NEW
Font size
S
M
L
XL
WorksheetsKinetics and Equilibrium TICKET
Total questions: 53
Worksheet time: 27mins
Name
Class
Date
1.
Which list of the phases of H2O is arranged in order of increasing entropy?
a)
ice, steam, and liquid water
b)
ice, liquid water, and steam
c)
steam, liquid water, and ice
d)
steam, ice, and liquid water
2.
An open flask is half filled with water at 25oC. Phase equilibrium can be reached after
a)
more water is added to the flask
b)
the flask is stoppered
c)
the temperature is decreased to 15oC
d)
the temperature is increased to 35oC
3.
Given the equation for a system at equilibrium:
N2(g) + 3H2(g) <--> 2NH3(g) + energy
If only the concentration of N2(g) is increased, the concentration of
N2(g) + 3H2(g) <--> 2NH3(g) + energy
If only the concentration of N2(g) is increased, the concentration of
a)
NH3(g) increases
b)
NH3(g) remains the same
c)
H2(g) increases
d)
H2(g) remains the same
4.
Given the reaction at equilibrium:
C2 + D2(g) <-->2 CD(g) + energy
Which change will cause the equilibrium to shift?
C2 + D2(g) <-->2 CD(g) + energy
Which change will cause the equilibrium to shift?
a)
increase in pressure
b)
increase in volume
c)
addition of heat
d)
addition of a catalyst
5.
Given the accompanying potential energy diagram for a reaction:
Which interval on this diagram represents the difference between the potential energy of the products and the potential energy of the reactants?
Which interval on this diagram represents the difference between the potential energy of the products and the potential energy of the reactants?
a)
1
b)
2
c)
3
d)
4
6.
A sample of helium gas is in a sealed, rigid container. What occurs as the temperature of the sample is increased?
a)
The mass of the sample decreases
b)
The number of moles of gas increases.
c)
The volume of each atom decreases.
d)
The frequency of collisions between atoms increases.
7.
Given the equation representing a reaction at equilibrium:
2SO2(g) + O2(g) <--> 2SO3(g) +HEAT
Which change causes the equilibrium to shift to the right?
2SO2(g) + O2(g) <--> 2SO3(g) +HEAT
Which change causes the equilibrium to shift to the right?
a)
adding a catalyst
b)
adding more O2(g)
c)
decreasing the pressure
d)
increasing the temperature
8.
Given the potential energy diagram for a chemical reaction:
(see image)
Which numbered interval represents the heat of reaction?
(see image)
Which numbered interval represents the heat of reaction?
a)
1
b)
2
c)
3
d)
4
9.
The solid and liquid phases of water can exist in a state of equilibrium at 1 atmosphere of pressure and a temperature of
a)
0oC
b)
100oC
c)
273oC
d)
373oC
10.
In most aqueous reactions as temperature increases, the effectiveness of collisions between reacting particles
a)
decreases
b)
increases
c)
remains the same
11.
Based on the nature of the reactants in each of the equations below, which reaction at 25°C will occur at the fastest rate?
a)
C(s) + O2(g) --> CO2(g)
b)
NaOH(aq) + HCl(aq) --> NaCl(aq) + H2O(l)
c)
CH3OH(l) + CH3COOH(l) --> CH3COOCH3(aq) + H2O(l)
d)
CaCO3(s) --> CaO(s) + CO2(g)
12.
At STP, which 4.0-gram zinc sample will react fastest with dilute hydrochloric acid?
a)
lump
b)
bar
c)
powdered
d)
sheet metal
13.
According to Table I, which equation represents a change resulting in the greatest quantity of energy released?
a)
2C(s) + 3H2(g) --> C2H6(g)
b)
2C(s) + 2H2(g) --> C2H4(g)
c)
N2(g) + 3H2(g) --> 2NH3(g)
d)
N2(g) + O2(g) --> 2NO(g)
14.
Which information about a chemical reaction is provided by a potential energy diagram?
a)
the oxidation states of the reactants and products
b)
the average kinetic energy of the reactants and products
c)
the change in solubility of the reacting substances
d)
the energy released or absorbed during the reaction
15.
Given the equation representing a reaction:
N2O4(g) <--> 2NO2(g)
Which statement describes this reaction at equilibrium?
N2O4(g) <--> 2NO2(g)
Which statement describes this reaction at equilibrium?
a)
The concentration of N2O4(g) must equal the concentration of NO2(g).
b)
The concentration of N2O4(g) and the concentration of NO2(g) must be constant.
c)
The rate of the forward reaction is greater than the rate of the reverse reaction.
d)
The rate of the reverse reaction is greater than the rate of the forward reaction.
16.
A chemical reaction between iron atoms and oxygen molecules can only occur if
a)
the particles are heated
b)
the atmospheric pressure decreases
c)
there is a catalyst present
d)
there are effective collisions between the particles
17.
Given the potential energy diagram and equation representing the reaction between substances A and D: (see accompanying diagram)
According to Table I, substance G could be
According to Table I, substance G could be
a)
HI(g)
b)
H2O(g)
c)
CO2(g)
d)
C2H6(g)
18.
Given the equation representing a system at equilibrium:
N2(g) + 3H2(g) <--> 2NH3 (g) + ENERGY
Which changes occur when the temperature of this system is decreased?
N2(g) + 3H2(g) <--> 2NH3 (g) + ENERGY
Which changes occur when the temperature of this system is decreased?
a)
The concentration of H2(g) increases and the concentration of N2(g) increases.
b)
The concentration of H2(g) decreases and the concentration of N2(g) increases.
c)
The concentration of H2(g) decreases and the concentration of NH3(g) decreases.
d)
The concentration of H2(g) decreases and the concentration of NH3(g) increases.
19.
Given the equation representing a closed system:
N2O4(g) <--> 2NO2(g)
Which statement describes this system at equilibrium?
N2O4(g) <--> 2NO2(g)
Which statement describes this system at equilibrium?
a)
The volume of the NO2(g) is greater than the volume of the N2O4(g).
b)
The volume of the NO2(g) is less than the volume of the N2O4(g).
c)
The rate of the forward reaction and the rate of the reverse reaction are equal.
d)
The rate of the forward reaction and the rate of the reverse reaction are unequal.
20.
In a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is equal to the
a)
activation energy
b)
kinetic energy
c)
heat of reaction
d)
rate of reaction
21.
Changes in activation energy during a chemical reaction are represented by a
a)
cooling curve
b)
heating curve
c)
ionization energy diagram
d)
potential energy diagram
22.
Given the balanced equation representing a reaction:
2H2O(l) + 571.6 kJ → 2H2(g) + O2(g)
What occurred as a result of this reaction?
2H2O(l) + 571.6 kJ → 2H2(g) + O2(g)
What occurred as a result of this reaction?
a)
Energy was absorbed, and entropy increased.
b)
Energy was absorbed, and entropy decreased.
c)
Energy was released, and entropy increased.
d)
Energy was released, and entropy decreased.
23.
Given the potential energy diagram representing a reversible reaction:
The activation energy for the reverse reaction is represented by
The activation energy for the reverse reaction is represented by
a)
A + B
b)
B + C
c)
B + D
d)
C + D
24.
Which term is defined as a measure of the disorder of a system?
a)
heat
b)
entropy
c)
kinetic energy
d)
activation energy
25.
Systems in nature tend to undergo changes toward
a)
lower energy and lower entropy
b)
lower energy and higher entropy
c)
higher energy and lower entropy
d)
higher energy and higher entropy
26.
A 1.0-gram piece of zinc reacts with 5 milliliters of HCl(aq). Which of these conditions of concentration and temperature would produce the greatest rate of reaction?
a)
1.0 M HCl(aq) at 20.oC
b)
1.0 M HCl(aq) at 40.oC
c)
2.0 M HCl(aq) at 20.oC
d)
2.0 M HCl(aq) at 40.oC
27.
Which expression represents the ΔH for a chemical reaction in terms of the potential energy, PE, of its products and reactants?
a)
PE of products + PE of reactants
b)
PE of products - PE of reactants
c)
PE of products × PE of reactants
d)
PE of products ÷ PE of reactants
28.
Which factors must be equal in a reversible chemical reaction at equilibrium?
a)
the activation energies of the forward and reverse reactions
b)
the rates of the forward and reverse reactions
c)
the concentrations of the reactants and products
d)
the potential energies of the reactants and products
29.
A 5.0-gram sample of zinc and a 50.-milliliter sample of hydrochloric acid are used in a chemical reaction. Which combination of these samples has the fastest reaction rate?
a)
a zinc strip and 1.0 M HCl(aq)
b)
a zinc strip and 3.0 M HCl(aq)
c)
zinc powder and 1.0 M HCl(aq)
d)
zinc powder and 3.0 M HCl(aq)
30.
For a given reaction, adding a catalyst increases the rate of the reaction by
a)
providing an alternate reaction pathway that has a higher activation energy
b)
providing an alternate reaction pathway that has a lower activation energy
c)
using the same reaction pathway and increasing the activation energy
d)
using the same reaction pathway and decreasing the activation energy
31.
Given the equation representing a reaction at equilibrium:
N2(g) + 3H2(g) <--> 2NH3(g) + ENERGY
Which change causes the equilibrium to shift to the right?
N2(g) + 3H2(g) <--> 2NH3(g) + ENERGY
Which change causes the equilibrium to shift to the right?
a)
decreasing the concentration of H2(g)
b)
decreasing the pressure
c)
increasing the concentration of N2(g)
d)
increasing the temperature
32.
At 20.oC, a 1.2-gram sample of Mg ribbon reacts rapidly with 10.0 milliliters of 1.0 M HCl(aq). Which change in conditions would have caused the reaction to proceed more slowly?
a)
increasing the initial temperature to 25oC
b)
decreasing the concentration of HCl(aq) to 0.1 M
c)
using 1.2 g of powdered Mg
d)
using 2.4 g of Mg ribbon
33.
Adding a catalyst to a chemical reaction results in
a)
a decrease in activation energy and a decrease in the reaction rate
b)
a decrease in activation energy and an increase in the reaction rate
c)
an increase in activation energy and a decrease in the reaction rate
d)
an increase in activation energy and an increase in the reaction rate
34.
Given the potential energy diagram of a chemical reaction: . . . (see image)
Which arrow represents the potential energy of the reactants?
Which arrow represents the potential energy of the reactants?
a)
A
b)
B
c)
C
d)
D
35.
Given the reaction at equilibrium:
2SO2(g) +O2(g) <--> 2SO3(g) + HEAT
Which change will shift the equilibrium to the right?
2SO2(g) +O2(g) <--> 2SO3(g) + HEAT
Which change will shift the equilibrium to the right?
a)
increasing the temperature
b)
increasing the pressure
c)
decreasing the amount of SO2(g)
d)
decreasing the amount of O2(g)
36.
What occurs when the temperature is increased in a system at equilibrium at constant pressure?
a)
The rate of the forward reaction increases, and the rate of the reverse reaction decreases.
b)
The rate of the forward reaction decreases, and the rate of the reverse reaction increases.
c)
The rate of the endothermic reaction increases.
d)
The rate of the exothermic reaction decreases.
37.
Which process is accompanied by a decrease in entropy?
a)
boiling of water
b)
condensing of water vapor
c)
subliming of iodine
d)
melting of ice
38.
A catalyst is added to a system at equilibrium. If the temperature remains constant, the activation energy of the forward reaction
a)
. decreases
b)
increases
c)
remains the same
39.
Given the reaction at 25oC:
Zn(s) + 2 HCl(aq) --> ZnCl2(aq) + H2(g)
The rate of this reaction can be increased by using 5.0 grams of powdered zinc instead of a 5.0-gram strip of zinc because the powdered zinc has
Zn(s) + 2 HCl(aq) --> ZnCl2(aq) + H2(g)
The rate of this reaction can be increased by using 5.0 grams of powdered zinc instead of a 5.0-gram strip of zinc because the powdered zinc has
a)
lower kinetic energy
b)
lower concentration
c)
more surface area
d)
more zinc atoms
40.
Which statement about a system at equilibrium is true?
a)
The forward reaction rate is less than the reverse reaction rate.
b)
The forward reaction rate is greater than the reverse reaction rate.
c)
The forward reaction rate is equal to the reverse reaction rate.
d)
The forward reaction rate stops and the reverse reaction rate continues.
41.
The activation energy required for a chemical reaction can be decreased by
a)
increasing the surface area of the reactant
b)
increasing the temperature of the reactant
c)
adding a catalyst to the reaction
d)
adding more reactant
42.
A catalyst increases the rate of a chemical reaction by
a)
lowering the activation energy of the reaction
b)
. lowering the potential energy of the products
c)
raising the temperature of the reactants
d)
raising the concentration of the reactants
43.
A solution that is at equilibrium must be
a)
concentrated
b)
dilute
c)
saturated
d)
unsaturated
44.
Given the reaction:
N2(g) +O2(g) +182.6 KJ <--> 2 NO(g)
Which change would cause an immediate increase in the rate of the forward reaction?
N2(g) +O2(g) +182.6 KJ <--> 2 NO(g)
Which change would cause an immediate increase in the rate of the forward reaction?
a)
increasing the concentration of NO(g)
b)
increasing the concentration of N2(g)
c)
decreasing the reaction temperature
d)
decreasing the reaction pressure
45.
Which 10-milliliter sample of water has the greatest degree of disorder?
a)
H2O(g) at 120°C
b)
H2O(l) at 80°C
c)
H2O(l) at 20°C
d)
H2O(s) at 0°C
46.
Which statement must be true about a chemical system at equilibrium?
a)
The forward and reverse reactions stop.
b)
The concentration of reactants and products are equal.
c)
The rate of the forward reaction is equal to the rate of the reverse reaction.
d)
The number of moles of reactants is equal to the number of moles of product.
47.
A closed container holds 3.0 moles of CO2 gas at STP. What is the total number of moles of Ne(g) that can be placed in a container of the same size at STP?
a)
1.0 mole
b)
1.5 moles
c)
3.0 moles
d)
0.0 moles
48.
Which statement best describes a chemical reaction when it reaches equilibrium?
a)
The concentrations of reactants and products are the same.
b)
The concentrations of the reactants decrease to zero.
c)
The forward and reverse reaction rates are the same.
d)
The forward reaction rate decreases to zero.
49.
In a potential energy diagram, the difference between the potential energy of the products and the potential energy of the reactants is equal to the
a)
heat of reaction
b)
entropy of the reaction
c)
activation energy of the forward reaction
d)
activation energy of the reverse reaction
50.
As the concentration of reacting particles increases, the rate of reaction generally
a)
decreases
b)
increases
c)
remains the same
51.
As the temperature of a gas increases at constant pressure, the volume of the gas
a)
decreases
b)
increases
c)
remains the same
52.
Based on Reference Table H, which sample has the highest vapor pressure?
a)
water at 20oC
b)
water at 80oC
c)
ethanol at 50oC
d)
ethanol at 65oC
53.
Which sample has the greatest entropy?
a)
NH3(g)
b)
NH3(l)
c)
NH3(s)
d)
NH3(aq)
Reset
