CM-UY 1004 Lecture Notes - Lecture 6: Bromine, Sodium Hydroxide, Sodium Chloride

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limehamster162

20 Sep 2016

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Synthesis (direct combination): element/compound + element/compound one compound. Decomposition (analysis): one compound element/compound + element/compound. Single replacement: element + compound compound + element. Double replacement (exchange of ions): compound + compound compound + compound. Combustion: hydrocarbon + oxygen carbon dioxide + water. Water is always gaseous during a combustion reaction. Exception: 2 ch3oh + o2 4 h2 + 2 co2. Alkali metal + water hydrogen gas + base 2 na + 2 h2o h2 + 2 naoh. Cation: positive charged ion (gets smaller, are metals, and loses electrons) Anion: negative charged ion (gets larger, are nonmetals and gains electrons) Democritus: world is made of empty space and tiny particles atomos . Aristotle: matter is continuous (not made of small particles) false. Boyle: worked with gases (v vs. p) and was the father of modern chemistry. Lavoisier: the law of conservation of mass (matter can"t be created or destroyed, it can only be rearranged)

Related Questions

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

silverclam911

substance	Î H_f Â° (kJ/mol)	Î G_f Â° (kJ/mol)	S Â° (J/molâK)
Aluminum
Al³⁺ (aq)	---	-485.0	---
Al (s)	0	0	28.3
Al₂O₃ (s)	-1675.7	-1582.3	50.9
Al(OH)₃ (s)	---	-1147.25	---
Bromine
Br^â (aq)	---	-104.0	---
Br₂ (l)	0	0	152.2
Br₂ (g)	30.9	3.1	245.5
HBr (g)	-36.3	-53.4	198.7
Calcium
Ca²⁺ (aq)	---	-553.6	---
CaCl₂ (s)	-795.4	---	---
CaO (s)	-634.9	---	---
Ca(OH)₂ (s)	-985.2	---	---
Ca₃(PO₄)₂ (s)	---	-3884.7	---
Carbon
C (s)	0	0	5.7
CCl₄ (g)	-95.7	-64.0	309.4
CCl₄ (l)	-128.2	-68.6	214.4
CCl₄ (s)	-136.8	---	---
CH₄ (g)	-74.6	-50.5	186.3
C₂H₂ (g)	227.4	---	---
C₂H₆ (g)	-84.0	---	---
C₃H₈ (g)	-103.85	-23.4	270.3
C₄H₁₀ (g)	-125.7	-15.7	310.0
C₄H₁₀ (l)	-147.3	-15.0	231.0
C₆H₆ (l)	49.1	124.5	173.4
C₆H₆ (g)	82.9	129.7	269.2
CH₃OH (l)	-239.2	-166.6	126.80
CH₃OH (g)	-201.0	-162.3	239.9
(CH₃)₂(CH₂)₂O (l)	-279.5	-346.74	253.5
C₆H₁₂O₆ (s)	-1237.3	-910.4	212.1
CO (g)	-110.5	-137.2	197.7
CO₂ (g)	-393.5	-394.4	213.8
C₂H₅OH (l)	-277.6	-174.8	160.7
C₂H₅OH (g)	-234.8	-167.9	281.6
HCH₃CO₂ (l)	-484.3	-389.9	159.8
HCH₃CO₂ (s)	-472.8	---	---
HCH₃CO₂ (g)	-432.2	---	283.5
HCN (l)	108.9	125.0	112.8
HCN (g)	135.1	124.7	201.8
CS₂ (s)	93.8	---	---
CS₂ (l)	89.0	64.6	151.3
CS₂ (g)	116.7	67.1	237.8
Chlorine
Cl₂ (g)	0	0	223.1
Cl^â (aq)	---	-131.2	---
HCl (aq)	-167.	---	---
HCl (g)	-92.3	-95.3	186.9
Chromium
CrO₄^2â (aq)	---	-727.8	---
Fluorine
F₂ (g)	0	0	202.8
HF (g)	-273.3	-275.4	173.8
Hydrogen
H₂ (g)	0	0	130.7
Iron
Fe (s)	0	0	27.3
FeCl₃ (s)	-399.5	-334.0	142.3
Fe₂O₃ (s)	-824.2	-742.2	87.4
Lead
Pb²⁺ (aq)	---	-24.4	---
PbBr₂ (s)	-278.7	-261.9	161.5
PbS (s)	-100.4	-98.7	91.2
PbSO₄ (s)	-920.0	-813.0	148.5
Magnesium
MgCl₂ (s)	-641.3	-591.8	89.6
MgO (s)	-601.6	-569.3	27.0
Mercury
Hg (g)	61.4	31.8	175.0
Hg (l)	0	0	75.9
Hg (s)	-2.29	---	---
Hg₂²⁺ (aq)	---	153.5	---
Hg₂Cl₂ (s)	---	-210.7	---
Nitrogen
N₂ (g)	0	0	191.6
N₂H₄ (g)	95.4	159.4	238.5
N₂H₄ (l)	50.6	149.3	121.2
NH₃ (g)	-45.9	-16.4	192.8
NH₃ (l)	-69.54	-26.50	95.09
NH₄NO₃ (s)	-365.6	-183.9	151.1
NO (g)	91.3	87.6	210.8
NO₂ (g)	33.2	51.3	240.1
NOCl (g)	51.7	66.1	261.7
N₂O₄ (g)	11.1	99.8	304.4
HNO₂ (g)	-79.5	---	---
HNO₃ (l)	-174.1	-80.7	155.6
HNO₃ (g)	-133.9	-73.5	266.9
Oxygen
OH^â (aq)	---	-157.2	---
H₂O (l)	-285.8	-237.1	70.0
H₂O (g)	-241.8	-228.6	188.8
O₂ (g)	0	0	205.2
H₂O₂ (l)	-187.8	-120.4	109.6
H₂O₂ (g)	-136.3	-105.6	232.7
Phosphorus
P₄ (s)	0	0	41.
P₄ (g)	58.9	24.4	280.0
PCl₃ (g)	-287.0	-267.8	311.8
PCl₃ (l)	-319.7	-272.3	217.1
PF₅ (g)	-1594.4	-1520.7	300.8
PO₄^3â (aq)	---	-1018.7	---
H₃PO₄ (l)	-1271.7	---	---
H₃PO₄ (s)	-1284.4	-1124.3	110.5
P₄O₁₀ (s)	-2984.	-2675.2	228.9
Potassium
KBr (s)	-393.4	-380.7	95.9
KNO₃ (s)	-492.7	-393.13	132.9
Silver
Ag⁺ (aq)	---	77.1	---
Ag₂CrO₄ (s)	---	-641.8	---
Sodium
NaCl (s)	-411.2	---	---
NaOH (s)	-425.8	---	---
Sulfur
S₈ (s)	0	0	32.0
H₂S (g)	-20.6	---	---
H₂SO₄ (l)	-814.0	---	---
SF₆ (g)	-1220.5	-1116.5	291.5
Tin
Sn (s)	0	0	51.2
SnO₂ (s)	-577.6	-515.8	49.0
Titanium
TiCl₄ (g)	-763.2	-726.3	353.2
TiCl₄ (l)	-804.2	-737.2	252.3
TiO₂ (s)	-944.0	-888.8	50.6

CM-UY 1004 Lecture Notes - Lecture 6: Bromine, Sodium Hydroxide, Sodium Chloride

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