Videos
(a)
Interpretation:
The effect of addition of catalyst on amount of carbon monoxide in given reaction has to be explained.
Concept introduction:
Le Chatelier's principle states that if a system in equilibrium gets disturbed due to modification of concentration, temperature, volume, and pressure, then it resets to counteract the effect of disturbance.
(b)
Interpretation:
The effect of increase in temperature of given reaction results in change in concentration of carbon monoxide has to be explained.
Concept introduction:
Le Chatelier's principle states that if a system in equilibrium gets disturbed due to modification of concentration, temperature, volume, and pressure, then it resets to counteract the effect of disturbance.
Effect of change in temperature:
Endothermic reaction: In this reaction increase in temperature which is absorbed in reactant side, the reaction occurs in a way to relieve the stress in reactant side. The reaction occurs along the direction of product side and increases equilibrium constant.
Exothermic reaction: In this reaction increase in temperature which is released in product side, the reaction occurs in a way to relieve the stress in product side. The reaction occurs along the direction of reactant side and decreases equilibrium constant.
(c)
Interpretation:
The effect of increase in pressure of the given reaction results in change in concentration of carbon monoxide has to be explained.
Concept introduction:
Le Chatelier's principle states that if a system in equilibrium gets disturbed due to modification of concentration, temperature, volume, and pressure, then it resetss to counteract the effect of disturbance.
Effect of change in pressure:
- According to Le Chatelier's principle, increase in pressure leads to flow of reaction in direction where number of moles is less.
- According to Le Chatelier's principle, decrease in pressure leads to flow of reaction in direction where number of moles is more.
(d)
Interpretation:
The effect of increase in pressure by adding argon of the given reaction has to be explained.
Concept introduction:
Le Chatelier's principle states that if a system in equilibrium gets disturbed due to modification of concentration, temperature, volume, and pressure, then it resets to counteract the effect of disturbance.
Effect of change in pressure:
- According to Le Chatelier's principle, increase in pressure leads to flow of reaction in direction where number of moles is less.
- According to Le Chatelier's principle, decrease in pressure leads to flow of reaction in direction where number of moles is more.
(e)
Interpretation:
The effect of increase in pressure by adding oxygen gas of the given reaction results in change in concentration of carbon monoxide has to be explained.
Concept introduction:
Le Chatelier's principle states that if a system in equilibrium gets disturbed due to modification of concentration, temperature, volume, and pressure, then it resets to counteract the effect of disturbance.
Effect of change in pressure:
- According to Le Chatelier's principle, increase in pressure leads to flow of reaction in direction where number of moles is less.
- According to Le Chatelier's principle, decrease in pressure leads to flow of reaction in direction where number of moles is more.
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Chapter 13 Solutions
General Chemistry: Atoms First
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- Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?arrow_forwardMethanol, a common laboratory solvent, poses a threat of blindness or death if consumed in sufficient amounts. Once in the body, the substance is oxidized to produce formaldehyde (embalming fluid) and eventually formic acid. Both of these substances are also toxic in varying levels. The equilibrium between methanol and formaldehyde can be described as follows: CH3OH(aq)H2CO(aq)+H2(aq) Assuming the value of K for this reaction is 3.7 1010, what are the equilibrium concentrations of each species if you start with a 1.24 M solution of methanol? What will happen to the concentration of methanol as the formaldehyde is further converted to formic acid?arrow_forward
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