The part of the universe that is of interest to us.
Heat transfer.
The part of the universe surrounding a reaction.
The universe.
Define the following term: surroundings.
A) / The part of the universe that is of interest to us.
B) / Heat transfer.
C) / The part of the universe surrounding the system.
D) / The universe.
Define the following term: potential energy.
A) / The energy available by virtue of an object's position.
B) / The energy associated with the random motion of atoms and molecules.
C) / The energy produced by a moving object
D) / The energy, which comes from the sun.
Define the following term: kinetic energy.
A) / The energy available by virtue of an object's position.
B) / The energy stored within the structural units of chemical substances.
C) / The energy produced by a moving object
D) / The energy, which comes from the sun.
Define the following term: law of conservation of energy.
A) / The capacity to do work.
B) / Directed energy change resulting from a process.
C) / The transfer of thermal energy between two bodies that are at different temperatures.
D) / The total quantity of energy in the universe is assumed constant.
Define the following term: thermochemistry.
A) / The study of heat change in chemical reactions
B) / The process of transferring thermal energy from a system to the surroundings.
C) / The process of transferring thermal energy from the surroundings to a system.
D) / The transfer of thermal energy between two bodies that are at different temperatures.
Define the following term: exothermic process.
A) / The study of heat change in chemical reactions
B) / The process of transferring thermal energy from a system to the surroundings.
C) / The process of transferring thermal energy from the surroundings to a system.
D) / The transfer of thermal energy between two bodies that are at different temperatures.
Define the following term: endothermic process.
A) / The study of heat change in chemical reactions
B) / The process of transferring thermal energy from a system to the surroundings.
C) / The process of transferring thermal energy from the surroundings to a system.
D) / The transfer of thermal energy between two bodies that are at different temperatures.
Think about what is meant by a state function. Give two examples of quantities that are state functions and two that are not.
A) / State functions: P,V; Not: work, energy
B) / State functions: energy, P; Not: T, heat
C) / State functions: energy, V; Not: work, heat
D) / State functions: energy, work; Not: T, heat
The following reaction takes place:
Hg(l) Hg(g)
Describe the work involved in this reaction. (No calculations are necessary.)
A) / Work is done by the system on the surroundings.
B) / Work is done by the surroundings on the system.
C) / No work is done.
Define the following term: enthalpy.
A) / Heat transfer at constant temperature.
B) / E + PV
C) / Heat flow under all conditions.
D) / Heat transfer at constant volume.
Consider the following data:
Metal / Al / Cu
Mass (g) / 10 / 30
Specific Heat (J/g°C) / 0.900 / 0.285
Temperature (°C) / 40 / 60
these two metals are placed in contact, which of the following will take place?
A) / Heat will flow from Al to Cu because Al has a larger specific heat.
B) / Heat will flow from Cu to Al because Cu has a larger mass.
C) / Heat will flow fro Cu to Al because Cu has a larger heat capacity.
D) / Heat will flow from Cu to Al because Cu is at a higher temperature.
E) / No heat will flow in either direction.
Which of these processes is endothermic?
A.O2(g) + 2H2(g) 2H2O(g)
B.H2O(g) H2O(l)
C.3O2(g) + 2CH3OH(g) 2CO2(g) + 2H2O(g)
D.H2O(s) H2O(l)
Which one of the following is an endothermic process?
A) ice melting
B) water freezing
C) boiling soup
D) Hydrochloric acid and barium hydroxide are mixed at 25 °C: the temperature increases.
E) Both A and C
ΔH for an endothermic process is ______while ΔH for an exothermic process is ______.
A) zero, positive
B) zero, negative
C) positive, zero
D) negative, positive
E) positive, negative
For the species in the reaction below, is zero for ______.
A) Co(s)
B)
C)
D)
E) both and
Answer the following:
1)During a chemical reaction, if the reaction was exothermic how would you be able to determine that without doing any calculations (using physical means)
a)If the reaction was endothermic
2)What is specific heat?
3)What is specific heat capacity?
4)What does Hess’s Law state?
5)What is the difference between a state function and a non-state function? Give an example of each.
6)What is internal energy? How can you change the internal energy of an object?
7)If you release 100 J of heat from the system to the surroundings, how much heat will be absorbed by the surroundings (more, less, or same)
8)What is temperature?
9)Heat is equal to enthalpy at a constant____?
10)All elements have a standard formation value of _____?
11)What does the first law of thermodynamics state?
12)What does enthalpy of reaction mean?
13)For Delta E to be positive a system ______energy and for a Delta E to be negative a system ____ energy
14)For q to be positive a system _____ heat and for q to be negative a system _____ heat
15)For w to be positive a system _____ and for w to be negative a system _____
16)What determines internal energy?
17)For internal energy to be positive what must happen
18)For internal energy to be negative what must happen
19)What is a state function. Give a few examples of state functions
20)What is the specific heat of water
21)Heat is always transferred from the ______object to the ______object
22)Enthalpy reactions always occur at a constant ______.
23)What is the difference between temperature and heat
24)What is the difference between specific heat and heat capacity?
25)What is the difference between heat of formation versus heat of reaction
26)