Chem II Final Exam

The energy of motion?

A.  Kinetic
B.  Potential

Stored energy?

A.  Kinetic
B.  Potential

Energy cannot be created or destroyed; it can only be converted from one form into another.

A.   3rd Law of Thermodynamics
B.   1st Law of Thermodynamics
C.   2nd Law of Thermodynamics

ΔE=E_final - E_initial

A.  Change in Time
B.  Change in Rate
C.  Change in Energy

Energy leaving the system.

A.  E_final > E_initial
B.  E_final < E_initial

Energy entering the system.


A.  E_final > E_initial
B.  E_final < E_initial

A function or property whose value depends only on the present state, or condition, of the system, not on the path used to arrive at that state.

F x d

PV work formula.

Enthalpy equation.

ΔH equals_____.

A.  Products - Reactants
B.  Reactants - Products

Internal energy formula.

Heat is represented by.

A.   w
B.   q
C.   V
D.   P

Energy is represented by.

A.   q
B.   w
C.   V
D.   E

The amount of heat required to raise the temperature of a certain object or amount by a certain temperature.

Heat capacity is represented by.

A.   V
B.   C
C.   q
D.   P

Heat capacity formula.

Specific heat formula.

The overall enthalpy change for a reaction is equal to the sum of the enthalpy changes for the individual steps.

For bond dissociation ΔH=______.

A.  Products - Reactants
B.  Reactants - Products

Spontaneous process happens when___

A.   ΔH is - and ΔS is -
B.   ΔH is - and ΔS is +
C.   ΔH is + and ΔS is -
D.   ΔH is + and ΔS is +

Nonspontaneous process happens when___

A.   ΔH is - and ΔS is +
B.   ΔH is + and ΔS is -
C.   ΔH is - and ΔS is -
D.   ΔH is + and ΔS is +

Free energy change formula.

When ΔG is < 0 then the process is______.

A.   nonspontaneous
B.   at equilibrium
C.   spontaneous

When ΔG is = 0 then the process is______.

A.   nonspontaneous
B.   at equilibrium
C.   spontaneous

When ΔG is > 0 then the process is______.

A.   spontaneous
B.   at equilibrium
C.   nonspontaneous

When a process proceeds on its own without and external influence.

Entropy change for a reaction is ΔS=_________.

A.  products - reactants
B.  reactants - products

Entropy change formula for ideal gas.

In any process, spontaneous or nonspontaneous, the total energy of a system and its surroundings is constant.

A.   1st Law of thermodynamics
B.   2nd Law of thermodynamics
C.   3rd Law of thermodynamics

In an spontaneous process, the total entropy of a system and its surroundings always increases.

A.   3rd Law of thermodynamics
B.   2nd Law of thermodynamics
C.   1st Law of thermodynamics

The entropy of a perfectly ordered crystalline substance at 0 K is zero.

A.   1st Law of thermodynamics
B.   3rd Law of thermodynamics
C.   2nd Law of thermodynamics

Formula for entropy change in the surroundings for a reaction.

Formula for relationship between ΔG and K.

Formula for free energy change under nonstandard conditions.

Formula for standard free energy of a reaction.

Rate Law.

Rate equals k

A.   zeroth order
B.   first order
C.   second order
D.   third order

Rate equals k[A]

A.   second order
B.   zeroth order
C.   third order
D.   first order

Rate equals k[A][B]

A.   first order
B.   second order
C.   zeroth order
D.   third order

Rate equals k[A][B]²

A.   third order
B.   second order
C.   first order
D.   zeroth order

Formula for half life of a first order reaction.

Equilibrium equation.

Mole of solute divided by liters of solution.

Equilibrium equation is______.

A.   reactants over products
B.   products over reactants
C.   unknown

Gas constant R equals____.

A.   0.05672
B.   0.08503
C.   0.08206

A substance that can transfer H⁺.

A substance that can accept H⁺.

H2O conjugate acid is?

HA conjugate base is?

NH3 conjugate acid is.

H2O conjugate base is.

Chemical species who formulas differs only by one proton are called.