Honors Chemistry Unit 2 Exam Review

Honors Chemistry Unit 2 Exam Review

Chm. 2.1 Understand the relationship among pressure, temperature, volume, and phase.

Chm. 2.2 Analyze chemical reactions in terms of quantities, product formation, and energy.

Chemistry 2.1

Chm.2.1.1 Explain the energetic nature of phase changes.

Chm.2.1.2 Explain heating and cooling curves (heat of fusion, heat of vaporization, specific heat, melting point, and boiling point).

Chm.2.1.3 Interpret the data presented in phase diagrams.

Chm.2.1.4 Infer simple calorimetric calculations based on the concepts of heat lost equals heat gained and specific heat.

Chm.2.1.5 Explain the relationships among pressure, temperature, volume, and quantity of gas, both qualitative and quantitative.

Multiple Choice

What would be the effect on the particles if more heat is supplied to the system?

• They would slow down
• They would stop moving
• They would speed up
• There would be no effect

Multiple Choice

Which statement is true for carbon dioxide at -60 °C?

• All three phases are possible.
• It can exist as a solid or a gas, depending on pressure.
• It is a solid.
• With enough pressure it can be melted.

Multiple Choice

What is point A?

• triple point
• critical point
• equilibrium point
• normal melting point

Multiple Choice

What change occurs from F to E?

• sublimation
• deposition
• melting
• condensation

Multiple Choice

What state of matter is X?

• solid 
• liquid
• gas
• supercritical fluid

Multiple Choice

Water exists as a _____________ at 700 mmHg and 50 °C.

• solid
• liquid
• gas
• supercritical fluid

Multiple Choice

What phase change(s) may occur at pressures below 4.58 mmHg?

• sublimation/deposition
• melting/freezing
• all phase changes are possible at these pressures
• vaporization/condensation

Multiple Choice

What happens to molecules when kinetic energy increases?

• they move slower
• they move faster
• they get heavier
• it depends on the types of molecules

Multiple Choice

What takes place when a solid changes to a liquid?

• condensation
• freezing
• melting
• evaporation

Multiple Choice

What takes place when a liquid changes to a solid?

• condensation
• melting
• evaporation
• freezing

Multiple Choice

What takes place when a liquid changes to a gas?

• condensation
• melting
• evaporation
• freezing

Multiple Choice

What takes place when a solid changes to a liquid?

• condensation
• melting
• evaporation
• freezing

Multiple Choice

From point A to point F, the sample is going through an __________ process by __________.

• exothermic, releasing heat to the surroundings

• exothermic, absorbing heat from the surroundings

• endothermic, releasing heat to the surroundings

• endothermic, absorbing heat from the surroundings

Multiple Choice

This curve indicates what about the heat energy?

• Heat energy is being added or absorbed

• Heat energy is being released

Chemistry 2.2

Chm.2.2.1 Explain the energy content of a chemical reaction.

Chm.2.2.2 Analyze the evidence of chemical change.

Chm.2.2.3 Analyze the law of conservation of matter and how it applies to various types of chemical equations (synthesis, decomposition, single replacement, double replacement, and combustion).

Chm.2.2.4 Analyze the stoichiometric relationships inherent in a chemical reaction.

Chm.2.2.5 Analyze quantitatively the composition of a substance (empirical formula, molecular formula, percent composition, and hydrates).

Multiple Choice

Describes the number of molecules in a compound and is used to balance a chemical reaction. 

• coefficient 
• subscript
• superscript
• SI unit

Multiple Choice

Which is the name of the kind of solid substance formed in this figure?  

• aqueous 
• precipitate
• acid
• synthesis 

Open Ended

What are evidences of a chemical reaction?

Multiple Choice

2H₂  +   O₂  →  2H₂O
How many moles of oxygen are consumed if 8 moles H₂ are used?

• 2
• 4
• 6
• 8

Multiple Choice

What is the molecular formula if the empirical formula is CH₂O and the molecular molar mass is 180.18?

• CH₂O
• C₂H₄O₂
• C₄H₈O₄
• C₆H₁₂O₆

Multiple Choice

2Na + 2H₂O → 2NaOH+ H₂
How many grams of hydrogen are produced if 120 g of Na are available?

• 5.2 g
• 2.6 g
• 690 g
• 45 g

Multiple Choice

CH₄ + 2 O₂ → CO₂ + 2 H₂O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH₄?

• 13.7 mol
• 2.75 mol
• 6.11 mol
• 6.85 mol

Multiple Choice

A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?

• Mg₄N₃
• MgN₂
• Mg₃N₂ 
• MgN

Multiple Choice

What is the percent composition by mass of oxygen in the compound MgSO₄ (gram formula mass = 120 g/mol)?

• 20%
• 27%
• 46%
• 53%

Multiple Choice

Which side of a chemical equation os the product side?

• Left (before the yields sign)
• Right (after the yields sign)

Multiple Choice

Which side of a chemical equation is the reactant side?

• Left (before the yields sign)
• Right (after the yields sign)

Multiple Choice

What is the arrow in a chemical equation...
H_{2 +} O --> H₂O

• Reactants
• Products 
• Yields 
• Chemical Equation 

Multiple Choice

Balance this equation:
MgCl₂ --> Mg₄+ Cl₂

• It's already balanced.
• 4MgCl₂ --> Mg₄+ 4Cl₂
• 4MgCl₂ --> Mg₄+ 5Cl₂

Multiple Choice

2 C₅H₅ + Fe ----> Fe(C₅H₅)₂

• Synthesis (or combination)
• Decomposition
• Single displacement
• Double displacement

Multiple Choice

SeCl₆ + O₂ ----> SeO₂ + 3Cl₂

• Synthesis (or combination)
• Decomposition
• Single displacement
• Double displacement

Multiple Choice

2 MgI₂ + Mn(SO₃)₂ ----> 2 MgSO₃ + MnI₄

• Synthesis (or combination)
• Decomposition
• Single displacement
• Double displacement

Multiple Choice

O₃  ----> O^. + O₂

• Synthesis (or combination)
• Decomposition
• Single displacement
• Double displacement