Reaction Rates and Equilibrium Module Exam Practice Quiz

Which of the following best explains why the sand at the beach feels hotter than the water on a sunny day?

• Sand has a lower specific heat capacity than water, so it heats up more quickly.

• Sand reflects more sunlight than water, causing it to absorb more heat.

• Water conducts heat better than sand, making the sand retain less heat.

• Water absorbs heat faster than sand but cools down just as quickly.

Tags

NGSS.HS-PS3-4

How much heat is transferred when a 30.0 g sample of a substance is cooled from 45.0°C to -5.0°C? The specific heat capacity of the substance is 0.850 J/g·°C.

Use the equation: q = m ⋅ c ⋅ ΔT

What is the temperature change when 350 J of heat is transferred to a 12.0 g sample of a metal? The specific heat capacity of the metal is 0.640 J/g·°C.

Use the equation: q = m ⋅ c ⋅ ΔT

Tags

NGSS.HS-PS3-4

Enthalpy is the measure of the ________________ of a system.

• energy

• volume

• temperature

• pressureenthalpy

Tags

NGSS.HS-PS3-1

How can you measure enthalpy?

• By calculating the starting enthalpy of a system before a change

• By calculating the total enthalpy of a system

• By calculating the enthalpy change experienced in a system

• By calculating the ending enthalpy of a system after a change

Tags

NGSS.HS-PS3-1

What type of reaction is represented by this graph?

• Endothermic

• Exothermic

• Reversible

• Decomposition

Tags

NGSS.HS-PS1-4

A chemical reaction starts with reactants that contain 950 kJ of energy, and the products contain only 720 kJ of energy.

Determine if this reaction is endothermic or exothermic using the equation: ΔH = ΣH_products - ΣH_reactants

• Endothermic, ΔH = +230 kJ

• Exothermic, ΔH = -230 kJ

• Endothermic, ΔH = -230 kJ

• Exothermic, ΔH = +230 kJ

Tags

NGSS.HS-PS3-1

What is entropy?

• The measurement of the heat in a system

• The measurement of energy in a system

• The measurement of the disorder in a system

• The measurement of pressure in a system

Tags

NGSS.HS-PS3-4

Which of the following processes represents a decrease in entropy?

• Ice melting into liquid water

• Water vapor condensing into liquid water

• A solid dissolving into a solution

• A gas expanding to fill a larger container

Which of the following correctly identifies and describes the Gibbs free energy of this reaction at 300 K?

CO _(g) + O2 _(g) ↔ CO_{2 (g)}

The enthalpy change (ΔH) of this reaction is -393.5 kJ/mol, and the entropy change (ΔS) is -0.214 kJ/(mol·K)

Use the equation ΔG=ΔH−TΔS to solve

• ΔG = −329.2 kJ/mol, reaction is nonspontaneous

• ΔG = −329.2 kJ/mol, reaction is spontaneous

• ΔG = −429.7 kJ/mol, reaction is spontaneous

• ΔG = −429.7 kJ/mol, reaction is nonspontaneous