General Chemistry 1 - Chapter 9 and 11

The additional energy in a beaker of hot water compared to an otherwise identical beaker of room temperature water is......?

Thermal Energy

Fill in the blanks regarding energy flow:
If the reactants have ____________ internal energy than the products, ΔEsys is ______________, and energy flows out the system into the surroundings.

Higher, Negative

Identify the energy exchange (heat or work):
The fireman extinguishes the fire with foam and cools the environment (The foam is the system)

Heat

Identify the energy exchange (heat or work):
Steam condenses on skin, causing a burn (The condensing steam is the system)

Heat

Identify the energy exchange (heat or work):
A metal cylinder is rolled up a ramp (The metal cylinder is the system)

Work

Is the sign of work positive or negative?:
A metal cylinder is rolled up a ramp. (The metal cylinder is the system.)

Positive

Is the sign of heat positive or negative?:
The fireman extinguishes the fire with foam and cools the environment. (The foam is the system.)

Positive

Is the sign of heat positive or negative?:
Steam condenses on skin, causing a burn. (The condensing steam is the system.)

Negative

What are the expected sign of ΔEsys if ΔEsurr is positive? (Positive or Negative)

Negative

What are the expected sign of ΔEsurr if ΔEsys is negative? (Positive or Negative)

Positive

A _________________ (constant-volume calorimetry) is the laboratory equipment used to measure energy exchanges at constant volume between the system and the surroundings via temperature changes of the surroundings.

Bomb calorimeter

For data obtained using a bomb calorimeter (constant-volume calorimetry), what equation defines ΔErxn for a reaction?

ΔErxn = qv

The ____________ of a system is the sum of its internal energy and the product of its pressure and volume.

Enthalpy

Which of the following statements correctly describes the enthalpy change, ΔHrxn, for a reaction at constant pressure:
a.) state function
b.) given a negative sign when heat is absorbed
c.) numerically equal to qp

A and C

Determine whether the process is exothermic or endothermic:
Dry ice evaporating

Endothermic

Determine whether the process is exothermic or endothermic:
A sparkler burning

Exothermic

Determine whether the process is exothermic or endothermic:
The reaction the occurs in a chemical cold pack often used to ice athletic injuries

endothermic

Indicate the sign of ΔH (positive or negative):
Dry ice evaporating

Positive

Indicate the sign of ΔH (positive or negative):
A sparkler burning

Negative

Indicate the sign of ΔH (positive or negative):
The reaction the occurs in a chemical cold pack often used to ice athletic injuries

Positive

____________ is anything that has the capacity to do work

Energy

____________ is a force acting over a distance

work

____________ = Energy motion

Kinetic

____________ = stored energy

Potential

What is the first law of Thermodynamics?

Law of conservation of energy

What are the forms of energy?

electrical, heat or thermal , light or radiant, nuclear and chemical

What form of energy is described?
Kinetic energy associated with the flow of electrical charge

Electrical

What form of energy is described?
Kinetic energy associated with molecular motion (associated with molecular motion)

Heat or thermal

What form of energy is described?
Kinetic energy associated with energy transitions in an atom

Light or radiant

What form of energy is described?
Potential energy in the nucleus of atoms

Nuclear

What form of energy is described?
Potential energy in the attachment of atoms or because of their position (associated with position)

Chemical

What is the metric measurement of energy?

Joules

ΔEsys + ΔEsurr = ___________

E universe

What is a quantity that only depends on the initial and final conditions not on the process of path used?

state function

When the E system is negative, it means that the system __________ energy.

Lost

When the E system is positive, it means that the system __________ energy.

Gained

The ____________ _____________ is the temperature at which the solid becomes a liquid.

melting point

The _____________ ___________ is the temperature at which the liquid becomes a gas.

boiling point

_______________ ________________ is the pressure exerted by the gas phase in equilibrium with the liquid. It is often convenient to think of vapor pressure as a measure of how quickly a liquid evaporates.

Vapor Pressure

_____________ ______________ is a liquid's resistance to spread out and increase its surface area.

Surface tension

_________________ is a liquid's resistance to flow. For example, honey is more viscous than water.

Viscosity

What happens to the boiling point as the strength of intermolecular forces increases?

increases

What happens to the viscosity as the strength of intermolecular forces increases?

increases

What happens to the melting point as the strength of intermolecular forces increases?

increases

What happens to the surface tension as the strength of intermolecular forces increases?

increases

What happens to the vapor point as the strength of intermolecular forces increases?

decreases

In general, which of the following types of force/interaction is responsible for the existence of the condensed phases of matter?
a.) Covalent bond forces
b.) Ionic bond forces
c.) Intramolecular forces
d.) Intermolecular forces

d

Which state of matter has a definite shape?

solid

Which 2 factors cause transitions between the liquid and gas state?
a.) In general, an increase in pressure promotes the formation of a less dense phase.
b.) A liquid can be converted to a gas by cooling.
c.) A gas cannot be converted into a liquid by increasing the pressure of a gas sample.
d.) A liquid can be converted to a gas by heating.
e.) In general, an increase in pressure promotes the formation of a denser phase.

d and e

Which factors cause transitions between the solid and liquid state?
a.) A solid can be converted to a liquid by cooling.
b.) The increase in pressure of most liquids cannot lead to the transition to the solid phase.
c.) In general, an increase in pressure promotes the formation of a denser phase.
d.) A solid can be converted to a liquid by heating.
e.) In general, an increase in pressure promotes the formation of a less dense phase.

c and d

What are the key properties of liquids (in contrast to gases and solids)?
a.) Liquids have an indefinite shape and assume the shape of their container.
b.) Liquids are not easily compressed.
c.) Liquids have an indefinite shape and do not assume the shape of their container.
d.) Liquids are easily compressed.Liquids have lower densities in comparison to gases.
e.) Liquids have much higher densities in comparison to gases.

a, b and e

Which of the following is a characteristic of dispersion forces?
a.) Stronger dispersion forces result in lower boiling points
b.) A type of permanent dipole
c.) Stronger in linear molecules than spherical molecules of similar molar mass
d.) Found in only nonpolar substances

c

Which property of a liquid increases with increasing temperature?

Vapor Pressure

Which of the following changes will result in a net increase in the vapor pressure of a liquid in a beaker?
a.) Replacing the liquid with one with stronger intermolecular forces
b.) Decrease in surface area of the liquid
c.) Increase in temperature
d.) Adding more liquid to the beaker

c