WorksheetsGroup Radon Units 7, 3.10, 3.13 Review
Total questions: 52
Worksheet time: 40mins
True or False: When a system reaches equilibrium, do the rates of forward and reverse reactions equal zero?
True
False
Which of the following could be an appropriate title for the y-axis?
Concentration
Rate
Partial Pressure
Time
Which of the following could be an appropriate title for the y-axis?
Concentration
Rate
Partial Pressure
Time
From the left flask to the right flask, which of the following best describes the changes in the system over time?
The system is at equilibrium, then there is an increase in the evaporation rate.
The condensation rate is greater than the evaporation rate, then the system reaches equilibrium.
The evaporation rate is greater than the condensation rate, then the system reaches equilibrium.
The system is at equilibrium in both flasks.
Dynamic Equilibrium is defined as the state “wherein the rates of the forward and reverse reactions are ______.”
Reciprocals
Zero
Inverse
Equal
Dynamic Equilibrium is defined as the state wherein the net change in concentration (or partial pressure) is _______.
Reciprocals
Zero
Inverse
Equal
If the rate of the forward reaction exceeds the reverse reaction, more (a) will be produced.
If the rate of the reverse reaction exceeds the forward reaction, Q (a) K.
Which chemical will not be factored into the Reaction Quotient?
H2(g)
CO2(g)
H2O (l)
CO(g)
What could a Reaction Quotient of zero tell us about a reaction?
There are only reactants in the system
There are only products in the system
The system is at equilibrium
There are both products and reactants in the system, but the system is not at equilibrium
Do we need to know how to convert from KC to KP?
Of course! We need to know all there is to know about chemistry!
That is impossible.
Not on the test, don’t need to know it.
Yes, or else Mr. Carmody will yell at you.
Which of the following is the Equilibrium Constant for the reaction below?
Consider the following reaction: CO (g) + 2H2 (g) → CH3OH (g). With initial concentrations of [CO] = 0.27 M and [H2] = 0.49, and equilibrium concentration of [CH3OH] = 0.11 M, find the equilibrium constant (Assume constant temperature).
15.9
16.1
118.9
9.4
Which of the following assessments regarding the two statements below accurately explains Beer’s Law:
I. The equation for Beer’s Law is A=εBC
BECAUSE
II. As the concentration of a solution increases, the solution blocks more light
I is TRUE and II is FALSE.
I is FALSE and II is TRUE.
Both I and II are true, but II is not the proper justification for I.
Both I and II are true, and II is a proper justification for I.
A solution’s color and lightwave’s color must be (a) in order to optimize absorbance.
A reaction has ∆H = -36 kJ and ∆S= -58 J/K. At what temperatures is it non-spontaneous?
982 J
593 J
236 J
1.82 kJ
Which of the following is true?
A standard state free energy of reaction equation can only be used under set circumstances
A large magnitude of △G indicates the reaction is close to equilibrium
In the event △H0 < 0 and △S0 > 0 or △H0 >0 and △S0 < 0, the reaction is favored by both entropy and enthalpy so there is no need to proceed with △G0 calculations
Entropy can be modeled by the equation:
△STotal = △SSurroundings + △SSystem
A spontaneous reaction will have △G (a) 0.
For an ongoing reaction Q < K. What will the numerical value of △G be?
△G > 0
△G < 0
△G = 0
There is not enough information to answer the question
No more Gibb's Free Energy questions!
Which of the following is an accurate assessments of the following two statements?
I. The solubility of a salt is strongly dependent on pH and other dissolved ions in the environment
BECAUSE
II. Anions formed from the dissolution of sparingly double acids and acidic salts will react with water to form OH- and a weak base.
I is TRUE and II is FALSE.
I is FALSE and II is TRUE.
Both I and II are true, but II is not the proper justification for I.
Both I and II are true, and II is a proper justification for I.
Which of the following is true?
A more acidic (or lower) pH will have a high solubility of sparingly double bases and basic salts
A more acidic (or lower) pH will have a low solubility of sparingly double bases and basic salts
Which of the following dissolved into a solution will result in the highest solubility of sparingly double bases and basic salts
HNO2
HF
HCN
HI
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Which of the following will dissolve in water?
AgI
CaSO4
CaS
PbBr
Why is paraffin wax not dissolvable in water.
Paraffin wax is an overall non-polar molecule
Paraffin wax is an overall polar molecule
Paraffin wax contains hydrogen bonds.
…because it's wax.
What is the formula for the solubility product constant of the reaction shown?
Ksp = [AgCl][Cl-]
Ksp = [Ag+][Cl-]
Ksp = [Ag+][AgCl]
Ksp = [Ag+][Cl-] / [AgCl]
For Zn(OH)2 the Ksp is 7.7 x 10-17. Calculate the solubility.
(a)
Write the equation for the dissociation of CaCl2 in water.
CaCl2(s) ----> Ca2+(aq) + 2Cl-(aq)
H2O(l) + CaCl2(s) ----> Ca2+(aq) + 2Cl-(aq) + OH-(aq)
H2O(l) + CaCl2(s) ----> Ca2+(aq) + 2Cl-(aq) + H2O(l)
CaCl2(s) ----> Ca2+(aq) + Cl- (aq)
If the equilibrium constant is much greater than one (K >> 1) then:
Equilibrium is not established.
Equilibrium lies to the right (products are favored)
Equilibrium lies to the left (reactants are favored)
Neither products or reactants are favored.
If the equilibrium constant is much less than one (K << 1) then:
Equilibrium is not established.
Equilibrium lies to the right (products are favored)
Equilibrium lies to the left (reactants are favored)
Neither products or reactants are favored.
If the reaction A + B ⇌ C is inverted, what is the exact value of K?
[C]/[A][B]
[A][B]/[C]
Log(C)-(A+B)
Log(AB)-(C)
If the reaction is raised to the second power what is the value of K?
√K
K^2
2K
In a reaction where the Q > K…
Products are favored
Reactants are favored
Products and reactants are equal
Products and reactants are not affected
If Q = K the reaction is at equilibrium.
True
False
What is needed to find the partial pressure of a substance in a reaction?
Balanced equation
Balanced equation AND Initial Conc.
Balanced equation, K value AND Initial Conc.
Balanced equation, K value, Change in H AND Initial Conc.
In the reversible reaction A + B ⇌ C + 10KJ, If more energy is added in the form of heat…
K increases
K decreases
Q increases
Q decreases
If a catalyst is added to a reversible reaction…
Increase product Conc.
Increase Reactant Conc.
Conc. does not change
What is the common ion effect?
When the addition of an ion common to two solutes causes precipitation or reduces ionization.
When the subtraction of an ion common to two solutes causes precipitation or reduces ionization.
When a molecule is added to a solution and causes precipitation or reduces ionization.
The effect of adding ions to a solution.
Given the equilibrium present in the saturated solution:
BaCO3(s) -> Ba2+(aq) + CO32-
(aq)
How would the addition of addition barium ions to the solution affect the amount of solid barium carbonate present?
The amount of BaCO3 would stay the same.
It would depend on the specific barium compound that was added.
The amount of BaCO3(s) would decrease.
The amount of BaCO3(s) would increase.
Which reversible reactions are occurring?
H2O + H2O ⇌ (H3O+) + (HO-)
H2O(l) ⇌ H2O(g)
H2O + H2O ⇌ (H3O+) + (HO-) AND H2O(l) ⇌ H2O(g)
What is Le Chatelier's Principle?
An element is the simplest form of matter that can exist under conditions that we find in a chemical laboratory.
Bonds are forces that hold atoms in their places.
Atoms are the smallest divisible components of matter that have the same properties which differ from the properties of other elements.
If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
What is the Ksp expression for Cu3(PO4)2?
Ksp = [Cu+2]3[PO4-3]2
Ksp = [Cu+2]2[PO4-3]3
Ksp = [Cu+2][PO4-3]
Ksp = [Cu+2]3[PO4-3]
A substance that ionizes completely in solution is...
an insulator.
a strong electrolyte.
a weak acid.
a non-electrolyte.
If Ksp < Qsp then...
no precipitate will form
precipitate will form
the reaction will not occur
the reaction will remain saturated
For the reaction...SO2 + O2 <−> SO3 If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.
Left
Right
left and right
neither left nor right
For the reaction… SO2 + O2 <−> SO3 If the equilibrium shifts to the right, the concentration of O2 will ___________.
Increase
Decrease
remain the same
Double
For the reaction… H2(g) + Cl2(g) <−> 2HCl(g) + heat. If the temperature is cooled, the _________ reaction will be favored.
Forward
Reverse
forward and reverse
For the reaction… N2(g) + 3 H2(g) <−> 2NH3(g). If the pressure in the system is increased by adding helium gas, _______ reaction will be favored.
the forward
the reverse
neither
For the reaction… N2(g) + 3H2(g) <−> 2NH3(g). If the pressure in the system is increased by reducing the volume of the container, which substance(s) will increase in concentration?
N2
H2
N2 and H2
NH3
Kc for the reaction can be written as...
Kc = [NO2]2/[N2O4]1
Kc = [N2O4]1/[NO2]2
Kc = [NO2]/[N2O4]
Kc = [N2O4]/[NO2]
Which of the following is FALSE about Qc and Kc?
Qc reaction quotient at a particular time and varies over time
Kc is equilibrium constant, which is fix at a fixed temp
Qc will eventually equal to Kc over time
Qc does not change
What will happen when Qc is less < than Kc?
Equilibrium is disturbed
Equilibrium contain more products than reactants
Equilibrium will shift to the right to increase Qc
Equilibrium will shift to the left to decrease Qc
