When a chemical reaction is at equilibrium the concentrations of reactants and products do not change over time. This is because the rate in the forward direction becomes equal to the rate in t reverse reaction. Note that the rates are not zero. So, if more reactant is added the forward rates increases and more product is made. If more product is added the reverse rate increases and more reactant is made. Adding or removing a reactant or product is called a stress. The chemical reaction responds to the stress in such a way to minimize the stress as the reaction goes to a ne point of equilibrium. This is called Le Chatelier's Principle. We'll use the following exothermic reaction where all are in the gaseous phase: 2 NO + 0₂ 2 NO₂ + 114 kJ/mol For example, when NO is added, the [NO₂] will increase result ^ 2 NO + 0₂ O 2 NO₂ + 114 kJ/mol ^ stress ^ [NO₂]² This can also be seen in the constant Keq which must remain a constant, Keq = To reduce the effect of added NO, [NO₂] will increase, and [O₂] will decrease Answer the following questions about the reaction at equilibrium 2 NO + 0₂ 2 NO₂ + 114 kJ/mol What happens to the [NO₂] when NO is added? What happens to the [NO₂] when NO is removed? What happens to the [NO₂] when O₂ is added? What happens to the [NO₂] when O₂ is removed? A. increases B. decreases ^ [NO]² [0₂] C. no change D. reactants E. products
When a chemical reaction is at equilibrium the concentrations of reactants and products do not change over time. This is because the rate in the forward direction becomes equal to the rate in t reverse reaction. Note that the rates are not zero. So, if more reactant is added the forward rates increases and more product is made. If more product is added the reverse rate increases and more reactant is made. Adding or removing a reactant or product is called a stress. The chemical reaction responds to the stress in such a way to minimize the stress as the reaction goes to a ne point of equilibrium. This is called Le Chatelier's Principle. We'll use the following exothermic reaction where all are in the gaseous phase: 2 NO + 0₂ 2 NO₂ + 114 kJ/mol For example, when NO is added, the [NO₂] will increase result ^ 2 NO + 0₂ O 2 NO₂ + 114 kJ/mol ^ stress ^ [NO₂]² This can also be seen in the constant Keq which must remain a constant, Keq = To reduce the effect of added NO, [NO₂] will increase, and [O₂] will decrease Answer the following questions about the reaction at equilibrium 2 NO + 0₂ 2 NO₂ + 114 kJ/mol What happens to the [NO₂] when NO is added? What happens to the [NO₂] when NO is removed? What happens to the [NO₂] when O₂ is added? What happens to the [NO₂] when O₂ is removed? A. increases B. decreases ^ [NO]² [0₂] C. no change D. reactants E. products
Introductory Chemistry: An Active Learning Approach
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Chapter18: Chemical Equilibrium
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Problem 80E: Classify each of the following statements as true or false. aSome equilibria depend on a steady...
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![When a chemical reaction is at equilibrium the concentrations of reactants and products do not change over time. This is because the rate in the forward direction becomes equal to the rate in the
reverse reaction. Note that the rates are not zero. So, if more reactant is added the forward rates increases and more product is made. If more product is added the reverse rate increases and
more reactant is made. Adding or removing a reactant or product is called a stress. The chemical reaction responds to the stress in such a way to minimize the stress as the reaction goes to a new
point of equilibrium. This is called Le Chatelier's Principle.
We'll use the following exothermic reaction where all are in the gaseous phase:
2 NO + 0₂
⇒ 2 NO₂ + 114 kJ/mol
For example, when NO is added, the [NO₂] will increase
result
2 NO + 0₂
->
^
^
2 NO₂ + 114 kJ/mol
^ [NO₂]²
stress
This can also be seen in the constant Keq which must remain a constant, Keq =
^ [NO]² [0₂]
To reduce the effect of added NO, [NO₂] will increase, and [0₂] will decrease
Answer the following questions about the reaction at equilibrium
2 NO + 0₂
2 NO₂+ 114 kJ/mol
What happens to the [NO₂] when NO is added?
What happens to the [NO₂] when NO is removed?
What happens to the [NO₂] when O₂ is added?
What happens to the [NO₂] when O₂ is removed?
A. increases
B. decreases
C. no change
D. reactants
E. products](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Feab2d2d3-91b0-42ef-9603-f34b4b53ecf8%2F0f84f249-3737-4ff0-81f4-238a35ad970e%2Fw26rcgr_processed.png&w=3840&q=75)
Transcribed Image Text:When a chemical reaction is at equilibrium the concentrations of reactants and products do not change over time. This is because the rate in the forward direction becomes equal to the rate in the
reverse reaction. Note that the rates are not zero. So, if more reactant is added the forward rates increases and more product is made. If more product is added the reverse rate increases and
more reactant is made. Adding or removing a reactant or product is called a stress. The chemical reaction responds to the stress in such a way to minimize the stress as the reaction goes to a new
point of equilibrium. This is called Le Chatelier's Principle.
We'll use the following exothermic reaction where all are in the gaseous phase:
2 NO + 0₂
⇒ 2 NO₂ + 114 kJ/mol
For example, when NO is added, the [NO₂] will increase
result
2 NO + 0₂
->
^
^
2 NO₂ + 114 kJ/mol
^ [NO₂]²
stress
This can also be seen in the constant Keq which must remain a constant, Keq =
^ [NO]² [0₂]
To reduce the effect of added NO, [NO₂] will increase, and [0₂] will decrease
Answer the following questions about the reaction at equilibrium
2 NO + 0₂
2 NO₂+ 114 kJ/mol
What happens to the [NO₂] when NO is added?
What happens to the [NO₂] when NO is removed?
What happens to the [NO₂] when O₂ is added?
What happens to the [NO₂] when O₂ is removed?
A. increases
B. decreases
C. no change
D. reactants
E. products
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