Electron Transfer and Reactions Systems in Balance & Water Balance of Power Questions Chemistry homeworkmostly mutiple choiceLet me know if you need anythi

Electron Transfer and Reactions Systems in Balance & Water Balance of Power Questions Chemistry homeworkmostly mutiple choiceLet me know if you need anything elseThanks Lesson 4 Hand-in Assignment:
Energy Is Predictable
1. The bombardier beetle uses the following explosive reaction as a defence mechanism.
The product acts as a repellent.
Calculate the enthalpy change for the above reaction using the following information
equations. Show your complete work. (4 marks)
1.
2.
3.
2. Sulphur trioxide gas, SO3(g) and water can react under appropriate conditions to form
sulphuric acid in the atmosphere. The reaction is responsible for much of the acid rain
that is affecting the environment.
a. What is the enthalpy change when one mole of the acid forms from SO3(g)? Show your
complete calculations. Assume that the water is liquid and the sulphuric acid is liquid. (4
marks)
b. Draw a labelled potential energy diagram to represent the change. You do not have to
use graph paper. Your graph axes should be between 5 cm and 7 cm long. (2 marks)
3. Use the given diagram to answer this question.
Calculate the heat of solution for one mole of NaCl(s). Show your work completely. (2
marks)
4. Aluminum metal reacts with solid copper(II) oxide to form copper metal and solid
aluminum oxide.
a. Write the equation (balanced with whole numbers) representing this reaction and
show all necessary calculations to find the enthalpy( Hr)change for two moles of
aluminum reacting. (4 marks)
b. Draw a labelled potential energy diagram for this reaction. You do not have to use
graph paper. Your graph axes should be between 5 cm and 7 cm long. (2 marks)
5. A student is required to determine the molar enthalpy (heat) of combustion for
calcium in the reaction
, using the following reactions and the data collected.
Reaction 1
Reaction 2
Reaction 3
Chart 2
Reaction
Mass
Volume of
1.0 mol/L
Initial
Temperatu
re
Final
Temperatu
re
1
0.50 g
Ca(s)
0.10 L
22.3°C
35.9°C
2
1.50 g
CaO(s)
0.10L
22.0°C
29.1°C
Assume the specific heat and density of HCl(aq) are the same values as for water.
Show your complete work in each part of this question.
a. Determine the molar enthalpy H​r​ value for calcium solid in Reaction 1 . (4 marks)(
Hint—Use the information in the second chart)
b. Determine the molar enthalpy H​r​ value for calcium oxide solid in Reaction 2 . (4
marks)( Hint—Use the information in the second chart)
c. Using Reactions 1 , 2 , and 3 determine the
value for the combustion of calcium
metal. (4 marks) (Hint— Use Hess’ Law — and your answers from a and b. to solve
.
Lesson 5 Assignment: Energy Alternatives and Society
Total /37
1. A student wished to determine the molar heat (enthalpy) of formation for sodium
sulphide, Na​2​S(s). The student designed an investigation where 11.4 g of hydrogen
sulphide gas, H​2​S(g), was completely reacted with solid sodium hydroxide in a bomb
calorimeter producing solid sodium sulphide and liquid water. The 250 mL of water in
the calorimeter changed in temperature from 23.2°C to 43.8°C. Assuming only the
calorimeter water gained the heat energy, calculate the molar heat of formation for
sodium sulphide. Show your work neatly and completely.
(5 marks)
2. You are given the following information equations:
1:
2:
3:
Calculate the
for the following reaction:
Show how
you manipulate your information equations to achieve your answer. (4 marks)
3. Use the following fission and fusion reactions to answer this question.
a. Which substance,
or
, is more efficient by releasing more energy per gram
reacted? Support your answer with calculations. (3 marks)
4. How much energy is released when 1.000t (1000kg) of sulphur trioxide is produced by
the following reaction?
(3 marks)
2SO​2(g) ​+O​2(g)​——–>2 SO​3(g)​
=-192.8 kJ
5. In respiration,glucose is oxidized by oxygen gas to produce carbon dioxide gas, liguid
water, and energy. What is the energy released when 18.0 g of glucose is consumed?
(5 marks)
6. Pick any one of the alternate energies covered in this lesson and provide a
risk/benefit assessment on the technology. Provide a minimum of 5 risk and 5 benefits
for it.(You may have to use the internet and other sources) Give our opinion and explain
using 3 different perspectives (ie. social, economical, ecological, political etc.) why or
why not it would be a viable alternative energy source for Canada. (8 marks)
7.a) Explain the difference between a chemical catalyst and a biological catalyst. (2 marks)
b) Explain why, in terms of energy, why H​2​0(l) is always produced in oxidation reactions,
using enzymes, in the body. (3 marks)
Lesson 6 Assignment: Electron Transfer and Reactions
1. Using your ​periodic table​ of the elements, indicate whether each of the following
substances could act as an oxidizing agent (OA), a reducing agent (RA), or possibly both
(OA/RA). (4 marks)
a.Ba​2+​(aq)
b.Co​2+​(aq)
c.Se(s)
d.Cs(s)
2. A student completed an investigation to identify some unknown metals, which were
labelled D, Z, A, and X. The choices for the metals were Zn, Pb, Fe, and Ag. The following
chart gives results of reactions that occurred between the metal ions and metals that
were placed in the solutions.
A positive result for a reaction is indicated by the word yes.
a. From the results in the table, create a redox table of reduction half-reactions. List the
oxidizing agents in decreasing order of strength. (4 marks)
b. Match each letter of the unknown metals with its correct metal symbol.
(2 marks)
3. For each of the following, indicate whether the equation represents a reduction
half-reaction or an oxidation half-reduction. (5 marks)
a. 2 H​2​O(l) +2e- –>H​2​(g) +2OH​-​(aq)
b.
S(s) + 3 H​2​O(l) —> H​2​SO​3​ (aq) + 4 H​+​(aq) +4 e-
c.
As​2​O​3​(s) +6 H+(aq) +6e- —> 2As(s) +3H​2​O(l)
d.Fe​3+​(aq) +3e- —> Fe(s)
e. Pb(s) + SO​4​2-​(aq) —> PbSO​4​(s) +2e4. Explain historically, in one-quarter page or less, what the terms ​oxidation and
reduction​ originally meant (give the empirical definitions). (2 marks)
5. Could you successfully store a solution of acidified potassium permanganate in a tin
can? Explain. Support your answer to this question with chemical equations. (4 marks)
6. For each of the following situations, write out the most likely redox equation. Follow
the five-step procedure for predicting redox reactions. Show all your steps.
a. Zinc metal is placed into a solution of AuCl​3​(aq). (3 marks)
b. Chlorine gas and hydrogen gas are simultaneously bubbled into a sodium hydroxide
solution. (3 marks)
c. A perchloric acid solution is slowly added to hydrogen peroxide,H​2​O​2​. (3 marks)
d. A fountain pen dipped into hydrochloric acid is used to etch a student’s name onto a
piece of copper foil. (3 marks)
7. Did the pen in question (6. d.) successfully etch the copper foil? Explain. (2 marks)
8. Predict the products of a reaction between a small piece of sodium metal and water.
Give three diagnostic tests that could be used to identify the products that were formed.
Support your answer for this question with chemical equations. (5 marks)
Lesson 7 Assignment: Redox Applications
total /34
Review the Evaluation information found in the introductory pages of this lesson.
1. An increase in the oxidation number of a chemical species causes it to be
__________(oxidized/reduced). ​select which one​ ​(1 mark)
2. Explain if it is possible to have a reaction in which oxidation takes place, but reduction
does not. make sure to use the proper termenology. ​(2 marks)
3. A student titrated a sample of an acidified tin(II) chloride solution with potassium
permanganate.
a. List the oxidizing agent and reducing agent that would participate in the reaction. ​(2
marks)
b. What colour change would signify the endpoint? ​(1 mark)
c. Which chemical species is the titrant? ​(1 mark)
d. When would the equivalence point of this titration be reached? Be specific. Give the
actual mole ratio of the oxidizing and reducing agents.— You do this by following the 5
step method to develop the redox reaction. ​(3 marks)
4. Indicate for each of the following equations whether or not they represent a redox
reaction. Write redox or not redox as your answer choice for each equation. ​(4 marks)
a. Ca(s) + F​2​(g) –> CaF​2​(s)
b. MgCl​2​(aq) + 2NaOH(aq) —> Mg(OH)​2​(aq) + 2 NaCl(aq)
c. CaCO​3​(s) + 2HCl(aq) —>CaCl​2​(aq) + H​2​O(l) + CO​2​(g)
d. NaI(aq) + 3HOCl(aq) —> NaIO​3​(aq) + HCl(aq)
5. Indicate the oxidation number of phosphorous in each of the following species. For each
case, write P = and then your answer. ​(4 marks)
a. HPO​4​2b. H​3​PO​2
c. P​4​O​10
d. Na​2​HPO​4
6. Write the balanced chemical equation for the redox reaction (5 step method) that might
occur when hydrogen gas is bubbled into a basic solution of gold(III) nitrate.
In your response, show the half-reactions, the overall equation, and predict the
spontaneity of the reaction. ​(3 marks)
7. Balance the following redox equation by using the oxidation number method or the 1/2
reaction method. In your response, indicate the appropriate oxidation numbers and
balancing coefficients. ​(3 marks)
NaIO​3​(aq) + NaI(aq) +HCl(aq) —> NaCl(aq) + I​2​(s) + H​2​O(l)
8. This question is a numerical response question. Record only your final answer to three
digits in a box similar to the following:
Enter the first digit of your answer in the left-hand box and leave any unused boxes blank.
If a decimal point occurs in your answer, it should occupy its own box.
When 1.20 mol of H​2​PO​4​-​(aq) reacts according to the following equation
12 H​2​PO​4​-​(aq) + 12 H​+​(aq) + 10Br​-​(aq) —> 3 P​4​(s) + 18 H​2​O(l) +10 BrO​3​-​(aq)
the number of moles of electrons transferred is ___ ___ ___ __ mol. ​(2 marks)
9. Use the following information to answer this question.
PCl​5​(s) + 2 Na(s) —> PCl​3​(s) +2 NaCl(s) + 729.5 kJ
Calculate the heat produced when 0.235 mol of reducing reagent reacts. Show all your
work. ​(3 marks)
10. A chemistry student titrated three 25.0 mL samples of acidified tin(II) nitrate solution
with 0.00800 mol/L potassium permanganate to find the concentration of the Sn​2+​(aq)
ions in the solution. Obtain the results of the three trials by reading the buret volumes (in
millilitres) of KMNO​4​(aq).
Based on the data given, calculate the concentration of Sn​2​+​(aq) ions in the solution. Show
all your work in your response, including a net redox equation and calculations. ​(5 marks)
Lesson 8 Assignment: Chemical Energy at Work
total /32
1. The following diagram represents a zinc/silver electrochemical cell with the following
notation:
The salt bridge contains NaNO​3​(aq) . Use the preceding notation and the diagram to
answer the seven parts of this question.
a. Label the appropriate letters with the following terms (not all letters may be used and
the same letter may be used more than once):
• cathode • direction of anion flow
• location of strongest oxidizing agent (SOA) • salt bridge
• location of strongest reducing agent (SRA)
b. The ions initially present in the solution indicated by point ​B​ would be
___________________________. (1 mark)
c. The ions initially present in the salt bridge would be
___________________________. (1 mark)
d. The ions that would migrate through the salt bridge from each solution would be
___________________________. (2 marks)
e. The direction of flow of electrons would be towards the electrode labelled letter
___________________________. (1 mark)
f. Describe what happens to the concentrations of the following ions as the cell operates:
(4 marks)
Calculate the standard cell potential of this silver/zinc cell. (2 marks)
2. Calculate the potential difference of the cells represented by the following
information:
a.
b.
(2 marks)
(2 marks)
3. If
was chosen as the standard reference electrode, explain
how it would affect the answer to question 2. a. (2 marks)
4. Rearrange the following sets of half-reactions to create an electrochemical cell in each
case. Write the labelled cathode half-reaction, anode half-reaction, and net ionic
reaction. Also calculate the net cell potential. Show all your work clearly. Marks will be
given for both your work and your answer. (6 marks)
a.
b.
5. Use the following information to answer all parts of this question. Show all your work
clearly. Marks will be given for both your work and your answer.
A voltaic cell was constructed from two half-cells as follows:
One half-cell was made from an unknown metal and a solution containing its ion. The
other half-cell was
. The net cell potential was +1.13 V. After 24 hours, it
was observed that the blue colour of the copper half-cell solution had intensified.
a. Determine the reduction potential of the unknown metal. (3 marks)
b. Considering experimental error, use your table of redox half-reactions to predict the
most likely identity of the unknown metal. (1 mark)
6. Three standard half-cells are constructed from unknown metals​ X(s), Y(s) , and Z(s)​ and
their ions ​X2+​
​ (aq) ,Y​2+​(aq) , and Z​2+​(aq)​ . Different combinations of the three half-cells are
tried when constructing various electrochemical cells. The following information is
obtained from the different combinations:
• An
standard half-cell attracts anions when the other standard
half-cell is
. The
.
• In a standard cell between​ X(s) and Z(s)​, the cathode is ​X(s)​ and the E​0​net​ = 0.14V.
Determine the cathode, anode, and net cell potential of a standard cell between
and
.
Lesson 9 Assignment:
Turning Electricity into Chemistry
total /31
1. Decide whether each of the following statements concerning an electrolytic cell are
true (T) or false (F). For each statement, explain why it is true or false. (7 marks)
a. A salt bridge or other semi-permeable membrane is required.
b. The oxidation number of the species reacting at the anode increases as the cell
operates.
c. The reduction half-reaction has a higher reduction potential than the reduction
potential of the oxidation half-reaction.
d. The reduction potential of Cd​2+​(l)​ + 2e- –> Cd​(l)​ is – 0.40 V during the electrolysis of
molten cadmium chloride (CdCl​2(l)​) .
e. In the electrolysis of NaBr(aq) , the solution will turn darker at the anode, while the
mass of the cathode will increase.
f. A greater mass increase will occur at the cathode from a CoCl​2​(aq) solution than from a
NiCl​3​(aq) solution with the same current over the same time.
g. An electrochemical cell with a potential of 3.0 V can be used to produce hydrogen at
the cathode in the electrolysis of aqueous lithium hydroxide.
2. A student wanted to determine the purity of a sample piece of iron. The following
equipment was available:
• the impure iron sample • a piece of zinc
• a piece of copper • 1.0 mol/L Fe(NO​3​)​2​(aq)
• 1.0 mol/L • 1.0 mol/L Cu(NO​3​)​2​ (aq)
• (2) 250 mL beakers • steel wool
• a porous cup • wire
• an electronic balance • voltmeter
The student constructed a cell using some of this material and recorded the following
results:
(Assume that the impurities are unreactive.)
a. Write the anode equation, cathode equation, and net ionic equation that represent the
reaction that occurs. (3 marks)
b. Calculate the net potential difference of this cell. (1 mark)
c. Draw a sketch of the cell operating in this question. Label the cathode, anode,
direction of cation and electron flow, and all materials used in the construction of the
cell. You may use only the materials listed in this question. (6 marks)
d. Is the cathode Electrode A or Electrode B? Explain. (2 marks)
3. Calculate the net cell potential of the following cells, making sure you include the
labelled cathode and anode half-reaction equations and the net ionic reaction equation
in your answer. Indicate, as well, whether the reaction is spontaneous or
non-spontaneous. Show all your work clearly. Marks will be given for both your work
and your answer.
a. A platinum and a copper electrode are immersed into a lead(II) nitrate solution and
connected to make a cell. (3 marks)
b. Two silver electrodes are placed in a solution of CaI​2​(aq) and connected to make a cell.
(3 marks)
4. Calculate the mass of element produced at the anode during the electrolysis of molten
chromium(III) bromide if 2.50 A runs through the cell for 45 minutes. Show all your work
clearly. Marks will be given for both your work and your answer.
(3 marks)
5. Use the following diagram to answer this question.
a. Predict the strongest oxidizing and reducing agents in the given cell. Based on your
answer, describe the necessary direction of electron flow in the cell (either from Sn(s) to
Cu(s) or from Cu(s) to Sn(s)) Explain your rationale. (2 marks)
b. Calculate the time in hours needed to make the anode change in mass by 3.00 g if the
current through the solution is 275 mA. Remember, 1 mA =10​-3​ A. Show all your work
clearly. Marks will be given for both your work and your answer. (3 marks)
Lesson 10 Assignment: Systems in Balance
Review the Evaluation information found in the introduction of this lesson.
Part A: Multiple Choice
Read each question carefully and decide which of the choices best answers the question
or completes the statement. Place the number of each question in a vertical column and
place your answer (A, B, C, or D) beside each number. (Total = 5 marks)
Use the following information to answer questions 1-3.
I.
II.
III.
IV.
V.
1. Which of the system(s) would shift towards the products with the addition of heat?
A. I, III
B. II
C. II, IV, V
D. V
2. The system(s) which would shift towards reactants with an increase in pressure by
compressing the system into a smaller vessel would be
A. I, III, IV
B. II
C. IV
D. V
3. The system whose equilibrium would not shift because of any change in pressure is
A. I
B. III
C. IV
D. V
4. Which of the following statements is true about a chemical system at equilibrium?
A. K = 1
B. [products]/[reactants] = 1
C. [reactants] = [products]
D. forward reaction rate = reverse reaction rate
5. A particular chemical equilibrium has an equilibrium constant K = 1250. A true
statement about this equilibrium would be
A. The products are favoured.
B. The reactants are favoured.
C. The reaction is exothermic.
D. The reaction reaches equilibrium quickly.
Part B: Written Response
For full marks, your answers must show all pertinent explanations, calculations, and
formulas.
6. The following is a graphical representation of this equilibrium:
Describe what stress must have occurred to create each situation shown on the graph.
The stresses are marked by a., b., c., and d. (4 marks)
7. In a closed environment, phosphorus pentachloride will decompose into, and form an
equilibrium system with, phosphorus trichloride and chlorine gas.
Calculate the equilibrium constant for this reaction at 25°C if a set of equilibrium
concentrations were found to be
marks)
and
. (2
8. In a flask initially containing colourless molecules of ,N​2​O​4​(g) the brown colour
characteristic of NO​2​(g)appears and the colour steadily intensifies. Is this system in
equilibrium? Explain. (2 marks)
9. The following reaction was performed at 1000°C.
The equilibrium constant was found to be 0.0232 (Reaction 1). When this same reaction
was performed at a different temperature, the equilibrium constant was calculated as
0.0563 (Reaction 2).
Was the temperature in Reaction 2 higher or lower than 1000°C? Explain your reasoning.
(3 marks)
10.
a. Write the equilibrium law expression and use the preceding table to calculate the K
value for the equilibrium system
at 227°C. (2 marks)
b. Calculate the values necessary to complete the rest of the table
(i, ii, an…
Purchase answer to see full
attachment