In reaction: 2H₂O(g)⇌2H₂(g)+O₂(g); ∆H=+242 kJ/mol In which direction the equilibrium shifts, if: a. Temperature is increased? b. Temperature is descreased? c. H₂ is added? d. O₂ is reduced? e. Pressure is enlarged?
The reaction is endothermic so the forward reaction is endothermic. If the temperature is increased, the equilibrium would shift to the right so more reactant is made and vice versa.
If more hydrogen is added, more water, more reactant is produced so equilibrium shifts to the left. If Oxygen is reduced, more water will decompose to produce more products so equilibrium shifts to the right.
If pressure is increased, the equilibrium will shift to the side with fewer moles of gas; 2:3 so more water will be formed than products. The equilibrium will shift to the left.
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Left: a,c,e
Right: b,d
Le Chatelier's principle states that equilirbium shifts to the direction which will counteract the effect of change.
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a. shift to left
b. shift to right
c. shift to left
d. shift to right
e. shift to left
Reaction shifts are pretty easy to identify if you think of the balanced equation as a literal "balance". Changing something on one side requires something to change on the other side to maintain the balance (equilibrium).
The same is true for thermodynamic (heat) effects. If the reaction requires heat input, adding more will make it proceed faster, and decreasing it will make it go slower.
Pressure affects the reaction rate , but not the equilibrium position. However, le Chatelier's Principle applied to gases will tend to reduce the total molar volume. Thus, higher pressure will shift the reaction to the left (2 molecules) from the right (three molecules).
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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