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When the heat shifts the direction of the reaction there has been a change in concentration and equilibrium will then be affected?
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∙ 10y ago
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Wiki User
∙ 10y ago
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What equilibrium concentrations are affected by changing the initial concentration?
Yes, the concentrations are constant but not necessarily static. The 'forward' reaction rate matches the 'reverse' reaction rate.
Looking at a free energy diagram for an equilibrium reaction what scenarios will favor the formation of more product?
The concentration of reactants is greater than the concentration of reactants at equilibrium. The concentration of products is less than the concentration of products at equilibrium
When a reaction is at equilibrium increasing the temperature favors the reaction that what?
First read this to understand equilibrium: if the point of equilibrium moves to the left there will be more reactants than products. If the point of equilibrium moves to the right there will be more products than reactants. Le Chatelier's principle states that whatever you do to the reaction, the reaction will try and reverse the effects. Eg: heat it, and it will try and cool it down. ANSWER: If you increase the concentration of the reactants (left side), according to Le Chatelier's principle the reaction will try and get rid of the extra reactants, so it will decrease the concentration of reactants. This means the position of equilibrium will move to the right, so more products will be formed.
What is the effect of reactant concentration?
Generally, the higher the concentrations the faster the reaction. It does not push the reaction further past the equilibrium.
What happens when there is a very high k value in an equilibrium reaction?
Forward reaction favored, concentration of products is higher
How would the equilibrium concentration of H2O be affected by adding a catalyst to the mixture?
None. A catalyst affects only the rate of reaction, and if the reaction is already at equilibrium, the net rate of the reaction is zero and remains so after a catalyst is added.
What equilibrium concentrations are affected by changing the initial concentration?
Yes, the concentrations are constant but not necessarily static. The 'forward' reaction rate matches the 'reverse' reaction rate.
What of the following characterizes reaction at equilibrium?
The reactants concentration is equal to products concentration.
Why does changing the concentration of reactant shift the equilibrium?
Le Chatlier's PrincipleIf an equilibrium reaction is occurring and some reactant from either side of the equilibrium is added, the reaction goes in a direction that is to oppose the addition of a reactant. For example. In the equilibrium of CO2 + H2O = H2CO3, if more CO2 is added then the equilibrium shifts in such a way that this change is opposed so more H2CO3 is produced. For more information, research Le Chatlier's Principle.
Looking at a free energy diagram for an equilibrium reaction what scenarios will favor the formation of more product?
The concentration of reactants is greater than the concentration of reactants at equilibrium. The concentration of products is less than the concentration of products at equilibrium
Looking at a free energy diagram for an equilibrium reaction which of the following scenarios will favor the formation of more reactant?
The concentration of reactants is less than the concentration of reactants at equilibrium. The concentration of products is greater than the concentration of products at equilibrium.
The equilibrium constant for the reaction below is 0.625 At equilibrium O2 0.40 and H2O 0.20 What is the equilibrium concentration of H2O2?
0.16
The equilibrium constant for the reaction below is 0.49 At equilibrium O2 equals 0.11 and N2 equals 0.15 What is the equilibrium concentration of NO?
0.09
What happens when the equilibrium constant is zero for a reaction?
If the equilibrium constant is zero, the reaction canNOT (will NEVER) reach equilibrium, it can not react back because all products are 'removed' (= concentration is zero).
In a reversible reaction two substances are in equilibrium if the concentration of each is doubled but the equilibrium constant remains unaffected?
TRUE
The equilibrium constant for the reaction below is 31.25 at equilibrium so2 0.03 o2 0.05 and h2s 0.15 what is the equilibrium concentration of H2O?
0.0001
When a reaction is at equilibrium increasing the temperature favors the reaction that what?
First read this to understand equilibrium: if the point of equilibrium moves to the left there will be more reactants than products. If the point of equilibrium moves to the right there will be more products than reactants. Le Chatelier's principle states that whatever you do to the reaction, the reaction will try and reverse the effects. Eg: heat it, and it will try and cool it down. ANSWER: If you increase the concentration of the reactants (left side), according to Le Chatelier's principle the reaction will try and get rid of the extra reactants, so it will decrease the concentration of reactants. This means the position of equilibrium will move to the right, so more products will be formed.
