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13 Dec 2019

âCompounds with carbon-carbon double bonds, such as ethylene, C2H4, add hydrogen in a reaction called hydrogenation.

C2H4(g)+ H2(g)---> C2H6(g)

Calculate the enthaply change for this reaction, using the following combustion data:

C2H4(g)+ 3O2(g)---> 2H2O(l), (delta) H = -1411 KJ

C2H6(g)+ 7/2O2(g)---> 2CO2(g)+ 3H2O(l), (delta) H = -1560 KJ

H2(g)+ 1/2O2(g)---> H2O(l), (delta) H = -286 KJ

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17 Dec 2019

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1. Calculate the standard change in free energy ?G? (kJ) at 298 K for the reaction C2H4(G)+3o2(G) --> 2CO2(G)+2H2O(G)

a -1310 b. +1180 c. -691 d. +1310 e. -1180

2. The value of E?cell for the reaction 2Cr3+(aq)+6Hg(l) --> 2Cr(s)+3Hg22+(aq) is 1.59 V. Calculate the ?G? (kJ) for the reaction.

a. -921 b. -153 c. -767 d. -460 e. -307

3. What is the value of the equilibrium constant for the cell reaction below at 25 deg C? E?cellÂ=0.61V 2Cr(s)+3Pb2+(aq) <---> 3Pb(s)+2Cr3+(aq)

a. 8.2*10^30 b. 6.7*10^61 c. 9.9*10^99 d. 4.1*10^20 e. 3.3*10^51

4. Which one of the following is not a redox reaction?

a. Na6FeCl8(s)+2Na(l) ---> 8NaCl(s)+Fe(s)

b. Al(OH)3 (aq)+3H+ ---> Al3+(aq)+3H2O(l)

c. CuCl2(aq)+Ni(s) ---> Cu(s)+NiCl2(aq)

d. C6H12O6(s)+6O2(g) ---> 6CO2+6H2O(l)

e. COÂ2(g)+H2(g) ---> CO(g)+ H2O(g)ÂÂÂÂÂÂÂÂ

5. A voltaic cell consists of a Zn/ZN2+ electrode and a Fe/Fe2+ electrode. If [ZN2+] = 0.005M and if [Fe2+] = .0500 M , what is Ecell?

a. .76 b. 0.25 c. 0.45 d. 0.31 e. 0.37

6. The formation constant for the reaction Ag+ (aq)+2NH3(aq) <----> Ag(NH3)2+(aq) is K=1.7*107 at 25 deg C. What is the ?G?(kJ/mol) at this temperature?

a. -23 b. -18 c. -3.5 d. -1.5 e. -41

7. Nitric oxide reacts with chlorine to form NOCL. What is the free energy (kJ) of the reaction at 277 deg C?

a. +144 b.. -41.0 c. -10.3 d. -22.2 e. +41.0

8. Estimate the boiling point (deg C) of phosphoric Acid.

H3PO4(s) <----> HÂ3PO4(l)

?H?f kJ/mol -1279 - -127.17

?G?f kJ/mol -1119 - 1123.6

?S?f J/(k mol) 110.5 - 150.8

a. 42 b. 181 c. 315 d. -92 e. 305

9. Calculate the equilibrium constant, K, for the following reaction at 25?C:

CH4(g)+2H2O(g) <---> Ã CO2(g)+4H2(g) ?G?= -113.6 kJ (please show ICE chart and explain process)

a. 8.2x1019 b. 0.58 c. 0.96 d. 1.4x10-46 e. 1.2x10-20

10. Which of the following results in a decrease in the entropy of the system?

a. O2(g), 300K --> O2(g), 400K b. H2O(s) --> H2O(l) c. N2(g) --> N2(aq) d. NH3(l) --> NH3(g)

e. 2H2O2(g) ---> 2H2O(g)+O2(g)

DearChegg Lifesaver. Here are the requirements:

1.Use given values as stated in questions below.

2.Clearly State Answer

3.(Please) LEAVE A COMMENT if you are currently working on anyproblems.

4.Formany of these problems you will need to use tabulated thermodynamicdata. Use the Information provided after problem 17.

---------------------------------------Questions---------------------------------------------------

1.Write a balanced formation equation for HNO3 at standardconditions. For the answer, enter the sum all of the coefficientsin the balanced equation. (If thisis not an integer, enter it as a decimal, not a fraction.)

2.Calculate ?HÂ° for the following reaction:

SiO2(s)+ 4HF(g) ? SiF4(g) + 2H2O(g)

3.Use heat of formation data to determine ?HÂ° for the reaction:

2NH3(g)? N2(g) + 3H2(g)

4.Calculate the mass of methane that must be burned to provide enoughheat to convert 330.0 g of water at 37.0Â°C into steam at 124.0Â°C.(Assume that the H2Oproduced in the combustion reaction is steam rather than liquidwater.)

5.Acetylene burns in air according to the following equation:

C2H2(g)+ 5/2 O2(g) ? 2 CO2(g) + H2O(g)

with?HÂ° = -1255.8 kJ.

Giventhat ?HfÂ° for CO2(g) = -393.5 kJ/mol and ?HfÂ° for H2O(g) is -241.8kJ/mol, what is ?HfÂ° for C2H2(g)?

6.Given the following data:

HNO3(l)? 1/2N2(g) + 3/2O2(g) + 1/2H2(g) ?HÂ° = 174.1 kJ

2N2O5(g)? 2N2(g) + 5O2(g) ?HÂ° = -28.4 kJ

H2O(l)? H2(g) + 1/2O2(g) ?HÂ° = 285.8 kJ

Calculate?HÂ° for the reaction:

2HNO3(l)? N2O5(g) + H2O(l)

Notethat you should be able to answer this one without needing to useany additional information from the thermo table.

7.Hydrocarbons containing halogens are very useful molecules insynthetic chemistry. Use tabulated thermodynamic data as needed tocalculate ?HfÂ° for the reactionproduct in the equation shown below if ?HÂ° for the reaction is-177.66 kJ.

C2H4(g)+ Cl2(g) ? CH2ClCH2Cl(g)

8.Identify the following statements as true or false. (Use thedrop-down menu and select "True" or "False" for each. You must getall 6 correct.)

Allsystems become more disordered spontaneously.

Both?Ssys and ?Ssurr must equal zero at equilibrium.

Theentropy of the universe is constant; the energy of the universedecreases towards a minimum.

Allspontaneous processes release heat.

Ifa reaction is spontaneous, the reverse reaction is non-spontaneous.

Ifa process decreases the randomness of the particles of a system,the entropy of the system increases.

9.Use tabulated thermodynamic data to calculate ?SÂ° for the reaction:

PbO2(s)+ 2Ni(s) ? Pb(s) + 2NiO(s)

10.Calculate ?SÂ° for the combustion of ethane (C2H6) to form carbondioxide and gaseous water.

11.Urea ((NH2)2CO) can be formed from ammonia and carbon dioxide asshown in the following reaction. The ?HÂ° value for this synthesisis -134.0 kJ. Calculatethe ?HÂ°f for urea.

2NH3(g)+ CO2(g) ? (NH2)2CO(s) + H2O(l)

12.The ?SÂ° value for urea the synthesis reaction above is -424.0 J/K.Calculate SÂ° for urea.

Tries0/99

13.Calculate ?GÂ° for the synthesis of urea under standard conditions(298 K and 1 atm).

Tries0/99

14.Compute the standard free energy change for the following reaction.

O3(g)+ NO(g) ? NO2(g) + O2(g)

Tries0/99

15.The most important commercial process for generating hydrogen gasis the water-gas shift reaction:

CH4(g)+ H2O(g) ? CO(g) + 3H2(g)

Usetabulated thermodynamic data to find ?GÂ° for this reaction at thestandard temperature of 25Â°C.

16.Now calculate ?GÂ°1100 for this process when it occurs at 1100 K.

17.The molar enthalpy of fusion (?HÂ°) of fluorine is 0.260 kJ/mol, andthe molar entropy of fusion (?SÂ°) of fluorine is 4.851 J/mol K.Using this information,estimate the freezing point of fluorine. (You must answer inKelvin.)

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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