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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 stress -> A A 2 NO₂ + ^ [NO₂]² This can also be seen in the constant Keq which must remain a constant, Keq = - ^ [NO]² [0₂] 114 kJ/mol 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

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 stress -> A A 2 NO₂ + ^ [NO₂]² This can also be seen in the constant Keq which must remain a constant, Keq = - ^ [NO]² [0₂] 114 kJ/mol 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

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 1RQ: Characterize a system at chemical equilibrium with respect to each of the following a. the rates of...
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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 stress 2 NO + 0₂ ^ -> A 2 NO₂ + 114 kJ/mol ^ [NO₂]² = This can also be seen in the constant Keq which must remain a constant, Keq D. reactants ^ [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 E. products
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 stress 2 NO + 0₂ ^ -> A 2 NO₂ + 114 kJ/mol ^ [NO₂]² = This can also be seen in the constant Keq which must remain a constant, Keq D. reactants ^ [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 E. products
Heat is treated as any other reactant or product. We also saw this in stoichometry. Answer the following questions about the reaction at equilibrium 2 NO + 0₂ 2 NO₂ + 114 kJ/mol What happens to the [NO₂] when heat is added? What happens to the [NO₂] when heat is removed? The reaction would respond to an increase in pressure by trying to reduce this stress. With gases, the pressure is related to moles by PV = nRT. Thus, reducing the moles at equilibrium will reduce the pressure. Which side of the reaction has the most moles, reactants or products? What happens to the [NO₂] when the pressure is increased ? What happens to the [NO₂] when the pressure decreased ? A. increases B. decreases C. no change Mark for Review What's This? D. reactants E. products
Transcribed Image Text:Heat is treated as any other reactant or product. We also saw this in stoichometry. Answer the following questions about the reaction at equilibrium 2 NO + 0₂ 2 NO₂ + 114 kJ/mol What happens to the [NO₂] when heat is added? What happens to the [NO₂] when heat is removed? The reaction would respond to an increase in pressure by trying to reduce this stress. With gases, the pressure is related to moles by PV = nRT. Thus, reducing the moles at equilibrium will reduce the pressure. Which side of the reaction has the most moles, reactants or products? What happens to the [NO₂] when the pressure is increased ? What happens to the [NO₂] when the pressure decreased ? A. increases B. decreases C. no change Mark for Review What's This? D. reactants E. products
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