Review of Stoichiometry

Full Book Quiz

1. Which of the following are chemically engineered products?

2. A mole is a measure of:

3. True or False: Only at STP will 1 mole of substance contain 6.02×1023 particles.

4. How many inches are there in 18 yards?

5. How many atoms are there in 3 moles of H2O?

6. A mole ratio is:

7. Given the following balanced equation: N2 +3H2→2NH3 Which of these is an INCORRECT mole ratio?

8. 4NH3(g) + 6NO(g)→5N2(g) + 6H2O(g) How many moles of each reactant were there if 13.7 moles of N2(g) is produced?

9. NaCl, Cl2, C2H6O2: Which has the greatest GFM?

10. What is the GFM of Ca3(PO4)2?

11. What is the mass of 2 moles of H2S?

12. What does STP stand for and what are its conditions?

13. If I have 1 mole of H2O, how many L is that?

14. What is the first step in solving a problem in stoichiometry?

15. Ammonium nitrate decomposes according to the following equation: NH4NO3→N2 + H2O + O2 Given that you start with 8 moles of NH4NO3, how much O2 will be produced? (Assume ideal conditions)

16. 2Al +3Cl2→2AlCl3 When 0.8 kg grams of aluminum is reacted with excess chlorine gas, how many formula units of AlCl3 are produced?

17. Sb2S3(s) + 3Fe(s)→2Sb(s) + 3FeS(s) If 3.87×1023 particles of Sb2S3(s) are reacted with excess Fe(s), what mass of FeS(s) is produced?

18. CO(g) +2H2(g)→CH3OH(g) At STP, what volume of H2(g) is needed to react completely with 8.02×1023 molecules of CO(g)?

19. 4Al +4O2→2Al2O3 13.2 moles of Al reacts completely with excess O2, how much 2Al2O3 is produced?

20. SiO2(s) + 3C(s)→SiC(s) + 2CO(g) At STP, how many kg of SiO2(s) reacted if 680 mL of CO(g) were produced?

21. At STP, which is equivalent to 1 mole?

22. I combine 75 L of hydrogen gas with excess iodine at STP. The resulting reaction is as follows: H2 + I2→2HI How many HI particles are produced?

23. You have 4 moles O2 and 2 moles of FeS2 and are given the following balanced equation: 4FeS2 + 11O2→2Fe2O3 +8SO2 Which reactant is the limiting reagent?

24. Li3N(s) +3H2O(l)→NH3(g) + 3LiOH(aq) How many mL of NH3(g) are produced at STP when 7.88×1024 molecules of water reacts with 120 grams of Li3N(s)?

25. The following equation is balanced: CaCO3 +2HCl→CaCl2 + CO2 + H2O Density is measured in grams/Liter. 345 grams of CaCO3 reacts with excess HCl to produce 200 L of CO2. What is the density of the CO2?

26. CaCO3(s) + 176 kJ→CaO(s) + CO2(g) What is the percent yield if 49.6 g of CaCO3(s) produces 13.1 grams of CaO?

27. True or False: A percent yield of 90 % - 100 % is common in chemistry.

28. 2Zn + O2→2ZnO What is the percent yield of this reaction if 14 moles of ZnO are produced from the reaction of 256 grams of O2 with excess Zn?

29. 2KClO3(s)→2KCl(s) + 3O2(g) If the percent yield is 40%, how many atoms of O are produced from 6.02×1023 formula units of KClO3(s)?

30. 2KClO3(s)→2KCl(s) + 3O2(g) At STP, 9.83×1024 formula units of KClO3(s) decompose into KCl and 82 L of O2(g). What is the percent yield?

31. The amount of heat a substance has at a given temperature and pressure is known as:

32. C(s) + O2(g)→CO2(g) + 393.5 kJ What kind of reaction is this?

33. N2(g) + O2(g) + 43.2 kcal→2NO(g) What kind of reaction is this?

34. What is the atomic mass of magnesium-26?

35. 2Mg(s) + O2→2MgO(s) + 288 kcal How much heat is given off when 8.5 grams of magnesium-26 reacts with excess \ O2?

36. CaCO3(s) + 176 kJ→CaO(s) + CO2(g) How much energy is required to decompose 10.4 moles of CaCO3(s)?

37. 2CO2(g) + 43.9 kJ→2CO(g) + O2(g) How many molecules of 2CO2(g) can be decomposed by the addition of 20 kcal of heat energy?

38. SO3(g) + H2O(l)→H2SO4(aq) + 129.6 kJ At STP, if 540 kJ is released, what volume of SO3(g) was originally added?

39. True or False: The state (s,l,g,aq) of all reactants and products MUST be given in an enthalpy reaction.

40. 2Cl(g)→C2 What is the standard heat of formation for the reaction?

41. Which is the correct equation for heat of reaction?

42. 2NO2(g)→2NO(g) + O2 Calculate the change in enthalpy for this equation given the following two heats of formation:

δHfNO2(g) = 33.85 kJ / mole    

δHfNO(g) = 90.37 kJ / mole    

43. 2SO2(g) + O2(g)→2SO3(g) Find the heat of reaction for this equation given the following two heats of formation:

δHfSO2 = -296.8 kJ / mole    

δHfSO3 = -395.7 kJ / mole    

44. 2SO2(g) + O2(g)→2SO3(g) Find the heat of reaction for this equation given you have 4.5 moles of SO2(g), excess oxygen, and the following two heats of formation:

δHfSO2 = -296.8 kJ / mole    

δHfSO3 = -395.7 kJ / mole    

45. I had 1 mole of NaCl and I put it in 2 L of solution. Which of the following is FALSE?

46. 3CaCO3(s) + 2H3PO4(aq)→Ca3(PO4)2(aq) + 3CO2(g) + 3H2O(l) How much 3CaCO3(s) was added if 650 mL of 2.5 M Ca3(PO4)2(aq) was produced?

47. Can the normality of a solution be numerically equivalent to its molarity?

48. I have a 1 N solution of Ca(OH)2 and a 1 M solution of NaCl. Which of the following are equivalent?

49. 2P2O5 +6H2O→4H3PO4 After 0.32 moles of P2O5 is dropped in a beaker of water, 500 mL remains. What is the normality of the resulting solution?

50. 2Na2O2(s) + 2H2O(l)→O2(g) + 4NaOH(aq) After 27.6 grams of Na2O2(s) is dropped into a beaker of water, 80 mL remains. What is the normality of the resulting solution?