Chemistry Question

don’t do questions 29 and 30

SCH 4U – Final Exam
29.
Which of the following classes of organic compounds does not contain oxygen?
a. aldehydes
b. amines
c. amino acids
30.
d. ethers
e. amides
The sequence of reactions shown here is best described as which of the following?
1.
2.
3.
a. (1) Dehydration; (2)substitution; (3) hydrogenation
b. (1) Hydrogenation; (2) dehydration; (3) substitution
c. (1) Hydrogenation; (2) substitution; (3) dehydration
d. (1) Substitution; (2) hydrogenation; (3) dehydration
e. (1) Dehydration; (2) hydrogenation; (3) substitution
PART B: COMPLETION (KNOWLEDGE – 14)
Complete each sentence or statement.
1. The shape of boron trihydride, BH3, is _________________________.
2. In an exothermic reaction, the potential energy of the products is
____________________ than the potential energy of the reactants.
3. A system at equilibrium always has forward and reverse reaction rates which are
_______________________.
4. A solution at 25oC with a pOH of 3.45 has a pH of ____________________.
5. When nitric acid is titrated to an end point by lithium hydroxide, two products are
_________________________ and _____________________.
6. The standard reduction potential table lists the
values of half-cell reactions
measured in combination with the ________________ standard half-cell.
7. Write the IUPAC name of the compound produced by this reaction:
SCH 4U – Final Exam
1. __________________________.
PART C: SHORT ANSWER (INQUIRY – 9)
3.
1.
Draw an energy level diagram for arsenic, As.
2.
Explain why CH3F is a polar molecule while CF4 is non-polar.
Using Le Chatelier’s principle, explain what effect, if any the following imposed
changes will have on this equilibrium system.
C2H4 (g)
+
H2 (g)
⇌
C2H6 (g)”
#$”%”─136.4 kJ/mol
i) increase in temperature
ii) increase in pressure
iii) increase in the concentration of ethane gas (C2H6)
SCH 4U – Final Exam
4.
Write an equilibrium equation showing how benzoic acid (C6H5COOH) acts like a
weak acid and identify both pairs of conjugate acid-base partners.
5.
Draw the structures of the following organic compounds.
a) 2,3-dinitrophenol
b) methoxyethane
c) cis-2-hexene
6.
Name the following organic compounds.
a)
______________________
b)
_____________________________________
c)
____________________________
SCH 4U – Final Exam
PART D: PROBLEMS
1.
When 1.2 mol of H2 and 2.4 mol of I2 were placed in a 2.0 L container and allowed
to reach equilibrium, the equilibrium concentration of HI was 0.40 mol/L. Calculate
the equilibrium constant (K).
.(”
/0″1/2342/56″#$o (in kJ/mol) for the combustion of 1 mol of ethanol, C2H5OH(l) with to
form gaseous carbon dioxide and gaseous water using Hess’s Law.
”
”
”
”
”
”
”
”
C (s) + O2 (g)
CO2 (g)
H2 (g) + ½ O2 (g)
H2O (g)
2 C(s) + 3H2 (g) + ½ O2(g)
”
”
C2H5OH (l)
”
“#Hform
-393.5
-241.8
-235.2
b) Based on your results from a), calculate the amount of energy released in the
combustion of 500 g of ethanol.
SCH 4U – Final Exam
3.
When sulfuric acid dissolves in water, a great deal of heat is given off. The enthalpy
change for this process is called the enthalpy of solution. To measure it, 175 g of
water was placed in a coffee-cup calorimeter and chilled to 10.0oC. Then 49.0 g of
pure sulfuric acid (H2SO4(l)) also at 10.0oC, was added, and the mixture was quickly
stirred with a thermometer. The temperature rose rapidly to 14.9oC. Calculate the
energy released during the for the formation of this solution and the enthalpy of
solution (in kilojoules per mole of H2SO4).
Assume that the mass of solution = mass water + sulfuric acid.
Assume that that the specific heat capacity of all solutions is 4.184 J/goC.
4.
Consider the following rate data for this reaction:
NO (g) +
a)
H2 (g)
HNO2 (g)
Experiment NO (mol/L)
H2 (mol/L)
1
2
3
4
5
6
0.004
0.004
0.004
0.001
0.002
0.003
0.001
0.002
0.003
0.004
0.004
0.004
Initial Rate of Reaction
(mol/(L·s))
0.002
0.008
0.018
0.008
0.016
0.024
Determine the rate law equation for this reaction.
SCH 4U – Final Exam
b)
Calculate the rate constant (k) using this data.
c)
What would the initial rate of reaction be if the concentration of both
reactants were both 0.008 mol/L?
5.
Calculate the mass of copper (I) sulfide that will completely dissolve in 1.0 L of
water. The Ksp of Cu2S is 6.0 x 10-37 .
6.
What is the pH of a 0.500 mol/L solution of sodium cyanide (NaCN) if the cyanide
ion has a Kb = 1.61 x 10-5?
SCH 4U – Final Exam
7.
8.
Balance the following redox equation using the oxidation number method.
Be sure to write and identify the oxidation and reduction reactions.
Cl─ (aq)
a) MnO47 (aq)
+
b) Al (s)
NO3- (aq)
a)
+
Mn2+ (aq) + Cl2 (g)
NH3 (aq) +
(acidic solution)
AlO2─ (aq)
(basic solution)
Draw a diagram showing the following electrochemical cell. Label the anode,
cathode, reduction half reaction, oxidation half reaction and direction of
electron and ion movement. Include an ammonium nitrate salt bridge.
Zn(s)
1 M Zn(NO3)2 ║
1.M CuNO3
Cu(s)
SCH 4U – Final Exam
b)
What is the standard cell potential (Eo) of this cell?