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23 Nov 2019

An electrolytic cell produces aluminum from Al2O3 at the rate of 20kg Al a day. Assume 100% yield.

[ 1 ampere = 1 coulomb/sec 1 mole electrons = 9.648x10^4coulomb]

How many moles of electrons must pass through the cell in one day,how many amperes are passing through the cell, and how many molesof oxygen are being produced simultaneously?

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Related questions

This is for the lab practical I take on Tuesday night. If you could answer each one and show your work/ explain that'd be amazing so I can do well on the actual practical on Tuesday! Thank you!

Chemistry 211 Lab Final Study Guide Spring 2015

Useful Information:
1 ampere =coulomb/sec
Faraday’s constant = 96,500 coulombs/mole of electrons
Molar mass of Au = 197.0 g/mole, Molar mass of Cu = 63.55 g/mole
m = moles , ' ’

c kg

ΔTf

= Tf

− Tf

where Tf is for the pure solvent and Tf

is for the mixture.

ΔT = (K

)(m ) ,

m = (

(mass of

solute, g )
)( ).

f f c

c molar

mass, g

mol −1

mass of

solvent, kg


7. Next question

(a) If you weigh 6.355 grams of copper, add concentrated nitric acid to dissolve it, and then dilute the solution to a total volume of 50 mL, how many moles of copper are in this solution?


(b) For the equilibrium reaction 3H2(g) + N2(g) → 2NH3(g), what is the equilibrium constant expression, Kc, for this reaction? (5pts)

8. Suppose at some temperature, the equilibrium concentration of H2 is 0.45M, the equilibrium concentration of N2 is 0.38M, and the equilibrium concentration of NH3 is 0.42M. What is the value of the equilibrium constant for the reaction 3H2(g) + N2(g) → 2NH3(g) at this temperature? (Show your work. No credit will be given if your work is not shown.)

9. Next question
(a) If you need 0.0534 moles of NaOH to reach equivalent point in the titration with acetic acid, how many mL of 0.09876M NaOH will you need?


(b) The Ksp of Cu(OH)2 is 2.2x10-20, what is the solubility of Cu(OH)2?


10. Next question
(a) In non-sulfide qualitative analysis of representative cations, the Group A cations comprising of Pb2+,

Hg2+, and Ag+ give a precipitate with solution.
(b) From a solution containing mixture of Pb2+, Fe3+, and Al3+, Pb2+ is removed by adding HCl solution. To the remaining cation mixture, on making the solution basic with NH3 (pH=9 – 10), both the cations form precipitate. Further analysis of the cation mixture containing Fe3+ and Al3+ is carried out by adding NaOH solution.


Aluminum hydroxide (dissolves/remains undissolved) in NaOH solution while Ferric hydroxide ( dissolves/remains undissolved).
(c) Fe(OH)3 precipitate is dissolved in minimal amount of aqueous HCl which gives a


yellow solution. To this solution addition of solution (at pH = 4 – 5) yields a dark blue solid known as Prussian Blue.

(d) Describe the method for checking for completeness of precipitate in qualitative analysis of ions.

The equation Mg + HCl MgCl2 + H2 can be balanced by _____.

A) Changing the coefficient of Mg to 2

B) Changing the coefficient of HCl to 2

C) Changing the coefficient of MgCl2 to 12 .

D) Changing MgCl2 to MgCl

E) Changing H2 to H

In the reaction below, how many molecules of water can be made from 38 molecules of C6H12O6?

C6H12O6 + 6O2  6H2O + 6CO2 A) 38
B) 6
C) 144

D) 228 E) 44

In the chemical reaction H2SO4 + 2NaOH Na2SO4 + 2H2O, the coefficient of sodium sulfate is _____.
A) 0
B) 1

C) 2 D) 3 E) 4

H2CO3 CO2 + H2O is an example of which type of reaction?

A) Substitution

B) Combination

C) Combustion

D) Decomposition

E) Formation

In the reaction H2 + F2  2 HF, which of the following is true?

A) H2 is reduced

B) H2 is the oxidizing agent

C) F2 is reduced

D) HF is called the reducing agent

E) HF is called the oxidizing agent

Page 1

Ascorbic acid (C6H8O6) acts as an antioxidant by being oxidized to _____. A) C6H8O6
B) C6H8O8
C) C4H9O7

D) C6H6O4 E) C6H6O6

During anaerobic metabolism pyruvic acid is converted to _____.

A) lactic acid

B) citric acid

C) oxalic acid

D) acetic acid

E) nitric acid

Reduction of CH3 = CH3 by hydrogen yields _____.

A) 2CH4

B) CH2 = CH2

C) CH3CHO

D) C2H6

E) CH3OH

Which of the following is not considered to be a form of reduction?

A) Gain of a hydrogen ion

B) Gain of electrons

C) Loss of an oxygen ion

D) Gain of negative charge

E) Gain of a sodium ion

Consider the reaction:
Au(s) + 3HNO3(aq) + 4HCl(aq)  HAuCl4(aq) + 3NO2(g) + 3H2O(l), how many Au atoms will react with 996 molecules of HCl?
A) 1992
B) 996
C) 498
D) 249
E) 336

Page 2

Oxidation of CH3CHO gives _____. A) CH3COOH

B) C2H6
C) C2H5OH D) H2C=CO E) CH3OH

Three moles of (NH4)2Fe(SO4)2·6H2O contains _____ moles of H2O.

A) 3

B) 6

C) 9

D) 12

E) 18

How many moles of hydrogen atoms are present in 27 grams of H2O?

A) Approximately one

B) Approximately one and a half

C) Approximately two

D) Approximately two and a half

E) Approximately three

Five
atoms of nitrogen?

A) 140.07 u

B) 28.014 u

C) 14.007 u

D) 280.14 u

E) 42.021 u

What is the molar mass of MgCO3?

A) 56.928 g/mol

B) 71.173 g/mol

C) 85.755 g/mol

D) 84.313 g/mol

E) 36.312 g/mol

moles of nitrogen molecules have a mass of 140.07 g. What is the mass of 10

Page 3

Consider the formation of ammonium chloride given by the equation:
NH3 + HCl  NH4Cl. How many grams of HCl would fully react with 76.43 moles of ammonia?
A) 1302
B) 2787
C) 2709
D) 4088
E) 4071

In the reaction 2P + 5Cl2  2PCl5, how many moles of atomic chlorine need to be reacted to form 525 g of PCl5?

A) B) C) D) E)

18. 1 Pa A)

B) C) D) E)

1.00 3.15 2.00 12.6 6.30

= _____ 1 atm
1 torr
1 J/s

1 N/m2 1 kJ/m

If a sample of gas has an initial pressure of 2.36 atm and an initial volume of 10.7 L, what is the final pressure if the volume is reduced to 4.09 L? Assume that the amount and the temperature of the gas remain constant.

A) 103 atm

B) 6.17 atm

C) 0.902 atm

D) 43.8 atm

E) 18.5 atm

A gas sample at 40°C has an initial volume of 40.0 L. What is its volume if the temperature is changed to 120°C? Assume that the pressure and the amount of the gas remain constant.

A) 1.99 L

B) 8.13 L

C) 50.2 L

D) 31.9 L

E) 123L

Page 4

Three moles of (NH4)2Fe(SO4)2·6H2O contains _____ moles of hydrogen atoms.

A) 4

B) 6

C) 20

D) 60

E) 100

How many moles of oxygen atoms would be present in 3.65 moles of Na2SO4?

A) 13.56

B) 3.65

C) 7.30

D) 10.95

E) 14.60

How many moles of NaCl are present in 20.0 g of NaCl?

A) 58.4

B) 1.01

C) 29.2

D) 0.342

E) 0. 0143

How many moles of oxygen atoms are present in one mol of (C2H5COO)2Ca?

A) 1

B) 2

C) 3

D) 4

E) 5

Codeine (C18H21NO3) is a painkiller. What is the molar mass of codeine? A) 195.60

B) 299.37 C) 227.30 D) 211.43 E) 313.35

Page 5

In the reaction H2SO4 + 2NaOH  Na2SO4 + 2H2O, the number of moles of H2O that can be produced from 10 moles of NaOH is _____.
A) 2
B) 3

C) 5 D) 10 E) 20

How many cal is 542.0 kJ? A) 129.5

B) 542.0 C) 2267 D) 542,100 E) 129,500

Which of the following is the correct definition for the specific heat of a particular substance?

A) The amount of heat released when one gram of the substance is heated.

B) The temperature change when one gram of the substance is burned.

C) The amount of substance in grams which when cooled by 1°C releases 1kJ of

energy.

D) The amount of heat released when one gram of a substance is cooled by 1°C.

E) The amount of heat absorbed when the temperature increases by 1°C

A specimen weighing 100.0 g is heated from 30.00°C to 63.30°C. If the quantity of heat transferred is 5834 cal, determine the specific heat of the specimen.

A) 17.25 cal/ g·°C

B) 1.572 cal/ g·°C

C) 12.75 cal/ g·°C

D) 1.752 cal/ g·°C

E) 1.257 cal/ g·°C

What quantity of heat is transferred when a 250.0 g block of aluminum is heated from 25.00°C to 73.30°C? (Hint: The specific heat of aluminum = 0.2150 (cal/g·°C).)

A) 56160 cal

B) 2596 cal

C) 1.110 cal

D) 1298 cal

E) 8986 cal

Page 6

How much heat is necessary to melt 70 g of ice (solid H2O) at 0°C? The heat of fusion of H2O is 79.9 cal/g.

A) 73 cal

B) 79 cal

C) 5500 cal

D) 1400 cal

E) 5600 cal

What is the process by which a substance forms vapor directly from the solid state without becoming a liquid?
A) Melting
B) Sublimation

C) Fusion
D) Condensation E) Vaporization

Which of the following statements is true for the bonding of atoms?

A) The energy of a compound is equal to the energies of the atoms which make up the

compound.

B) The energy of the individual atoms is lower than the energy of the compound.

C) The formation of a compound naturally, from individual atoms requires external

energy.

D) When a compound disintegrates there is a release of energy which equals the

difference in energy between individual atoms.

E) Individual atoms have higher amounts of energy than when in a compound.

What term is used to describe the strength of interactions between atoms in an ionic compound?

A) Bond energy

B) Lattice energy

C) Chemical energy

D) Crystal energy

E) Ionic energy

The reaction between sodium metal and HCl gives off heat. This type of reaction is called an _____ reaction.

A) isothermal

B) exothermic

C) endothermic

D) energy requiring

E) energy-less

Page 7

Which of the following is an endothermic reaction?

A) 2H2 + O2  2H2O + 135 kcal

B) H2 + F2  2HF + 130 kcal

C) CH4 + 2O2  CO2 + 2H2O + 213 kcal

D) C2H4 + H2  C2H6 + 137 kJ

E) 2SnCl2 + 33 kcal  Sn + SnCl4

Which of the following is true about gases?

A) They have a definite shape.

B) Their particles are in close contact with each other.

C) They have no definite volume.

D) They take the shape of the bottom of the container.

E) They have strong intermolecular interactions.

As
other and with the walls of their container. The force generated by gas particles divided by the area of the container walls yields_____.
A) volume
B) pressure
C) temperature
D) amount
E) density

If a sample of gas has an initial pressure of 4.83 atm, what is the initial volume if the pressure is increased to 10.0 atm and the volume is reduced to 10.0 L? Assume that the amount and the temperature of the gas remain constant.

A) 10.0 L

B) 20.7 L

C) 4.83 L

D) 483L

E) 0.207 L

A sample of gas has Pi = 0.50 atm, Vi = 9.5 L, and Ti = 290 K. What is the final volume

if Pf A) B) C) D) E)

= 0.75 atm and Tf = 350 K? 7.6 mL
7.6 cL
7,600 cL

7,600 mL 7,600 L

Having trouble with thse questions. Please answer all questions correctly. Will provide a thumbs up.

1.Which of these equations is the balanced reaction between nitrous acid solution and solidmagnesium hydroxide ?

A.2NH3(aq) + MgOH (s) Mg(NH4)2(aq) + 2 H2O(l)

B.2HNO2(aq) + Mg(OH)2(s) Mg(NO2)2(aq) + 2 H2O(l)

C.2HNO3(aq) + Mg(OH)2(s) Mg(NO3)2(aq) + 2 H2O(l)

D.2HNO2(aq) + MgOH (s) Mg(NO3)2(s) + 2H2O(l)

2.Balance the following chemical equation:

C3H7OH(l) + O2(g)CO2(g) + H2O(g)

a. C3H7OH(l) + 4 O2(g)3 CO2(g) + 4 H2O(g)

b.2 C3H7OH(l) + 9 O2(g)6 CO2(g) + 8 H2O(g)

c.C3H7OH(l) + 5 O2(g)3 CO2(g) + 4 H2O(g)

d.C3H7OH(l) + O2(g)CO2(g) + H2O(g)

3.Which species would be considered a spectator ion based on the following equation?

Ba2+ + 2NO3− + 2Na+ + SO42- → BaSO4(s) + 2NO3− + 2Na+

SO42-

2NO3−

Ba2+

BaSO4

4.Barium sulfate is often ingested to aid in the diagnosis of GI tract disorders. The equation for its production is Ba2+ + SO42- → BaSO4(s). What type of equation is this?

A full equation

A net ionic equation

A total ionic equation

An oxidation-reduction equation

5.Which species is being reduced in this reaction?

CuO(s) + H2(g) Cu(s) + H2O(g)

H2O

CuO

Cu

H2

6.Which of the following is an oxidizing agent?

H2

NH3

O2

H2O

7.The following chemical equation,

HC2H3O2(aq) + KOH(aq) KC2H3O2(aq) + H2O(l),

is an example of a(n) _______ reaction.

a.oxidation-reduction and acid-base

b.acid-base

c.precipitation

d.oxidation-reduction and precipitation

e.oxidation-reduction

8.What substance is oxidized in the following reaction?

4HCl + MnO2 → Cl2 + 2H2O + MnCl2

a.Mn in MnO2

b.O in MnO2

c.Cl in HCl

d.H in HCl

9.What is the reducing agent in the following reaction?

4HCl + MnO2 → Cl2 + 2H2O + MnCl2

Cl2

MnCl2

HCl

MnO2

10.All redox reactions involve oxygen.

True

False

11.The term formula weight can be used with respect to which of the following?

A.ionic compounds

B.covalent compounds

C.both a and b

D.neither a nor b

12.What is the molecular weight of ibuprofen, C13H18O2?

A.206.3 amu

B.377.7 amu

C.29.0 amu

D.289.4 amu

13.The mass of an atom of 12C is exactly 12 atomic mass units. Which of the following describes a mole of 12C atoms?

A.a sample which weighs exactly 12 atomic mass units

B.a sample which contains 6.02 × 1023 atoms of 12C

C.both a and b

D.neither a nor b

14.The mass of an atom of 12C is exactly 12 atomic mass units. Which of the following describes a mole of 12C atoms?

A.a sample which contains 6.02 × 1023 atoms of 12C

B.a sample which weighs exactly 12.011 grams

C.both a and b

D.neither a nor b

15.What is the molar mass of water, H2O?

A.18.02 g

B.18.02 amu

C.17.01 g

D.17.01 amu

16.What is the molar mass of glucose, C6H12O6?

A.180.2 amu

B.180.2 g

C.60.05 amu

D.60.05 g

17.In the reaction 2H2O → 2H2 + O2, 2.0 mol water will produce how many grams of O2?

32

64

16

36

18.In the reaction 2CH4 + O2 → 2CO + 4H2, how many molecules of CO will be produced by the complete reaction of 1.60 grams of CH4?

3.01 × 1022

2.00

12.0 × 1023

6.02 × 1022

19.Suppose 2.43 g of magnesium is reacted with 3.20 g of oxygen: 2Mg + O2 → 2MgO. How many grams of MgO will be produced?

1.27

4.03

5.63

8.06

20.Which of the following conversion factors would allow one to calculate the amount of PbI2produced from a given amount of NaI in the following unbalanced reaction?

Pb(NO3)2 + Nal → Pbl2 + NaNO3

a.

b.

c.

d.

21.The unbalanced equation for the reduction of copper(I) sulfide with oxygen is given below. What mass of copper is produced from the reduction of 7.50 g Cu2S?

Cu2S(s) + O2(g) Cu(s) + SO2(g)

18.8 g

5.99 g

1.50 g

9.39 g

2.99 g

22.How many grams of aluminum oxide are produced by the complete reaction of 19.8 g aluminum with excess oxygen?

10.5 g aluminum oxide

37.4 g aluminum oxide

49.9 g aluminum oxide

74.8 g aluminum oxide

23.If 5 grams of CO and 5 grams of O2 are combined according to the reaction, which is the limiting reagent?

2CO + O2 → 2CO2

O2

CO and O2

CO2

CO

24.In an industrial process, nitrogen is reacted with hydrogen to produce ammonia. The percent yield of this particular process is 26%. How much hydrogen is needed to produce 4.8 kg ammonia?

1.5 kg

7.0 kg

0.85 kg

3.3 kg

25.A percentage yield greater than 100% has been reported in a scientific paper you are assigned to read. What would be a reasonable explanation for this?

a. The product was measured more than once.

b. It must be a typographical error since yields can't exceed 100%.

c. A lack of training of the professor who published the study.

d. Small measurement errors could have caused this to occur.

26.In an industrial process, nitrogen is reacted with hydrogen to produce ammonia. The percent yield of this particular process is 24.8%. How much hydrogen is needed to produce 3.7 kg ammonia?

1.8 kg

1.2 kg

4.4 kg

12 kg

2.7 kg

27.The following reaction has a percent yield of 90.5%. How many grams of carbon dioxide are produced from 78.5 g calcium carbonate via this reaction?

2 HNO3(aq) + CaCO3(aq) Ca(NO3)2(aq) + H2O(l) + CO2(g)

34.5 g

21.6 g

38.1 g

31.2 g

28.When gas molecules dissolve in liquids to form a saturated system, the process is usually

exothermic.

endothermic.

independent of the nature of the liquid.

temperature independent.

29.The reaction below would be considered.

CaCO3 + heat → CaO + CO2

an exothermic combination.

an exothermic decomposition.

an endothermic combination.

an endothermic decomposition.

30.The combustion of one mole of propane, C3H8, releases 531 kcal. How much heat is released by the combustion of 1.20 moles of propane?

A.584 kcal

B.690 kcal

C.443 kcal

D.637 kcal

31.The combustion of one mole of propane, C3H8, releases 531 kcal. How much heat is released by the combustion of 4.40 g of propane?

A.531 kcal

B.5.31 × 104 kcal

C.53.1 kcal

D.5.31 × 103 kcal

32.Metabolism of one mole of glucose, C6H12O6, releases 670 kcal. How much heat is released by the combustion of 0.300 moles of glucose?

A.201 kcal

B.2.41 × 103 kcal

C.186 kcal

D.2.23 × 103 kcal

33.Metabolism of one mole of glucose, C6H12O6, releases 6.70 × 102 kcal. How much heat is released by the combustion of 50.0 g of glucose?

A.201 kcal

B.2.41 × 103 kcal

C.186 kcal

D.2.23 × 103 kcal

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