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Go to: Midterm I | Final Exam

Geochemistry (GLGY 323-UCAL) Midterm II

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Question 1

What is the term used to describe the intersection (highlighted in red)? (ID-GCM2-11)

A	Invariant point
B	Univariant point
C	Mating point
D	Reaction point
E	Interaction point

Question 2

The thermodynamic activity coefficient depends on which of the following? (ID-GCM2-12)
I. Pressure
II. Temperature
III. Composition of phase
IV. Atomic (nuclear) structure of compounds

A	I, III and IV only.
B	I, II and III only.
C	All of the above.
D	II and IV only.
E	I and II only.

Question 3

Under what criterion would you expect "marine snow" build up in the ocean? (ID-GCM2-18)

A	Environments with higher calcium carbonate dissolution rates and bellow the carbonate compensation depth.
B	Environments with higher calcium carbonate dissolution rates and above the carbonate compensation depth.
C	Environments with lower calcium carbonate dissolution rates and bellow the carbonate compensation depth.
D	Environments with lower calcium carbonate dissolution rates and above the carbonate compensation depth.
E	None of the answers are correct.

Question 4

Which of the following statement is correct about metastable equilibrium and/or stable equilibrium? (ID-GCM2-08)

A	It requires higher amount of energy to reach stable equilibrium than to reach metastable equilibrium.
B	Stable equilibrium can only be reached if the temperature and pressure of the system remain constant.
C	Metastable equilibrium only occurs exothermic reactions.
D	Metastable equilibrium is reached when the reaction is not at its lowest energy level.
E	Some chemical reactions do not have a stable equilibrium, hence they have Metastable equilibrium.

Question 5

What is the source of Fe in Banded Iron Formation (BIF)? (ID-GCM2-04)

A	Leaching of Fe from iron rich deposits and formations.
B	Dissolved Fe in ground water.
C	Oxidation of metallic deposits in the subsurface.
D	Fe in the atmosphere.
E	Underwater igneous activities.

Question 6

Oxidation of pure water will result in liberating ______. (ID-GCM2-01)

A	hydrogen, oxygen and electrons.
B	oxygen and electrons.
C	oxygen.
D	hydrogen.
E	oxygen and hydrogen.
F	hydrogen and electrons.

Question 7

Raoult's law of thermodynamics describes a relationship between which of the following? (ID-GCM2-16)

A	Temperature and the pressure required for a reaction to take place in a given environment.
B	Vapor pressure of pure components and its mole fraction.
C	Temperature and pressure changes as a function of time in a closed system.
D	Atomic mass of pure components and the possible reactions under given pressure.

Question 8

Mineral stability diagrams are typically derived for what standard state? (ID-GCM2-13)

A	25 degree Celsius, at 1 bar pressure
B	Temperature of 25 degree Celsius, at atmospheric pressure
C	100 degree Kelvin, at 10 bar pressure
D	273.15 degree Kelvin, at 10 bar pressure
E	100 degree Celsius, at 10 bar pressure

Question 9

Why is decrease in temperature result in increase in solubility of CaCO₃? Choose the best answer. (ID-GCM2-10)

A	Decrease in T result in increase in Gibbs Free Energy.
B	Concentration of CaCO3 in the surrounding environment is very low in low Ts.
C	Solubility is an exothermic reaction.
D	It results in net shift to the right on the phase diagram.

Question 10

Which of the following statement is correct? (ID-GCM2-07)

A	Change in one variable in thermodynamic reactions will impact all other remaining variables.
B	Thermodynamic phase diagram for calcite-aragonite has a negative slope.
C	Thermodynamic properties are constant for most solids.
D	Enthalpy change is sufficient to predict spontaneity of a reaction.
E	Thermodynamic properties are a function of temperature and pressure.

Question 11

What is Schreinemakers Analysis? (ID-GCM2-14)

A	A geometric approach to constructing phase diagrams based on averaging univariant reactions around an invarient point.
B	A empirical approach to constructing phase diagrams based on observable phase transitions.
C	An approach to constructing phase diagrams using a combination of empirical and theoretical analysis.
D	A geometric approach to constructing phase diagrams based on averaging invarient reactions around an univariant point.
E	A empirical approach to constructing phase diagrams under ideal pressure, temperature conditions.

Question 12

On activity-activity diagrams, which variables must be constant? (ID-GCM2-06)

A	Volume and Density
B	Density and Enthalpy
C	Temperature and Pressure
D	Enthalpy and Volume
E	Pressure and Volume

Question 13

What is the primary drive of chemical reactions? (ID-GCM2-09)

A	Free energy.
B	Atomic charge differences between molecules.
C	Atomic structures of chemical compounds.
D	Energy differences between systems.

Question 14

What is the equilibrium constant (K) equation for the following reaction? (ID-GCM2-15)
Fe₃Al₂Si₃O₁₂ + 3TiO₂ = 3FeTiO₃ + Al₂SiO₅ + 2SiO₂

A
B
C
D
E	None of the answers are correct.

Question 15

Which of the following statement is correct regarding saturation of CaCO₃ (calcium carbonate) in the ocean? (ID-GCM2-17)

A	Majority of the ocean floor has a coating of calcium carbonate.
B	Deepest parts of the ocean basins have the most concentration of calcium carbonates due to clam waters at higher depths.
C	Calcium carbonates dissolution increases with depth.
D	Modern marine organisms do not produce calcium carbonate based byproducts.

Question 16

Electromotive force describes which of the following? (ID-GCM2-02)

A	Concentration of hydronium ion.
B	Flow of electrons.
C	Amount of excess energy produced by a reaction.
D	Amount of force (energy) required to reach equilibrium.
E	Amount of energy used by a reaction.

Question 17

What is the primary cause of acid mine drainage? (ID-GCM2-05)

A	None of the answers are correct.
B	Exposed BIF after mining.
C	Acid rain.
D	Oxidation of pyrite.
E	Low oxygen concentrations in underground mines.

Question 18

What is the oxidizing agent in the following reaction? (ID-GCM2-03)
2Fe + 3Cl₂ --> 2Fe³⁺ + 6 Cl^-

A	Cl
B	Neither, since it is not a redox reaction.
C	Fe
D	Both Cl and Fe

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Credits: Based on the excellent class notes provided by, Dr. Rajeev Nair during Winter 2017 and textbook ISBN-978-1-444-35095-1.
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