CHEM 1021 Lecture Notes - Lecture 28: Vinyl Chloride, Polyvinyl Chloride, Aluminium Hydroxide

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1 Nov 2016

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How many atoms of aluminum react for every 1. 00 g of aluminum oxide formed: we are given 1. 00 al2o3, unknown: atoms of al. G al) x [(1 mole al2o3)/(101. 90 g al2o3)] x [(2 mole al)/(1 mole al2o3)] x [(6. 022x10^23 al atoms)/(1mole al)] = 1. 18 x 10^22 al atoms. Clicker: using 2h2(g) + o2(g) 2h2o(l), what mass of o2(g) is consumed when 180,000 kg of hydrogen burns? (180,000 kg h2) x [(1000g)/(1kg)] x [(1 mole h2)/(2. 01 gh2)] x [(1 mole o2)/(2 mole h2)] x. [(32. 00 g o2)/(1 mol o2)] = 1. 4 x 10^9 g o2. Strategy to solving these review problems and similar problems on the exam: start with a balanced equation, change to moles for given amount. If needed: use mole ratio to convert from given subtext to what you want to find, never skip this step!!, convert (if needed) to units other than moles for unknown subtext.

Related Questions

3. Write the product formed in the following reactions in the space provided. If the reaction does not take place write NO RXN. Indicate physical states by (s), (l), (g), (aq). Make sure the reaction is balanced! Please write the net ionic equation below.

a. Pb(CH₃CO₂)_2(aq) + Na₂SO₄_(aq) Ã

b. AgNO_3(aq) + NH₄Br_(aq) Ã

4. Balance the following reactions and answer the questions below.

a. Al_(s) + HCl _(aq) Ã AlCl₃ + H₂

What is the element that is oxidized _______________________

What is the element that is reduced _______________________

Which compound is the oxidizing agent ____________________

Which compound is the reducing agent ____________________

b. Na_(s) + FeCl₂ Ã NaCl + Fe

What is the element that is oxidized _______________________

What is the element that is reduced _______________________

Which compound is the oxidizing agent ____________________

Which compound is the reducing agent ____________________

8. Using the unbalanced equation how many grams of lithium nitrate will be needed to make 250g of lithium sulfate, assuming that you have an adequate amount of lead (IV) sulfate to do the reaction.

Pb(SO₄)_2(aq) + LiNO_3(aq) Ã Pb(NO₃)_4(s) + Li₂SO_4(aq)

9. Using the following equation determine how many grams of sodium fluoride can react with 184.4 grams of magnesium.

Mg + NaF₂ Ã MgF₂ + Na

10. Determine how many Oxygen atoms are present in 46.7g of Zr(SO₄)₂

10. Given the following unbalanced equation:

Al₂O_3(aq) + Fe_(s) Ã Fe₂O_3(aq) + Al_(s)

Determine how many grams of Iron (III) Oxide can be formed if 224 grams of aluminum oxide is reacted with iron.

Multiple choice:

10b. Which of the following statement is true about 1 mole of Ca(NO₃)₂?

a. It contains the 6.02 x 10²³ NO₃^- ions.

b. It weighs 146 grams

c. It will most likely dissolve in a bucket of water.

d. It will produce equal number of Ca⁺² and NO₃^- ion in a solution.

10. How many molecules are present in 48.0 grams of oxygen gas? (O₂)

a. 6.02 x10²³ b. 1.81 x10²⁴ c. 9.03 x10²³ d. 1.03x10²⁴

12. If there are 12 moles of carbon in 1 mole of sucrose, C₁₂H₂₂O_11.How many atoms of carbon are there in 1 mole of sucrose?

a. 1 x6.03 x 10²³ b. 12x 6.03 x 10²³ c. 22 x 6.03 x 10²³

13. Determine the oxidation state of oxygen in the compound Cr₂O₃ in the following equation:

Cr₂O_3(s) + 2Al_(s) Ã Cr_(s) + Al₂O_3(s)

-2 b. -6 c. 6 d. 2

16. Determine the oxidation state of Al in the following equation:

Al_(s) + HCl Ã AlCl_3(aq) + H₂

+2 b. 0 c. +3 d. -5

1. Consider the unbalanced equation for the reaction of solid lead with a silver nitrate solution.

_____Pb (s) + ______AgNO3 (ac) â ______Pb(NO3)2 (ac) + _______Ag (s)

a. Balance the equation.

b. How many moles of silver nitrate are required to react completely with 9.3 mol of lead?

c. How many moles of silver, Ag, are formed by the complete reaction of 28.4 mol of Pb?

2. For the following reaction: _____CaO (s) + _____CO2 (g) â _____CaCO3 (s), Calculate how many grams of CaCO3, are formed when 2.4 g of CaO Do they react completely with CO2?

3. For the following reaction: 2 Li (s) + F2 (g) â 2 LiF (s), find the reagent limiting with the amounts of 1.0 mol of Li and 1.0 mol of F2.

4. For the next reaction, determine the limiting reagent, calculate the yield Theoretical product in grams with 5.5 g of Al and 19.8 g of Cl2.

2 Al (s) + 3 Cl2 (g) â 2 AlCl3 (s)

5. Consider the reaction between NiS2 and O2:

2 NiS2 (s) + 5 O2 (g) â 2 NiO (s) + 4 SO2 (g)

When 11.2 g of NiS2 react with 5.43 g of O2, 4.86 g of NiO are obtained. Determine the limiting reagent, the theoretical yield of NiO and the% yield for the reaction.

6. How many atoms of mercury are in 5.8 mol of mercury?

7. Complete the following table:

Element Moles Mass Number of molecules

8. How many grams of sodium are there in 1.00 g of each of the following compounds?

a. Na3PO4

b. NaC7H5O2

c. Na2C6H6O7

9. A sample of 4.78 g of aluminum reacts completely with oxygen to form 6.67 g of aluminum oxide. Use the data to calculate the percent of composition by mass.

10. Citric acid, the compound responsible for the bitter taste in lemons, has the following composition: C - 37.51%

H - 4.40%

O - 58.29%

Calculate the empirical formula.

11. A compound containing phosphorus and oxygen has a molar mass of 219.9 g / mol and an empirical formula of P2O3. Find the molecular formula of compound.

12. It is a term used in chemistry, to describe a system in which a

or more substances, are mixed or dissolved homogeneously in another

substance.

a. Mixture

b. Solution

c. Compound

d. None of the above

13. It is the component that is in a solution, in smaller quantity.

a. Solution

b. Solvent

c. Solvent

d. Soluto

14. It is the component that is in a solution in greater quantity.

a. Solution

b. Solvent

c. Solvent

d. The answers b and c are correct.

15. The quantitative expression of the dissolved amount of solute in a quantity determined solvent is known as:

a. Solution

b. Volume

c. Concentration

d. Stoichiometry

16.Express the moles of solute among the liters of solution

a. Molality

b. Molarity

c. % weight by volume

d. % weight by weight

17.Express the moles of solute between kg of solvent

a. Molarity

b. ppm

c. ppt

d. Molality

18. What is the molarity of a solution prepared by dissolving 7.50 g of nitrate of magnesium, Mg (NO3) 2 in enough water to prepare 25.0 mL of solution?

a. 10.3 M

b. 5.6 M

c. 6.5 M

d. 2.03 M

19. How many grams of sodium chloride, NaCl are needed to prepare 125 mL of 0.037 M NaCl solution

a. 1.021 M

b. 0.268 M

c. 0.201 M

d. 0.500 M

20. Calculate the molality of a solution containing 12.5 g of ethylene glycol (C2H6O2) dissolved in 135 g of water.

21. A solution of ethylene glycol contains 21.2 g of ethylene glycol (C2H6O2) in 85.4 mL of water. Calculate the freezing point and the boiling point of the solution. (Assume the water density is 1.00 g / mL)

22. At what volume should you dilute 75 mL of a 10.0 M solution of H2SO4 to obtain a 1.75 M solution of H2SO4.

HERE IS HOW THIS IS GOING TO WORK! IF YOU ANSWER THE QUESTIONS IWILL GIVE YOU THE 3K POINTS + MORE AFTER I REPOST IT.

2. The amount of heat involved in the synthesis of 1 mole of acompound from its elements, with all substances in their standardstates at 25*C, is called _________.

3. What is a valid unit for specific heat?

4. Use Hess's Law to find the heat of reaction in the examplebelow.

N2O4 (g) ----> 2NO2 (g)

Given that:

N2O4 (g) ----> N2 (g) + 2O2 (g) (Delta H =-9.7kJ)

2NO2 (g) ----> 2O2(g) + N2(g) ( Delta H= -67.7kJ)

5. Use Hess's Law to find the heat of reaction in the examplebelow. (Example doesn't exist btw.)

6. (Delta H) for the formation of rust (Fe2O3) is -826 kJ/mol. Howmuch energy is involved in the formation of 5 grams ofrust?

7. How many kilocalories of heat are required to raise thetemperature of 50g of aluminum from -5*C to 35*C? (Specific heat ofAluminum = 0.21 cal/g*C)

8.Calculate the (Delta H) for this reaction:

Zn(s) + Cu (2+ ion)(aq) ---> Zn(2+) + Cu(s)

(Delta H) for Cu(2+) = +64.4 kJ/Mol; (Delta H) for Zn(2+) = -152.4kJ/mol

9. The following equation shows the reaction that occurs whennitroglycerine explodes.

4C3H5O9N3 ----> 12CO2 + 6N2 + O2 +10H2O + 1725 Kcal

Is this reaction exothermic , endothermic, a combustion reaction ,or a combination reaction?

10. What does it mean for ammonia, (NH3) to have a (Delta H f) =-46 kJ/mol?

(for example: Define heat of formation. What does a negative heatof formation mean? what do the units of kJ/mol mean?)

11. What is the maximum amount of KCl that can dissolve in 500g ofwater?

(solubility of KCl is 34 g/ 100g of water at 20*C)

12.List the ways(operations) that can help make a substancedissolve faster in a solvent?

13. If a crystal added to an aqueous solution causes many particlesto come out of solution, the original solution was (saturate,unsaturated, supersaturated).

14. What is the number of moles of solute in 165 mL of a 0.82 Msolution?

15. What mass of NaCl is needed to make 350 mL of a 1.00 Msolution?

16. Colligative properties depend upon...

17. If one mole of each of these solutes in added to the sameamount of water, which solution has the highest boiling point?(glucose, aluminum sulfate, magnesium acetate, copper (I)chloride)

18. When an acid reacts with a base, what compounds areformed?

19. If the [H+] in a solution is 1x10^(-13) mol/L, what is the[OH-]?

20. If the [OH-] = 1x10^-6 mol/L, what is the pH of thesolution?

21. For a solution to be considered acidic what must be thehydrogen-ion concentration?

22. Which of the following represents a Bronsted-Lowry conjugateacid-base pair?

a) SO3(2-) and SO2 b) CO3(2-) and CO c) H3O and H2 d) NH4(+) and NH3

23. With solutions of "strong" acids and "strong" bases, the word"strong" refers to ...

24. What are the products of Al(OH)3 + H2CO3?

25.What is the concentration of hydrochloric acid if 5.0 mL of acidis neutralized by 30.0 mL of 2.00M sodium hydroxide.

26. At equilibrium, what is the rate of production of reactantscompared with the rate of production of products?

27. What is the equilibrium constant for the following reaction2SO3 ---> 2SO2 + O2

28. How does an increase in pressure affect the following reaction?2SO3 (g) --> 2SO2(g) +O2(g)

29.What stresses would shift the reaction to the right?

2SO3(g) ==> 2SO2(g) + O2(g)

30. The Keq of a reaction 4.9 x 10^(-7). Are products or reactantsfavored at equilibrium?

31. In which of these systems is the entropy decreasing?

a) air escaping from a tire b) snow melting c) a gas condensing d) salt dissolving inwater

32. If an atom is reduced in a redox reaction, what must occur toanother atom in the system?

33. Identify the oxidizing agent in the following reaction: 2Na + S---> Na2S

34. What are transferred in an oxidation -reductionreaction?

35. Give the oxidation number for each atom in KMnO4.

36. Which atom has a change in oxidation number of +4 in thefollowing reaction?

K2Cr2O7 + H2O + S ----> KOH + Cr2O3 +SO2

37. What is the oxidation number of sulfur in each of the following:

a. SO3 c.SO2(2-)

b. Na2SO4 d. S2O4 (2-)

38.Fe(3+) ----> Fe represents oxidation, reduction, orhydrolysis?

39. When the half reactions Br2+ 2e- -----> 2Br- and Na---->e- + Na(+) are combined the balanced redox equation is_____________________ ( WRITE the BALANCED REDOX eq)

40. To balance the oxygen and hydrogen for a redox reaction thattakes place in basic solution, it is necessary to use whichsubstance?

41. What particle completes this nuclear equation? 55/25 Mn + 2/1 H====> _____ +2 1/0 n

42. The half-life of tungsten-182 (182/74 W) is 1.1x10^(17) years.How long would it take for a 376.2 kg sample to decay until only123.0 grams remain?

43. After 3 days, the quantity of certain radioisotope is reducedfrom 13.6 grams to 1.9 grams. Calculate the half-life of theisotope.

44. What is the name of the compound having the formulaC8H18.

45. What is the name of the following compound:

CH3---CH2----CH---CH2--C

I \

CH3 OH

46. What is an isomer? Give an isomer of hexane (C6H14) and drawit's structure.

47. What is the name of the hydrocarbons with double covalentbonds?

48. Draw the stucture for 3-methylbutanoic acid.

49. Draw the structure for methylbenzene?

50. What is the name of the following compound:

CH3----C-----CH3

CH3

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CHEM 1021 Lecture Notes - Lecture 28: Vinyl Chloride, Polyvinyl Chloride, Aluminium Hydroxide

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