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WorksheetsChemistry S2 Final Exam Review
Total questions: 50
Worksheet time: 25mins
1. Stoichiometry is:
the calculation of reactants and products in chemical reactions
the study of motion
the measurement of temperature
the process of distillation
Given 5.40 moles of hydrogen, how many moles of water would be produced? (Use the balanced equation: 2 H₂ + 1 O₂ → 2 H₂O)
5.40 moles H₂O
2.70 moles H₂O
10.8 moles H₂O
1.80 moles H₂O
Given 12.6 g of oxygen, how many grams of water would be produced? (Use the balanced equation: 2 H₂ + 1 O₂ → 2 H₂O)
14.2 g H₂O
8.4 g H₂O
25.2 g H₂O
6.3 g H₂O
What mass of aluminum oxide is produced when 3.65 g of aluminum react with iron(III) oxide?
6.89 g Al₂O₃
2.45 g Al₂O₃
10.12 g Al₂O₃
4.32 g Al₂O₃
Limiting reactant is defined as:
The reactant that is completely consumed in a chemical reaction, thus limiting the amount of product formed.
The reactant that is present in excess in a chemical reaction.
The product formed in the largest amount in a chemical reaction.
The substance that speeds up a chemical reaction without being consumed.
Identify the limiting reactant if 8.27 g of CO and 7.55 g of Fe₂O₃ react in the following equation. (solve for Fe) 3 CO + Fe₂O₃ → 2 Fe + 3 CO₂
Limiting reactant: CO; Theoretical yield of Fe: 4.90 g
Limiting reactant: Fe₂O₃; Theoretical yield of Fe: 8.20 g
Limiting reactant: CO; Theoretical yield of Fe: 7.55 g
Limiting reactant: Fe₂O₃; Theoretical yield of Fe: 4.90 g
The difference between actual yield and theoretical yield is:
Actual yield is always greater than theoretical yield.
Actual yield is the amount actually obtained, while theoretical yield is the maximum possible amount.
Theoretical yield is always less than actual yield.
There is no difference between actual yield and theoretical yield.
Determine the percent yield for the reaction between 26.13 g of NH₃ and 30.0 g of oxygen to produce nitrogen monoxide gas and unknown amounts of water.
83.6%
72.4%
91.2%
65.8%
Write complete electron configurations for the following elements. Chlorine
1s2 2s2 2p6 3s2 3p5
1s2 2s2 2p6 3s2 3p6
1s2 2s2 2p6 3s2 3p4
1s2 2s2 2p6 3s2 3p3
Write complete electron configurations for the following elements. Gold ____________________________________________
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d9
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d9 6p6
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p1
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d8 6p6
Write the abbreviated (Noble Gas) electron configuration for the following elements. Mg ____________________________________________
[Ne] 3s2
[He] 2s2 2p6 3s2
[Ar] 4s2
[Ne] 3p2
Write the abbreviated (Noble Gas) electron configuration for the following elements. Cs ____________________________________________
[Xe] 6s1
[Kr] 5s2 4d10 5p6 6s1
[Xe] 6s2
[Rn] 7s1
Ionic bonds and covalent bonds are formed by which of the following processes?
Transfer of electrons and sharing of electrons, respectively
Sharing of electrons and transfer of electrons, respectively
Both involve sharing of electrons
Both involve transfer of electrons
Valence electrons are:
the electrons in the outermost shell of an atom
the protons in the nucleus of an atom
the neutrons in the nucleus of an atom
the electrons in the innermost shell of an atom
How many valence electrons do each of the following elements have?
Mg: 2, O: 6, Ne: 8
Mg: 8, O: 2, Ne: 6
Mg: 6, O: 2, Ne: 8
Mg: 2, O: 8, Ne: 6
The Octet rule states that:
Atoms tend to gain, lose or share electrons to achieve eight electrons in their outermost shell.
Atoms always have eight protons in their nucleus.
Atoms combine to form molecules only when they have eight neutrons.
Atoms are stable with only two electrons in their outermost shell.
Which of the following Lewis dot diagrams correctly illustrates the formation of a compound between aluminum and fluorine?
Aluminum loses three electrons to three fluorine atoms, each fluorine gains one electron, forming AlF3.
Aluminum shares electrons equally with three fluorine atoms, forming AlF3.
Aluminum gains three electrons from three fluorine atoms, forming AlF3.
Aluminum and fluorine do not transfer electrons, forming a covalent bond.
Identify Mg3P2 as IONIC or COVALENT.
Ionic
Covalent
KCl is an example of which type of compound?
Ionic
Covalent
Metallic
Network Covalent
PH3 is an example of which type of compound?
Ionic
Covalent
A cation is formed when an atom ________ electrons, while an anion is formed when an atom ________ electrons.
gains; loses
loses; gains
shares; loses
shares; gains
Predict the charges on the ions formed by the following elements: Rb, Ra, Se, B, Kr, As.
Rb: +1, Ra: +2, Se: -2, B: +3, Kr: 0 (noble gas, typically does not form ions), As: -3
Rb: +2, Ra: +1, Se: -2, B: +3, Kr: 0, As: +3
Rb: +1, Ra: +2, Se: +2, B: -3, Kr: 0, As: -3
Rb: +1, Ra: +2, Se: -2, B: +3, Kr: -1, As: +5
The Ideal Gas Law is represented by which of the following equations, and what are the required units for its variables?
PV = nRT; Pressure in atm, Volume in liters, n in moles, R in L·atm/(mol·K), Temperature in Kelvin
PV = nRT; Pressure in Pa, Volume in m³, n in grams, R in J/(mol·K), Temperature in Celsius
PV = nRT; Pressure in mmHg, Volume in mL, n in moles, R in mmHg·L/(mol·K), Temperature in Fahrenheit
PV = nRT; Pressure in atm, Volume in liters, n in grams, R in L·atm/(mol·K), Temperature in Celsius
STP is defined as:
Standard Temperature and Pressure
Standard Time and Pressure
Standard Temperature and Power
Standard Time and Power
Convert 645 torr to atm.
645 torr = 0.849 atm (since 1 atm = 760 torr)
645 torr = 1.25 atm (since 1 atm = 760 torr)
645 torr = 0.567 atm (since 1 atm = 760 torr)
645 torr = 0.945 atm (since 1 atm = 760 torr)
Convert: 98 degrees Celsius = __________ Kelvin
371 Kelvin
273 Kelvin
198 Kelvin
400 Kelvin
A gas at a pressure of 806 mm Hg is held in a container with a volume of 736 cm³. The volume of the container is increased to 1276 cm³ without a change in temperature. What is the new pressure of the gas?
464 mm Hg
927 mm Hg
500 mm Hg
1400 mm Hg
What will the volume of a gas sample be at 245 K if its volume at 273 K is 5.77 liters?
5.18 liters
6.43 liters
4.92 liters
6.00 liters
A gas has a pressure of 1.25 atm and a volume of 236 ml. If the temperature is 44.0 degrees Celsius, how many moles of the gas do you have?
0.0121 moles (using the ideal gas law: PV = nRT)
0.0215 moles
0.0018 moles
0.120 moles
A mixture of 2 gases has a total pressure of 777 mmHg. If one of the gases has a pressure of 0.67 atm, what is the pressure of the second gas (in atm)?
0.35 atm (First convert 777 mmHg to atm: 777/760 = 1.022 atm. Then subtract 0.67 atm: 1.022 - 0.67 = 0.352 atm)
0.67 atm
1.02 atm
0.45 atm
A student adds ammonium chloride to a beaker with water. She touches the beaker and it feels cold. Is the reaction in the beaker endothermic or exothermic?
Endothermic
Exothermic
Neutral
Combustion
In an exothermic reaction, heat is ___________________________ from the system out to the surroundings.
released
absorbed
created
destroyed
What are examples of units of thermal energy (heat)?
Joules (J), calories (cal)
Watts (W), amperes (A)
Meters (m), liters (L)
Volts (V), ohms (Ω)
How many joules of heat are needed to raise the temperature of 35.0 grams of aluminum from 36°C to 67°C? The specific heat capacity of aluminum is 0.90 J/g°C?
972 J
450 J
1500 J
250 J
What was the change in temperature of the zinc?
5°C
10°C
15°C
20°C
In what part of the curve would the molecules of substance X be farthest apart? Closest together?
Farthest apart: Gas phase; Closest together: Solid phase
Farthest apart: Solid phase; Closest together: Gas phase
Farthest apart: Liquid phase; Closest together: Gas phase
Farthest apart: Solid phase; Closest together: Liquid phase
In what part of the curve would the molecules of X have the lowest kinetic energy? Highest kinetic energy?
Lowest kinetic energy: Solid phase; Highest kinetic energy: Gas phase
Lowest kinetic energy: Gas phase; Highest kinetic energy: Solid phase
Lowest kinetic energy: Liquid phase; Highest kinetic energy: Solid phase
Lowest kinetic energy: Gas phase; Highest kinetic energy: Liquid phase
Which phase changes are ENDOthermic? EXOthermic?
Endothermic: Melting, Vaporization, Sublimation; Exothermic: Freezing, Condensation, Deposition
Endothermic: Freezing, Condensation, Deposition; Exothermic: Melting, Vaporization, Sublimation
Endothermic: Melting, Freezing, Deposition; Exothermic: Vaporization, Condensation, Sublimation
Endothermic: Condensation, Deposition, Freezing; Exothermic: Melting, Sublimation, Vaporization
What type of reactions are shown below? Label each. Reactants → Products + heat ____________________ Reactants + heat → Products ____________________
Reactants → Products + heat: Exothermic Reactants + heat → Products: Endothermic
Reactants → Products + heat: Endothermic Reactants + heat → Products: Exothermic
Reactants → Products + heat: Combustion Reactants + heat → Products: Synthesis
Reactants → Products + heat: Decomposition Reactants + heat → Products: Neutralization
In a calorimetry lab, when a hot metal sample is placed into a calorimeter containing room temperature water, what is the direction of heat flow and what happens to the temperatures of the metal and the water?
Heat flows from the metal to the water; the metal cools down and the water heats up.
Heat flows from the water to the metal; the metal heats up and the water cools down.
No heat flows; both temperatures remain the same.
Heat flows both ways equally; both temperatures increase.
What is a solution?
A solution is a homogeneous mixture of two or more substances.
A solution is a pure element found in nature.
A solution is a type of chemical reaction.
A solution is a solid formed from two metals.
What is the difference between a solvent and a solute?
A solvent is the substance that dissolves the solute. The solute is the substance that is dissolved.
A solute is the substance that dissolves the solvent. The solvent is the substance that is dissolved.
A solvent and a solute are always the same substance in a solution.
A solvent is always a solid, while a solute is always a liquid.
At 25°C, the solubility of Compound X is 55 grams /100 grams of water. Identify each of the following solutions as unsaturated, saturated, or supersaturated: 38 grams of X dissolved in 100 grams of water
unsaturated
saturated
supersaturated
cannot be determined
At 25°C, the solubility of Compound X is 55 grams /100 grams of water. Identify each of the following solutions as unsaturated, saturated, or supersaturated: 27.5 grams of X dissolved in 50 grams of water
saturated
unsaturated
supersaturated
concentrated
What is the molarity of a 0.65 L solution containing 8.7 g NaCl in water?
0.23 M
0.38 M
0.15 M
0.45 M
How many grams of MgF₂ are in 625.0 mL of a 0.6 M solution of the solute?
23.0 g
15.0 g
28.5 g
34.2 g
Which of the following factors affect the rate at which a solute dissolves in a solvent?
Temperature, agitation, and particle size
Color and odor of the solute
Shape of the container
Type of stirring rod used
How would the following variables be affected when a solution is diluted?
Moles of solute: Remains the same; Liters of solvent: Increases; Molarity of solution: Decreases
Moles of solute: Increases; Liters of solvent: Remains the same; Molarity of solution: Increases
Moles of solute: Decreases; Liters of solvent: Decreases; Molarity of solution: Remains the same
Moles of solute: Remains the same; Liters of solvent: Decreases; Molarity of solution: Increases
What volume, in L, of 3.5M NaOH is required to prepare 6 L of 0.5 M NaOH?
0.86 L
1.2 L
2.5 L
3.0 L
If 335 ml of 6.0 M HNO₃ is diluted to 5.45 L, what is the molarity of the diluted solution?
0.37 M
0.21 M
0.62 M
0.12 M
