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13 Dec 2019

1)estimate deltaX rxn of the following reaction from the bond enthalphies.Bond H-H Bond enthalpy (kj/mol)=436Bond Cl-Cl Bond enthalpy (kj/mol)=242Bond H-Cl Bond enthalpy (kj/mol)=431H2+Cl2 arrows 2HCl2) Iron atomic weight 55.8 g/mol forms a bbc crystal with the unit cell length of a 287 pm. How many atoms are present in a unit cell.calculate the density of iron and report it in units g/cm^33)Which of the following molecules is likely to have the highest solubility in water? Explain your answers briefly in terms of intermolecular solvent- solute interactionsEthane CH3-CH3Formaaldehyde CH2=OMethanol CH3-OHChloromethane CH3-Cl

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Hello, I mainly need help with 11 through 15 but I would definitely not mind more help. Thank you in advance

CHM2046 Revicw Assignment Wed Feb 22, 2017 Due: Directions: Write the answers to each problem on the answer sheet prov ded. However, to receive credit must attached the work on separate paper. You may work together on these problems. Be sure to yo include proper u ts in your answer. How many protons, neutrons and electrons are present n each of the following Cr Provide the systematic names for the following: a. CaCO3 b, Cro c. N20 3. Provide the formula for the following: c. iron (II) oxide a. potassium sulfate b. sulfur hexafluoride The density of gold is about 19.32 g/cms. What is the density in units of lbs/ins? 1 kg 2.205 lbs. n 2.54 em. 5. Nicotine is a poisonous, addictive compound found in tobacco. Its form a is C10H14N a. Calculate the molar mass of nicotine b. How many nitrogen atoms are in 1.3 mg of nicotine 6. Ferrocene, first synthesized in 1951, was the first organic iron compound with direct Fe C bonds the combustion analysis of ferrocene, which contains only Fe, C, and H, a 0.9437 g sample produced 2.233 g of CO2 and 0.457 g of H2O. What is the empirical formula of ferrocene? 7, Balance the reactions listed on the answer sheet. Be sure to include "1" as coefficients so each specie has a coefficient 8. One of the first steps in the enrichment of uranium for use in nuclear power plants involves a displacement re between UO2 and aqueous HF to produce the green salt, UF4, and water. a. Write the balance reaction If the reaction in part b resulted in 3481 g of UF4, what is the percent yield of that reaction? 9. For the reaction of aqueous strontium chloride and lithium sulfate, a. write the balanced molecular equation, including correct states of matter b. complete ionic equation, including correct states of matter c. the net ionic, including correct states of matter 10. Automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d 4 g/mL M-62.07 g/mol) and water (d 1.00 g/mL, M 8.02 g/mol). Ethylene glyco the solute and water is the solvent. Assume that the volumes are additive, calculate concentration in the following units a. molarity b. weight/vo me percent c. volume/volume percent Given the following data, calculate the lattice energy of K2O. Show work via Born-Haber cycle or Hess's law Enthalpy of formation of K2O 363.2 kJ/mol Enthalpy of sublimation for K 89.24 kJ/mol ionization energy for K 4.18.8 kJimol Bond dissociation energy of O2 498 kJ/mol electron affinity of O 142 kJ/mol 2'd electron affinity of O 744 J/mol

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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