The specific heat of water is 4.18J/(g·ºC). How many joules are required to heat 100 grams of water from 25ºC to 35ºC?
4180 J
239 J
14630 J
10450 J
A 5 gram piece of a metal at 0ºC absorbs 1000 J of energy, after which the temperature of the metal is 400ºC. What is the specific heat of the metal?
0.5 J/(g·ºC)
2 J/(g·ºC)
0.25 J/(g·ºC)
2 x 106 J/(g·ºC)
The specific heat of gold is 0.13 J/(g·ºC). How many joules are required to heat 40 grams of gold from 60ºC to 85ºC?
130 J
12.3 J
4.8 J
13 J
Ice has a specific heat of 2 J/(g·ºC). How many joules must be absorbed by a 50 gram piece of ice in order to raise the temperature from -18ºC to -10ºC?
800 J
12.5 J
3.125 J
0.32 J
The molar heat of fusion for water is 6 kJ/mol. How much energy is required to melt 3 moles of ice at 0ºC?
18 kJ
2 kJ
0.50 kJ
9 kJ
The molar heat of fusion for water is 6 kJ/mol. How much energy must be removed from 10 moles of water at 0ºC in order to convert it to ice at 0ºC?
60 kJ
0.6 kJ
1.66 kJ
16 kJ
The molar heat of vaporization for water is 41 kJ/mol. How much energy must be absorbed by 20 moles of water at 100ºC in order to convert it to steam at 100ºC?
820 kJ
4100 kJ
82 000 kJ
8.2 kJ
The process of converting ice to water by occurs by:
the addition of energy
the removal energy
no change in energy
Which of the following is written incorrectly?
liquid water + energy --> ice
liquid water + energy --> water vapor
water vapor --> liquid water + energy
ice + energy --> liquid water
Equal masses of each of the following substances absorb an equal amount of energy. Which substance experiences the greatest temperature increase?
Iron; specific heat = 0.449 J/(g·ºC) Aluminum; specific heat = 0.897 J/(g·ºC) Liquid water; specific heat = 4.18 J/(g·ºC) Ice; specific heat = 2.06 J/(g·ºC)
Iron
Aluminum
Liquid water
Ice
Which of the following will always increase the rate of a chemical reaction?
An increase in temperature increases the rate of a chemical reaction by what means
Catalysts increase the rate of a chemical reaction by what means?
Which of the following will burn most rapidly?
Solid alcohol
Liquid alcohol
Vaporized alcohol
All burn at the same rate
In chemical reactions, electricity, a spark, and sunlight are all ways in which _______________ may be provided.
activation energy
reactants
products
catalysts
For an effective collision to take place, there must be:
Which of the following is guaranteed to slow down the rate of a chemical reaction?
At 25 ºC, a certain reaction is able to produce 0.80 moles of product per minute? At what rate might the product be produced at 35 ºC?
0.40 moles per minute
1.6 moles per minute
0.20 moles per minute
0.80 moles per minute
At 25 ºC, a certain reaction is able to produce 0.80 moles of product per minute? At what rate might the product be produced at 15 ºC?
0.40 moles per minute
1.6 moles per minute
1.20 moles per minute
0.80 moles per minute
In this chemical reaction:
2 HCl(aq) + Mg(s) <--> MgCl2(aq) + H2(g) + heat
energy is given off, so the reaction is endothermic
energy is given off, so the reaction is exothermic
energy is absorbed, so the reaction is endothermic
energy is absorbed, so the reaction is exothermic
Given the following reaction:
P4(s) + 5 O2(g) --> 2 P2O5(s)
If the intial rate of the reaction consumes 1 mole of phosphorus, P4, per second, what is the rate at which oxygen, O2, is consumed initially?
1 mole per second
2 moles per second
0.2 moles per second
5 moles per second
Given the following reaction:
P4(s) + 5 O2(g) --> 2 P2O5(s)
If the intial rate of the reaction consumes 1 mole of phosphorus, P4, per second, what is the rate at which diphosphorus pentoxide, P2O5, is formed initially?
1 mole per second
2 moles per second
0.2 moles per second
5 moles per second
Given the following reaction:
C3H8(g) + 5 O2(g) --> 3 CO2 + 4 H2O(g)
If the intial rate of the reaction produces 2 moles of water vapor, H2O, per second, what is the rate at which carbon dioxide, CO2, is formed initially?
3 moles per second
2 moles per second
2.67 moles per second
1.5 moles per second
Given the following reaction:
C3H8(g) + 5 O2(g) --> 3 CO2 + 4 H2O(g)
If the intial rate of the reaction produces 2 moles of water vapor, H2O, per second, what is the rate at which oxygen, O2, is consumed initially?
1 mole per second
2 moles per second
8 moles per second
2.5 moles per second
Given the following reaction:
C3H8(g) + 5 O2(g) --> 3 CO2 + 4 H2O(g)
If the intial rate of the reaction produces 2 moles of water vapor, H2O, per second, what is the rate at which propane, C3H8, is consumed initially?
1 mole per second
2 moles per second
4 moles per second
0.5 moles per second
Given the following reaction:
2 H2(g) + O2(g) --> 2 H2O
As this reaction takes place:
the quantity of water vapor, H2O(g), decreases
the quantities of hydrogen, H2, and oxygen, O2, decrease
the quantities of hydrogen, H2, and oxygen, O2, increase
the quantity of hydrogen, H2, increases and the quantity of oxygen, O2, decreases
Given the following reaction:
H2(g) + Cl2(g) --> 2 HCl
As this reaction takes place:
For the forward reaction depicted in this diagram, DH = ?
10 kJ/mol
-20 kJ/mol
65 kJ/mol
30 kJ/mol
-30 kJ/mol
For the forward reaction depicted in this diagram, the Activation Energy, Ea = ?
10 kJ/mol
55 kJ/mol
-30 kJ/mol
-20 kJ/mol
65 kJ/mol
For the reverse reaction depicted in this diagram, DH = ?
10 kJ/mol
-20 kJ/mol
65 kJ/mol
30 kJ/mol
-30 kJ/mol
For the reverse reaction depicted in this diagram, the Activation Energy,Ea = ?
-20 kJ/mol
65 kJ/mol
85 kJ/mol
10 kJ/mol
-55 kJ/mol
The forward reaction depicted in this diagram is:
Endothermic
Exothermic
Isothermic
When extra NH3 is added to the following system at equilibrium:
3 H2(g) + N2(g) <--> 2 NH3(g)
In order to restore equilibrium, the reaction shifts right, toward products
In order to restore equilibrium, the reaction shifts left, toward reactants
No change occurs
When N2 is removed from the following system at equilibrium:
3 H2(g) + N2(g) <--> 2 NH3(g)
In order to restore equilibrium, the reaction shifts right, toward products
In order to restore equilibrium, the reaction shifts left, toward reactants
No change occurs
When H2 is added to the following system at equilibrium:
3 H2(g) + N2(g) <--> 2 NH3(g)
In order to restore equilibrium, the reaction shifts right, toward products
In order to restore equilibrium, the reaction shifts left, toward reactants
No change occurs
When the pressure is increased on the following system at equilibrium:
3 H2(g) + N2(g) <--> 2 NH3(g)
In order to restore equilibrium, the reaction shifts right, toward products
In order to restore equilibrium, the reaction shifts left, toward reactants
No change occurs
When the pressure is decreased on the following system at equilibrium:
3 H2(g) + N2(g) <--> 2 NH3(g)
In order to restore equilibrium, the reaction shifts right, toward products
In order to restore equilibrium, the reaction shifts left, toward reactants
No change occurs
When the temperature is decreased on the following system at equilibrium:
2 HCl(aq) + Mg(s) <--> MgCl2(aq) + H2(g) + heat
In order to restore equilibrium, the reaction shifts right, toward products
In order to restore equilibrium, the reaction shifts left, toward reactants
No change occurs
When the temperature is increased on the following system at equilibrium:
2 HCl(aq) + Mg(s) <--> MgCl2(aq) + H2(g) + heat
In order to restore equilibrium, the reaction shifts right, toward products
In order to restore equilibrium, the reaction shifts left, toward reactants
No change occurs
When the temperature is decreased on the following system at equilibrium:
2 HCl(aq) + Mg(s) <--> MgCl2(aq) + H2(g) + heat
In order to restore equilibrium, the reaction shifts right, toward products
In order to restore equilibrium, the reaction shifts left, toward reactants