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WorksheetsChemistry 262 Final Study Guide
Total questions: 67
Worksheet time: 17hrs 45mins
What element is being OXIDIZED in the following redox reaction?
C3H8O2(aq) + K2Cr2O7 (aq) = C3H4O4 (aq) + Cr^3+ (aq)
Cr
H
O
K
C
A voltaic cell ...
Produces electrical current from electricity
Produces electrical current from a spontaneous chemical reaction
Consumes electrical current to drive a spontaneous chemical reaction
Produces electrical current from a non-spontaneous chemical reaction
Consumes electrical current to drive a non-spontaneous chemical reaction
Identify the location of OXIDATION in an electrochemical cell
The socket
The anode
The cathode
The electrode
The salt bridge
Define a salt bridge.
A pathway composed of salt water, that ions pass through
A pathway in which no ions flow
A pathway by which counter-ions can flow between the half-cells without the solution in the half-cell totally mixing.
A pathway between the cathode and anode in which ions are reduced
A pathway between the cathode and anode in which ions are oxidized
Identify a characteristic that does not describe a standard hydrogen electrode.
1 atomosphere
Zinc electrode
Inert platinum electrode
Potential of zero
1 M HCl solution with hydrogen gas
Identify the characteristic of a SPONTANEOUS reaction.
K > 1
Delta G 0 < 0
E Cell 0 > 0
All of the above
None of the above
Which of the following reactions would have the SMALLEST value of K at 298 K?
A + B = C; E Cell 0 = +1.22V
A + 2B = C; E Cell 0 = +0.98V
A + B = 3C; E Cell 0 = +0.15 V
A + B = 2C; E Cell 0 = -0.030V
More information is needed to determine
What is undergoing REDUCTION in the redox reaction represented by the following cell notation?
Pb(s) / Pb^2+(aq) // H^+(aq) / H2(g) / Pt
Pb^2+(aq)
Pb(s)
Pt
H2(g)
H^+(aq)
Which of the following is the STRONGEST reducing agent?
F^ - (aq)
Na(s)
Cd(s)
Fe^2+ (aq)
Fe^3+ (aq)
In which of the following is the WEAKEST oxidizing agent?
K^+ (s)
Cu^+ (s)
Fe^2+ (aq)
Cr^3+ (aq)
Sn^4+ (aq)
Determine which of the following pairs of reactants will result in a spontaneous reaction.
Ag(s) + Ni^2+(aq)
I^ - (aq) + Zn^2+ (aq)
Ba(s) + Mn^2+(aq)
H2(g) + Cd^2+(aq)
All of the above pairs will react
Write the nuclear equation for the ALPHA decay of 90 ^232 Th.
2^4 He + 90^232 Th = 92^236 U
90^232 Th = 2^4 He +88^228 Ra
90^232 Th = -1^0 e + 91^232 Pa
0^1 n + 90^232 Th = 90^233 Th
90^232 Th = +1^0 e + 89^232 Ac
Determine the identity of the daughter nuclide from the positron emission of 6^11 C
7^11 N
7^12 N
6^12 C
5^10 B
5^11 B
Determine the identity of the daughter nuclide from the electron capture by 26^55 Fe.
27^55 Co
27^56 Co
25^54 Mn
25^55 Mn
24^51 Cr
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 degrees Celsius (the equation is unbalanced).
K(s) + I2(s) = K^+ (aq) + I^ - (aq)
K^+(aq) + e^ - = K (s); E 0 = -2.93 V
I2(s) + 2e ^ - = 2I^ - ; E 0 = +0.54 V
-5.32 V
+1.85 V
+3.47 V
+5.32 V
+6.40 V
Use the tabulated half-cell potentials to calculate the ln K for the following balanced redox reaction at 25 degrees Celsius.
2 Al (s) + 3 Mg^2+ (aq) = 2 Al^3+ (aq) + 3 Mg (s)
82.88
165.76
-55.25
-82.88
-167.76
Write a balanced reaction for which the following rate relationships are true.
Rate = -1/2 (Delta [N2O5]/Delta t) = 1/4 (Delta [NO2]/Delta t) = (Delta [O2]/Delta t)
4 NO2 + O2 = 2 N2O5
2 N2O5 = NO2 + 4 O2
1/2 N2O5 = 1/4 NO2 + O2
2 N2O5 = 4 NO2 + O2
1/4 NO2 + O2 = 1/2 N2O5
Given the following balanced equation, determine the rate of reaction with respect to [O2]. If the rate of formation of O2 is 6.94 x 10^ -1 M/s, what is the rate of the loss of O3?
0.231 M/s
2.08 M/s
4.16 M/s
1.04 M/s
0.463 M/s
What are the units of k in the following rate law:
Rate = k [X][Y]^2
1/Ms^2
1/M^3s
M^2s
M^2/s
1/M^2s
Given the following rate law, how does the rate of reaction change if the concentration of X and Y are both doubled?
Rate = k [X]^2[Y]^3
The rate of reaction will increase by a factor of 4
The rate of reaction will increase by a factor of 10
The rate of reaction will increase by a factor of 16
The rate of reaction will increase by a factor of 32
The rate of reaction will remain unchanged
Determine the rate law the value of k for the following reaction using the data provided.
2 No (g) + O2 (g) = 2 NO2 (g)
[NO]i (M) : 0.020, 0.030, 0.060
[O2]i (M) : 0.0055, 0.0110, 0.0055
Initial Rate (M^ -1 s^ -1): 8.55 x 10^ -3, 1.71 x 10^ -2, 3.42 x 10^ -2
Rate = 57 M^ -1 s^ -1 [NO][O2]
Rate = 3.1 x 10^5 M^ -3 s^ -1 [NO]^2 [O2]^2
Rate = 1.7 x 10^3 M^ -2 s^ -1 [NO]^2 [O2]
Rate = 3.8 M^ -1/2 s^ -1 [NO][O2]^1/2
Rate = 9.4 x 10^3 M^ -2 S^ -1 [NO][O2]^2
Which of the following statements is TRUE?
Rate constants are temperature dependent
A catalyst raises the activation energy of a reaction
The addition of a homogeneous catalyst does not change the activation energy of a given reaction
The rate constant does no depend on the activation energy for a reaction where the products are lower in energy than the reactants
None of the above are true
How many half-lives are required for the concentration of reactant to decrease to 1.56% of its original value?
4
6
6.5
7.5
24
Identify an homogeneous catalyst.
SO2 over vanadium (V) oxide
Pt with methane
N2 and H2 catalyzed by Fe
Pd in H2 gas
H2SO4 with concentrated HCl
The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant.
H2 (g) + Br2 (g) = 2HBr (g); Kc = 3.8 x 10^4
4 HBr (g) = 2 H2 (g) + 2 Br2 (g); Kc = ?
1.6 x 10^3
5.1 x 10 ^ -3
6.9 x 10^ -10
1.9 x 10^4
2.6 x 10^ -5
In which of the following reactions will Kc = Kp?
SO3 (g) + NO (g) = SO2 (g) + NO2 (g)
2 N2 (g) + O2 (g) = 2 N2O (g)
None of the above reactions have Kc = Kp
4 NH3 (g) + 3 O2(g) = 2 N2(g) + 6H2O(g)
2 SO2(g) + O2(g) = 2 SO3(g)
Express the equilibrium constant for the following reaction.
4 Al (s) + 3 O2 (g) = 2 Al2O3 (s)
K = [Al2O3]^2 / [O2]^3 [Al]^4
K = 1/ [O2]^3
K = 1/ [3O2]^3
K = [O2]^3
K = [3O2]^3
Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows:
[N2]equ = 1.5 M, [H2]equ = 1.1 M, [NH3]equ = 0.47 M
N2 (g) + 3H2 (g) = 2 NH3 (g)
0.11
0.28
0.78
3.5
9.1
In a reaction mixture containing only products, what is the value of Q?
-1
1
0
Infinity
It cannot be determined without concentrations
Consider the following reaction at equilibrium. What will happen if the pressure increased?
4 FeS2 (s) + 11 O2 (g) = 2 Fe2O3 (s) + 8 SO2 (g)
The equilibrium constant will increase
The equilibrium constant will decrease
The equilibrium will change in the direction of the reactants
The equilibrium will change in the direction of the products
No change in equilibrium is observed
Consider the following reaction at equilibrium. What effect will removing H2O have on the system?
2 H2S (g) + 3 O2 (g) = 2 H2O (g) + 2 SO2 (g)
The reaction will shift to the left
No change will be observed
The equilibrium constant will decrease
The equilibrium constant will increase
The reaction will shift in the direction of products
Consider the following reaction at equilibrium. What effect will increasing the volume of the reaction mixture have on the system?
2 H2S (g) + 3 O2 (g) = 2 H2O (g) + 2 SO2 (g)
No effect will be observed
The equilibrium constant will decrease
The equilibrium constant will increase
The reaction will shift to the left in the direction of reactants
The reaction will shift to the right in the direction of the products
Consider the following reaction at equilibrium. What effect will decreasing the temperature have on the system?
CO2 (g) + 2 H2O (l) = CH4 (g) + 2 O2 (g)
Delta H 0 = +890 KJ
No effect will be observed
The equilibrium constant will decrease
The equilibrium constant will increase
The reaction will shift to the right in the direction of products
The reaction will shift to the left in the direction of the reactants
Give the direction of the reaction, if K << 1.
Neither direction is favored
The reverse reaction is favored
The forward reaction is favored
If the temperature is raised, then the forward reaction is favored
If the temperature is raised, then the reverse reaction is favored
What is the conjugate acid of HCO3 ^ -
H3O^ +
H2O
H2CO3
CO3^ 2-
OH^ -
Identify the products that are in equilibrium with NH3 and H2O
NH2^ - and H3O^ +
NH4^+ and OH^ -
NH3, H^+, and OH^ -
NH3 and H2O
NH2^ -, H^+, and H2O
Identify the strong diprotic acid.
H2SO3
H2CO3
HNO3
HOOCCH2COOH
H2SO4
Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25 degrees Celsius. The acid is followed by its Ka value.
HClO2, 1.1 x 10^ -2
HNO2, 4.6 x 10^ -4
HF, 3.5 x 10^ -4
HCHO2, 1.8 x 10^ -4
HCN, 4.9 x 10^ -10
What is the Kw of pure water at 50 degrees Celsius, if the pH is 6.630?
1.00 x 10^ -14
2.13 x 10^ -14
5.50 x 10^ -14
2.34 x 10^ -7
There is not enough information to calculate the Kw
Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25 degrees Celsius.
7.1 x 10^ -5 M
6.5 x 10^ -5 M
8.7 x 10^ -10 M
4.2 x 10^ -10 M
1.4 x 10^ -10 M
Which one of the following is a buffer solution?
0.10 M NaCl
0.40 M KF and 0.10 M HF
0.40 M HNO3 and 0.10 M NaNO3
0.40 M CH3COONa
0.40 M HBr and 0.10 M NaBr
Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80.
2.7
5.4 x 10^ -3
1.2 x 10^ -5
8.5 x 10^ -6
4.9 x 10^ -7
If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.11, which of the following is TRUE?
[HCHO2] > [NaCHO2]
[HCHO2] < [NaCHO2]
[HCHO2] = [NaCHO2]
[HCHO2] << [NaCHO2] (a << b means a is much smaller than b)
It is not possible to make a buffer of this pH from HCHO2 and NaCHO2
Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 200.0 mL of 0.12 M NH3. The Kb for NH3 is 1.8 x 10^ -5
9.45
9.26
9.06
4.55
4.74
When titrating a strong monoprotic acid and KOH at 25 degrees Celsius, the ...
pH will be less than 7 at the equivalence point
pH will be equal to 7 at the equivalence point
pH will be greater than 7 at the equivalence point
titration will require more moles of base than acid to reach the equivalence point
tiration will require more moles of acid than base to reach the equivalence point
Define buffer capacity.
Buffer capacity is the amount of acid that can be added until all of the base is used up.
Buffer capacity is the amount of base that can be added until all of the base is used up
Buffer capacity is the amount of base that can be added until all the acid is used up
Buffer capacity is the amount of acid that can be added until all of the acid is used up
Buffer capacity is the amount of acid or base that cab be added to a buffer without destroying its effectiveness
Given the following substances in order of increasing acid strength,
HOCl (aq) < HC2H3O2 (aq) < HC2O4^- (aq) < HOCN (aq) < HNO2 (aq) < HCl (aq)
which species listed below is the strongest base?
Cl^ - (aq)
OCl^ - (aq)
H2C2O4 (aq)
NO2^ - (aq)
OCN^ - (aq)
In the reaction, HSO4^ - + HS^ - = H2S + SO4^ 2-, which two species are both bases?
HSO4^ -, HS ^ -
HSO4^ - , H2S
HS, SO4^ 2-
HS^ -, H2S
H2S, SO4^ 2-
For the system
NH2OH +CH3NH3^ + = CH3NH2 + NH3OH^+
the position of the equilibrium lies to the left. Which is the strongest acid in the system?
NH2OH
CH3NH3^+
CH3NH2
NH3OH^+
NH2OH and CH3NH3^+ are equal in acid strength, and are the strongest acids in the system
Given that X is the same atom for each of the following, which is the strongest oxyacid?
The structure with the most single bonded H's
The structure with the most single bonded O's
The structure with an equal number of single bonded H's and O's
The structure with the most double bonded O's
The structure with an equal number of double bonded H's and O's
Determine the molar solubility for Pb3(PO4)2 in pure water. Ksp for Pb3(PO4)2 is 1.0 x 10^ -54.
4.1 x 10 ^ -28
5.8 x 10^ -10
1.1 x 10^ -11
6.2 x 10^ -12
1.0 x 10^ -54
Identify the ion that is less soluble in acidic water.
NH4^ +
S^2-
CO3^ 2-
OH^ -
CN^ -
The difference between Q and Ksp is
Q is greater than Ksp
No difference
Ksp is the value of the product at equilibrium and Q is the value of the product under any condition
Ksp is greater than Q
Q is the value of the product at equilibrium and Ksp is the value of the product under any condition
Which of the following compounds will have the highest molar solubility in pure water?
PbSO4, Ksp = 1.82 x 10^ -8
MgCO3, Ksp = 6.82 x 10^ -6
AgCl, Ksp = 1.77 x 10^ -10
CdS, Ksp = 8.00 x 10^ -28
HgS, Ksp = 1.60 x 10^ -54
The ____ Law of Thermodynamics states that for any spontaneous reaction, the entropy of the universe increases.
Zero
First
Second
Third
Fourth
Identify the process in which the entropy increases.
A decrease in the number of moles of a gas during a chemical reaction
The phase transition from a gas to a liquid
The phase transition from a solid to a gas
The phase transition from a gas to a solid
The phase transition from a liquid to a solid
Above what temperature does the following reaction become nonspontaneous?
2 H2S (g) + 3 O2 (g) = 2 SO2 (g) + 2 H2O (g)
Delta H = -153.2 J/K
6.762 x 10^ 3 K
158.7 K
6.762 K
This reaction is nonspontaneous at all temperatures
This reaction is spontaneous at all temperatures
The ___ Law of Thermodynamics states the entropy of a perfect crystal at absolute zero is zero.
Zero
First
Second
Third
Fourth
For a given compound, list the decreasing order of entropy for a liquid, solid, and gas.
solid > gas > liquid
liquid > solid > gas
gas > liquid > solid
gas > solid > liquid
solid > liquid > gas
Which of the following statements is TRUE?
Entropy is an extensive property
Entropy is not temperature dependent
Exothermic processes decrease the entropy of the surroundings
Delta S universe is always greater than zero for a nonspontaneous process
None of the above is true
Place the following in order of increasing entropy at 298 K.
Ne, Xe, He, Ar, kr
He < Kr < Ne < Ar < Xe
Xe < Kr < Ar < Ne < He
Ar < He < Ar < Ne < Kr
Ar < Ne < Xe < Kr < He
He < Ne < Ar < Kr < Xe
Calculate Delta S 0 rxn for the following reaction. The S 0 for each species is shown below the reaction.
4 NH3 (g) + 5 O2 (g) = 4 NO (g) + 6 H2O (g)
S 0 (J/mol*K) 192.8, 205.2 , 210.8, 188.8
-287.4 J/K
-401.2 J/K
+160.0 J/K
+336.6 J/K
+178.8 J/K
Identify the compound with the highest delta G 0 f.
N2 (g)
H2 (g)
O2 (g)
Cl2 (g)
All compounds have a value of zero
What is true if ln K is negative?
Delta G 0 rxn is positive and the reaction is spontaneous in the forward direction
Delta G 0 rxn is negative and the reaction is spontaneous in the forward direction
Delta G 0 rxn is negative and the reaction is spontaneous in the reverse direction
Delta G 0 rxn is positive and the reaction is spontaneous in the reverse direction
Delta G 0 rxn is zero and the reaction is at equilibrium
Which of the following reaction will have the largest equilibrium constant (K) at 298 K?
CaCO3 (s) = CaO (s) + CO2 (g); Delta G 0 = +131.1 KJ
2 Hg (g) + O2 (g) = 2 HgO (s); Delta G 0 = -180.8 KJ
3 O2 (g) = 2 O3 (g); Delta G 0 = +326 KJ
Fe2O3 (s) + 3 CO (g) = 2 Fe (s) + 3 CO2 (g); Delta G 0 = -28.0 KJ
It is not possible to determine without more information
Which of the following processes has delta S > 0?
SO2 (l) = SO2 (s)
N2 (g) + 3 H2 (g) = 2 NH3 (g)
CH4 (g) + H2O (g) = CO (g) + 2 H2 (g)
K2CO3 (s) + H2O (g) + CO2 (g) = 2 KHCO3 (s)
All of the above processes have a delta S > 0
For the Following example, identify the following.
F2 (l) = F2 (s)
EXOTHERMIC
A negative delta H and a negative delta S
A positive delta H and a negative delta S
A negative delta H and a positive delta S
A positive delta H and a positive delta S
It is not possible to determine without more information
