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Go to: Midterm I | Final Exam

Geochemistry (GLGY 323-UCAL) Midterm II

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Question 1

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

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

Question 2

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

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

Question 3

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

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

Question 4

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

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

Question 5

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

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

Question 6

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

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

Question 7

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

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

Question 8

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

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

Question 9

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

Question 10

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

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

Question 11

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

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

Question 12

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

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

Question 13

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

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

Question 14

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

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

Question 15

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

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

Question 16

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 17

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	Fe in the atmosphere.
C	Underwater igneous activities.
D	Oxidation of metallic deposits in the subsurface.
E	Dissolved Fe in ground water.

Question 18

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

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

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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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