HERE IS HOW THIS IS GOING TO WORK! IF YOU ANSWER THE QUESTIONS I WILL GIVE YOU T
ID: 780287 • Letter: H
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HERE IS HOW THIS IS GOING TO WORK! IF YOU ANSWER THE QUESTIONS I WILL GIVE YOU THE 3K POINTS + MORE AFTER I REPOST IT.
2. The amount of heat involved in the synthesis of 1 mole of a compound from its elements, with all substances in their standard states 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 example below.
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 example below. (Example doesn't exist btw.)
6. (Delta H) for the formation of rust (Fe2O3) is -826 kJ/mol. How much energy is involved in the formation of 5 grams of rust?
7. How many kilocalories of heat are required to raise the temperature of 50g of aluminum from -5*C to 35*C? (Specific heat of Aluminum = 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+) = -152.4 kJ/mol
9. The following equation shows the reaction that occurs when nitroglycerine 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 heat of formation mean? what do the units of kJ/mol mean?)
11. What is the maximum amount of KCl that can dissolve in 500g of water?
(solubility of KCl is 34 g/ 100g of water at 20*C)
12.List the ways(operations) that can help make a substance dissolve faster in a solvent?
13. If a crystal added to an aqueous solution causes many particles to 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 M solution?
15. What mass of NaCl is needed to make 350 mL of a 1.00 M solution?
16. Colligative properties depend upon...
17. If one mole of each of these solutes in added to the same amount 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 are formed?
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 the solution?
21. For a solution to be considered acidic what must be the hydrogen-ion concentration?
22. Which of the following represents a Bronsted-Lowry conjugate acid-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 acid is neutralized by 30.0 mL of 2.00M sodium hydroxide.
26. At equilibrium, what is the rate of production of reactants compared with the rate of production of products?
27. What is the equilibrium constant for the following reaction 2SO3 ---> 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 reactants favored 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 in water
32. If an atom is reduced in a redox reaction, what must occur to another atom in the system?
33. Identify the oxidizing agent in the following reaction: 2Na + S ---> Na2S
34. What are transferred in an oxidation -reduction reaction?
35. Give the oxidation number for each atom in KMnO4.
36. Which atom has a change in oxidation number of +4 in the following 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, or hydrolysis?
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 that takes place in basic solution, it is necessary to use which substance?
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 only 123.0 grams remain?
43. After 3 days, the quantity of certain radioisotope is reduced from 13.6 grams to 1.9 grams. Calculate the half-life of the isotope.
44. What is the name of the compound having the formula C8H18.
45. What is the name of the following compound:
O
//
CH3---CH2----CH---CH2--C
I
CH3 OH
46. What is an isomer? Give an isomer of hexane (C6H14) and draw it's structure.
47. What is the name of the hydrocarbons with double covalent bonds?
48. Draw the stucture for 3-methylbutanoic acid.
49. Draw the structure for methylbenzene?
50. What is the name of the following compound:
Br
|
CH3----C-----CH3
|
CH3
Explanation / Answer
2) standard heat of formation
3) Joules per gram
4) dH = (-9.7) -(-67.7) = 58 KJ/mol
5) example not given
6) heat involved for 5 gm rust = 5 x ( -826 /159.59) = -25.88,
7) heat = (35-(-5) x 50 x 0.21 = 420 Calories
8) dH rxn = -152.4-(64.4) = -216.8 KJ
9) exothermic reaction
10) heat required for NH3 to form from basic elements like N2 and H2 is 46 KJ/mol,
negative sign indicates heat is released in process,KJ/mol means heat required in KJ per 1 mole NH2 formation
11) 500x(34/100) = 170 gm
12) heating , stirring , etc
13) saturated
14) 0.82 x 0.165 = 0.1353
15) moles of NaCl = 1x0.35 = 0.35 , mass of NaCl = ( 0.35 x58.5) = 20.475 gm
16) number of solute moles
17) aluminium sulphate ( since more ions produced in water)
18) salt and water
19) [OH-] = 10^ -14/10^ -13 = 10^ -1
20) [H+] = 10^ -14/10^ -6 = 10^ -8 , pH = -log(10^-8) = 8
21) [H+] < 10^ -7 ,
22) d
23) strong means they dissociate more they refer to dissociation const
24) Al2O3 + CO2 + H2O
25) M1V1 = M2V2 , M acid =( 2x30/5) = 12 M
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