CHEM 2311 Study Guide - Heat Capacity, Order Of Merit, Photon

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lemonrat895

17 Feb 2014

School

Northeastern University

Department

Chemistry & Chemical Biology

Course

CHEM 2311

Professor

Stenburg

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Document Summary

What you need: o (observed value), and a (absolute value) What you need: o, and m (mean of values) What you need: da(ave) (average of absolute deviations), and m (mean of values) What you need: m (mass), cp (specific heat capacity), t (change in temp) What it finds: q (heat/ energy transition of a solid, liquid or vapo) What you need: m, hf (heat of fusion) What it finds: q (heat/ energy transition from the solid to liquid phase) What you need: m, hv (heat of vaporization) What it finds: q (heat/ energy transition from the liquid to gas phase) C > f = 5/9 ( f 32) F > c = 9/5 c + 32. K > c = c + 273. 15 k. What you need: temp in c, f, or k. What you need: k (constant with a value of 8. 99x 109 nm2/c2), q1 and q2 (quantity of charge on the two objects), r (distance between the objects)

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

Can someone explain the concepts of 3-12?

3- the boiling point if its nonpolar then the highest in mass, the stronger they are (if the are nonpolar). If they are polar then the smaller the radius and the larger charger the higher the boiling point. (if there is any information to add, please do so).

4- The Clasius Clapeyron equation is used, correct? If so, the equation would be ln(p2/1atm) = -38.56/8.314 x (1/348 - 1/351). For some reason though I am getting .99 at rather than .89

5- For enthlapy of Fusion is q = Enthlapy x moles. Because it is released, then it is exothermic which is negative. So 11.8/10 and being exothermic -1.18

6 and 7 I understand that. No need to explain

8- What equation is to calculate the lattice?

9 - Can you explain how the answer was picked? The options are not there but out of those options, it was (a) AI

10- For the band gap, the lower it goes down the periodic table, the lower the band gap (correct?)

11 - For this problem I have no idea which equation to use and I do not understand the problem.

12 - Same with this question as well.

Everytime I make the graph based off my calculations in the chart it looks like this and I have no idea if it is even close? Please help ! For the questions I just need to understand how to start them and what info is nessiary to do so. very confused.

Data Analysis

Fill in the following table. Look below the table for instructions on how to calculate the values for each row of the table.

a	total volume (L)	0.065L
b	mol S₂O₃^2-_consumed	0.010 mol
c	mol I₃^-_produced	0.015M
d	[S₂O₃^2-] _consumed (M)	0.154M
e	[I₃-] _produced (M)	0.231M

Calculate the final volume of the reaction mixture after the contents of beaker B are added to beaker A. Report your answer in liters.

All S₂O₃^2- is consumed at the end of the reaction. Therefore, the moles of S₂O₃^2- consumed can be calculated using the equation below.
(moles S₂O₃^2-)_consumed = M_stock x (V_stock)

The I₃^- produced in reaction 1 reacts with S₂O₃^2- in reaction 2 as shown.
I₃^- (aq) 2S₂O₃^2- (aq) â 3I^- (aq) S₄O₆^2- (aq)

Therefore, for every mole of I₃^- produced, 2 moles of S₂O₃^2- have reacted.
(moles I₃^-)_produced = (moles S₂O₃^2-)_consumed / 2

[S₂O₃^2-]_consumed = (moles S₂O₃^2-)_consumed / (V_total)

Calculation is the same as d, but using I₃^- instead of S₂O₃^2-.

Fill in the following table. Look below the table for instructions on how to calculate the values for each column of the table.

	a	b	c	d	e	f	g	h	i
Trial	Ît	Î[I₃^-] / Ît (M/s)	log(Î[I₃^-] / Ît)	V 0.2 M KI added (mL)	[I^â]₀(M)	log[I^â]₀	V of 0.2 M (NH₄)S₂O₈ (mL)	[S₂O₈]₀ (M)	log[S₂O₈]₀
1	19	.011	-1.94	25	.077	-1.35	25	.077	-1.11
2	40	.0055	-2.24	25	.077	-1.11	12.5	.038	-1.42
3	85	.0030	-1.84	25	.077	-.1.11	6.25	.019	-1.72
4	42	.0055	-2.26	12.5	.038	-1.42	25	.077	-1.11

Conclusions

If a large amount of heat was released at the start of the reaction, what effect would this have on the rate measurements?

The rate of reaction would be much slower due to its exothermic reaction properties.

Click the box underneath the graph to show the trendline. It will automatically calculate your slope and intercept. Record them below.

Determine the value of q from the graph. Explain your answer.

What is the rate law for the reaction?

For each trial, calculate the rate constant. What is average value of the rate constant?

In this experiment, you assumed that [S₂O₈^2â] >> [S₂O₃^2â]. To find out if this assumption is correct, calculate the ratio of [S₂O₈^2â] / [S₂O₃^2â] for Trial 3. (In Trial 3, the [S₂O₈^2â] was lowest, and therefore the ratio [S₂O₈^2â] / [S₂O₃^2â] is the smallest).

In this experiment, you assumed that only a small amount of S₂O₈^2â was used during the time trial so that the concentration of this reactant did not change appreciably during the course of the reaction. Calculate how much S₂O₈^2â was used in Trial 3 and the percent remaining at the end of the reaction. Was this assumption valid?

CHEM 2311 Study Guide - Heat Capacity, Order Of Merit, Photon

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