NEW
Font size
WorksheetsUnit 11 test review
Total questions: 55
Worksheet time: 1hrs 20mins
the difference between the energy of an activated complex and the energy of the reactants of a chemical reaction; the energy with which particles must collide in order to react
Activation energy
Activation complex
entropy
enthalpy
a collection of intermediate structures in a chemical reaction that persist while bonds break and new bonds form; a range of configurations that atoms pass through in between clearly defined products and reactant
Activation complex
activation energy
catalysis
enthalpy
the alteration of the rate of a chemical reaction because of the presence of a catalyst
catalysis
catalyst
equilibrium
potential energy
a substance that increases the rate of a chemical reaction by lowering the activation energy without being chemically changed by the reaction
catalyst
catalysis
endothermic reaction
le chatelier's principle
a chemical process that absorbs heat
endothermic reaction
exothermic reaction
forward reaction
equilibrium
the heat content of a system at constant pressure
enthalpy
entropy
reaction rates
catalyst
a quantitative measure of the disorder or randomness of a system
entropy
enthalpy
potential energy
spontaneous reaction
the concentrations of the reactants and products are constant and their ratio does not vary; forward and reverse reactions occur at the same rate
equilibrium
entropy
reaction rates
forward reaction
a chemical process that releases heat
exothermic reaction
forward reaction
potential energy
catalysis
a chemical reaction that proceeds from left to right
forward reaction
reversible reaction
spontaneous reaction
activated complex
a principle that states that a reversible reaction at equilibrium will shift is a direction that will offset a stress such as pressure or concentration changes, imposed on a system
Le chatelier's principle
potential energy
endothermic reaction
catalysis
the energy possessed by a body by virtue of its position relative to others, stresses within itself, electric charge, and other factors.
potential energy
potential energy diagram
reaction rates
enthalpy
a diagram that shows the potential energy changes of the substances in a reaction over a period of time
potential energy diagram
potential energy
reaction rates
le chatelier's principle
changes in the concentration of reactants and products per unit of time as the reaction proceeds
reaction rates
activated complex
activation energy
potential energy
a reaction in which the conversion of reactants to products and the conversion of products to reactants occurs simultaneously
reversible reaction
forward reaction
spontaneous reaction
exothermic reaction
a process that proceeds on its own without any outside intervention
spontaneous reaction
reversible reaction
endothermic reaction
catalysis
A student mixed two chemicals to allow them to react. The temperature before the reaction was 25 ° C. The temperature after the reaction was 18° C. Which of the following is true?
The temperature did not change.
It is an endothermic reaction
It is an exothermic reaction
Energy is released from the reaction into the surrounding.
Photosynthesis takes place inside of leaf cells. Sunlight is required. Is this an Exothermic or an Endothermic reaction?
Endothermic
Exothermic
The graph above is from which type of reaction?
Endothermic reaction
Exothermic Reaction
The graph above is from which type of reaction?
Endothermic reaction
Exothermic reaction
The minimum energy particles must have to react is the
acting energy
active energy
activation energy
A reaction profile shows....
the relative difference in temperature of reactants and products
the relative difference in amounts of reactants and products
the relative difference in energy of reactants and products
the relative difference in volume of reactants and products
Bond making is
Endothermic
Exothermic
Bond breaking is..
Endothermic
Exothermic
Which letter shows the activation energy
A
B
C
In a reaction the energy required to break bonds is less than the energy released when bonds are made. What type of reaction is this?
Exothermic
Endothermic
Is this showing an endothermic or an exothermic reaction?
Endothermic
Exothermic
Which letter shows the heat change?
A
B
C
D
E
Which letter represents the reactants?
A
B
C
D
E
Which letter represents the products?
A
B
C
D
E
Which letter represents the transition state?
A
B
C
D
E
What type of reaction occurs in a hand warmer?
exothermic
endothermic
Which of the following process is exothermic?
Candle was melting
A puddle evaporating
Dry ice (solid carbon dioxide) subliming to form gaseous carbon dioxide
Water freezing to form ice
What is the Heat of Reaction ΔH for this reaction?
-200 KJ
200 KJ
400 KJ
-300 KJ
SO2(g) + O2(g) <−> SO3(g)
If the concentration of SO2(g) is increased, the equilibrium of the reaction will ___________.
SO2(g) + O2(g) <−> SO3(g)
If the equilibrium shifts to the right, the concentration of O2(g) will ___________.
energy + N2(g) + O2(g) <−> 2NO(g)
If O2(g) is removed, the concentration of N2 will _______.
Rewrite the above equation with energy as a reactant or product:
heat + N2(g) + O2(g) <−> 2NO(g)
If the heat is removed to the chemical system, the equilibrium will _______.
N2 (g) + 3 H2 (g) <−> 2 NH3 (g)
If the pressure in the system is increased, the reaction will __________________.
ΔHrxn= -453 kJ/mol
If the [B] is decreased then the reaction is will shift to the _______.
2SO3(g) ⇋ 2SO2(g) + O2(g)
