) + 02(g)  2H2O(g)How many liters of oxygen are requiredto produce 2 liters of water at STP? A 1 B 2 C 3 D 4

  41. The molar volume of an ideal gas in liters at STP is — A 6.02 x 1023 L B 11.2 L C 22.4 L D 0.0821 L

  42. What is the density of carbon dioxide at STP? A 1.96 g/L B 22.0 g/ C 46.0 g/L D 5.09 x 10-1 g/L

  43. What is the density of carbon dioxide at STP? Carbon Dioxide is CO2 Mass CO2 = 1(12.0) + 2(16.0) = 44.0g Volume at STP is 22.4L

  44. What is the density of carbon dioxide at STP? A 1.96 g/L B 22.0 g/ C 46.0 g/L D 5.09 x 10-1 g/L

  45. Which of these is about 2 moles? A 2.0 liters (dm3) of H2 B 4.0 grams of H2 C 2.0 x 1023 molecules of H2 D 4.0 kilograms of H2

  46. Which of these is about 2 moles? 2 mol of a gas (STP) = 2(22.4 L) 2 mol = 2(6.02 x 1023) 2 mol = 2(2.0g)

  47. Which of these is about 2 moles? A 2.0 liters (dm3) of H2 B 4.0 grams of H2 C 2.0 x 1023 molecules of H2 D 4.0 kilograms of H2

  48. When magnesium metal (Mg) is burned, it forms MgO. How many moles of oxygen gas (O2) are needed to burn 10 moles of Mg? A 2 B 5 C 10 D 20

  49. When magnesium metal (Mg) is burned, it forms MgO. How many moles of oxygen gas (O2) are needed to burn 10 moles of Mg?

  50. When magnesium metal (Mg) is burned, it forms MgO. How many moles of oxygen gas (O2) are needed to burn 10 moles of Mg? A 2 B 5 C 10 D 20

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