NEW
Font size
WorksheetsGeneral Chemistry 2.1
Total questions: 50
Worksheet time: 56mins
Entropy is a measure of
accuracy
precision
the disorder of a system
the attraction of a nucleus for an electron
What phase of matter has the most entropy?
solid
liquid
gas
all of the above
What is a spontaneous process ?
slow process
fast process
process that needs an external intervention to occur
process that does not need external intervention to occur / keep happening
Reactions which do not produce the written products under the given conditions.
spontaneous
nonspontaneous
Spontaneous reactions may be extremely slow.
True
False
Nonspontaneous reactions may be extremely fast under the specified conditions.
True
False
Two factors that determine the spontaneity of a reaction are:
entropy and free energy
enthalpy and free energy
entropy and enthalpy
endothermic and exothermic
The entropy will usually increase when
a molecule is broken into two or more smaller molecules
a reaction occurs that results in an increase in the number of moles of gas
a solid changes to a liquid
all of these
Ammonium nitrate dissolves in water. It is a spontaneous endothermic process because the system undergoes....
a decrease in enthalpy
an increase in entropy
an increase in enthalpy
a decrease in entropy
Systems in nature tend to undergo changes toward
lower energy and less disorder
lower energy and more disorder
higher energy and less disorder
higher energy and more disorder
A reaction has a positive ΔH and a positive ΔS. Which of the following is true?
It will be spontaneous at all temperatures.
It will be nonspontaneous at all temperatures.
It will be spontaneous at low temperatures.
It will be spontaneous at high temperatures.
An ice cube is placed on a table and begins to melt. The following conclusion can be made.
Energy is being absorbed by the table which causes the cube to melt.
Energy is being transferred from the table to the ice cube.
Energy is being created by the air and table and making the cube heat up.
Energy is being created by the ice cube and is being released to the air
The _____ Law of Thermodynamics says that heat always flows from an object with a higher temperature to an object of lower temperature naturally
Zeroth
First
Second
Third
Entropy increases from solid, liquid to gas. Why?
Molecular disorder increases
Molecular randomness decreases
Molecules are more energetic
Molecules are more reactive
Two cups of water, one at 100oC and the other at 50oC are poured into a larger container. What would be the final temperature of the water?
Less than 50oC.
Greater than 100oC.
Between 50oC and 100oC.
The water temperature will rise and fall continually.
7. As water in a freezer turns into ice,
the water absorbs energy from the air in the freezer.
the water absorbs the coldness from the air in the freezer.
the freezer air absorbs heat from the water.
the water neither absorbs nor releases energy.
8. What causes water to freeze solid when placed in a freezer? The freezer–
adds heat to the water
puts electricity in the water
takes heat away from the water
does not let light shine on the water
Free energy is often expressed as Gibbs free energy.
True
False
Free energy is often expressed as Gibbs free energy.
True
False
Free energy can either be released or absorbed during a physical or chemical process
True
False
For the following reaction indicate if entropy is increased or decreased. 2 Li(s) + 2 H2O(l) ---->2 LiOH(s) + H2(g) + 213.0 kJ (Kilojoules)
increase
decrease
Which has a +ΔS (system)?
AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
H2O(g) + CO2(g) → H2CO3(aq)
H2(g) + I2(g) → 2Hl(g)
C2H2O2(g) → 2CO(g) + H2(g)
Given the following information, calculate ΔG0 for the reaction below at 250C: (K = 0C + 273)
SnCl4(l) + 2 H20(l) → SnO2(S) + 4HCl(g),
ΔH0=133.0 kJ and ΔS0 =401.5 J/K
-252.6 kJ
-13.4 kJ
13.4 kJ
252.6 kJ
At elevated temperatures ammonium carbonate, NH2COONH4, is in equilibrium with NH3 and CO2 according to the equation;
NH2COONH4(s) ↔ 2 NH3(g) + CO2(g)
What is the equilibrium expression for this reaction?
K = 2 [NH3][CO2]
[NH2COONH4]
K = [NH3]2[CO2]
[NH2COONH4]
K = 2 [NH3][CO2]
K = [NH3]2[CO2]
What is the equilibrium-constant expression for
CO2(g) + H2(g) ↔ CO(g) + H2O(l)
Kc= [CO][H2O] / [CO2][H2]
Kc= [CO2][H2] / [CO]
Kc= [CO2][H2] / [CO][H2O]
Kc= [CO] / [CO2][H2]
For the following reaction: H2(g) + Cl2 (g) ↔ 2HCl(g), calculate the concentration of HCl when Keq= 2.3x10-5, [H2]= 0.0056mol, [Cl2]= 0.0048mol.
6.2 x 10-10 M
2.5 x 10-5 M
1.1 M
1.2 M
Which of the following are equal for a chemical system at equilibrium?
The concentrations of reactants and products are equal
The rate constant for the forward and reverse reactions are equal
The time that a particular atom or molecule spends as a reactant and product are equal
The rate of the forward and reverse reaction
Which of the following is TRUE for a chemical reaction at equilibrium?
a. only the forward reaction stops
b. only the reverse reaction stops
d. the rate constant for the forward and backward reactions are equal
e. the rates of the forward and backward reactions are equal
Which of the following is TRUE regarding the concentration of products, for a chemical reaction that is already at equilibrium assuming no disruptions to the equilibrium?
The concentrations of products will not change because there are no more reactants.
The concentrations of products will not change because the limiting reagent is gone.
The concentrations of products will not change because the forward and reverse rates are equal
The concentrations of products will change continually because of reversibility.
A chemical equilibrium may be established by starting a reaction with ____________________.
reactants only
products only
any quantities of reactants and products
all of the above
An equilibrium that strongly favors products has ______________.
a value of K≪ 1
a value of K ≫1
a value of Q ≫1
a value of Q ≪ 1
The equilibrium constant for the acid ionization of mercaptoethanol is 1.91 * 10-10. The reaction is given by
HSCH2CH2OH (aq) H+(aq) + SCH2CH2OH- (aq)
Which of the following statements is true regarding this equilibrium?
I. The reaction is product favored.
II. The reaction is reactant favored
III. Equilibrium lies far to the right
IV. Equilibrium lies far to the left
I and III
I and IV
II and III
II and IV
The equilibrium constant for the formation of hydrogen iodide from iodine is 45 at a certain temperature.
H2 (g) + I2 (g) 2HI
Which of the following statements is true regarding this equilibrium?
I. The reaction is product favored.
II. The reaction is reactant favored
III. Equilibrium lies far to the right
IV. Equilibrium lies far to the left
a. I and III
b. I and IV
c. II and III
d. II and IV
If the reaction quotient Qc has a smaller value than the related equilibrium constant Kc, ______________________.
the reaction is at equilibrium
the reaction is not at equilibrium, and will make more products at the expense of the reactants
the reaction is not at equilibrium, and will make more reactants at the expense of the products
the value of Kc will decrease until it is equal to Q
If the reaction quotient Qc has a smaller value than the related equilibrium constant Kc, ______________________.
the reaction is at equilibrium
the reaction is not at equilibrium, and will make more products at the expense of the reactants
the reaction is not at equilibrium, and will make more reactants at the expense of the products
the value of Kc will decrease until it is equal to Q
If the equilibrium is established by initially adding 0.10 mol each of A and B to a 1L container, then which of the following must be true once the mixture achieves equilibrium?
A + 2B 2C Kc = 320
[A] = [B]
[A] = [B] = [C]
[B] = 2[C]
[A] > [B]
Which of the following is the correct equilibrium expression for the following reaction:
man + woman couple
Kc=[𝑚𝑎𝑛][𝑤𝑜𝑚𝑎𝑛][𝑐𝑜𝑢𝑝𝑙𝑒]
Kc=[𝑚𝑎𝑛]+ [𝑤𝑜𝑚𝑎𝑛][𝑐𝑜𝑢𝑝𝑙𝑒] [woman]
Kc = [man] [woman] [couple]
[𝑐𝑜𝑢𝑝𝑙𝑒][𝑚𝑎𝑛][𝑤𝑜𝑚𝑎𝑛]
Which of the following is the correct equilibrium expression for the following reaction assuming homogeneity:
fool (money)10 fool + 10money
a. Kc= [fool(money)10] [fool] [money]
b. Kc = [𝑓𝑜𝑜𝑙][𝑚𝑜𝑛𝑒𝑦]10[𝑓𝑜𝑜𝑙(𝑚𝑜𝑛𝑒𝑦)10]
c. Kc = [fool(money)10] [fool] [money]
d. Kc = [𝑓𝑜𝑜𝑙(𝑚𝑜𝑛𝑒𝑦)10]10[𝑓𝑜𝑜𝑙][𝑚𝑜𝑛𝑒𝑦]
For the following hypothetical equilibrium, what is the value of the equilibrium constant if the concentrations at equilibrium are shown as
A(g) + 2B(g) 2C(g)
when A = 4.5 * 10-5M; B = 2.2 * 10-2M; and C = 2.2 * 10-3M
0. 22
9.9
4.3 * 105
2.3 * 108
For the following hypothetical equilibrium, what is the value of the equilibrium constant if the concentrations at equilibrium are shown as
A(aq) + 2B(aq) 2C(aq) + D(aq)
when A = 4.5 * 10-5M; B = 2.2 * 10-2M; C=2.2 * 10-3M; and
D = 1.2 * 10-2M
52
32
67
49
All of the following are NOT seen in a equilibrium-constant expression EXCEPT _______ of the reacting species
amount
molar concentration
phase
molal concentration
If an acid is combined with a base of equal strength, the result will most likely be
a neutral solution.
a stronger acid.
impossible to tell without testing the pH.
a stronger base
Human blood has a pH between 7.35 and 7.45. Which of the following best describes human blood?
strongly acidic
slightly acidic
strongly basic
slightly basic
Buffer is defined as
ability to resist pH change
ability to prevent pH from decreasing
ability to resist a pH increase
ability to resist pH change when small amount of acid added
What might happen if buffers did not exist within the human body?
Our blood and other bodily fluids might become too acidic or basic.
Our stomach acid would not be able to break down food.
We would not be able to process glucose within our cells.
We would not be able to inhale oxygen into our lungs.
Why would a potato have a buffering system?
To survive if its environment changes
To vary the pH according to the environment
To keep the pH of the potato low
To keep the pH very acidic
Two beakers have liquids in them. When you add a base such as ammonia to beaker 1, the pH did not change. But when you add ammonia to beaker 2, the pH changes drastically. Choose the best explanation.
Beaker 1 had only water and Beaker 2 contained a buffer.
Beaker 1 contained a buffer and Beaker 2 contained only water.
Beaker 2 contained an acid.
The beaker that changed pH contained a buffer.
Which statement is true:
Mg → Mg2+ + 2e–
Mg gains 2 electrons
Mg2+ loses 2 electron
Mg loses 1 electron
Mg loses 2 electrons
Substance that oxidizes another substance by accepting its electrons.
oxidizing agent
reducing agent
combustion
all of the above
Reduction is the ___________ of electrons.
loss
gain
transfer
share
