For each event stated below, indicate how the concentration of each species in t
ID: 1026667 • Letter: F
Question
For each event stated below, indicate how the concentration of each species in the chemical equation will then change to reach equilibrium.Click in each blue box below to toggle the relative change in concentration (up=increases, down=decreases, leave the box blank for no change).
2Co(g) + O2(g)-> 2CO2(g)
a) increasing the concentration of CO b) increasing the concentration of CO2 c) decreasing the the volume of the system uestion 5 of 5 Sapling Learning Map For each event stated below, indicate how the concentration of each species in the chemical equation will then change to reach equilibrium. Click in each blue box below to toggle the relative change in concentration (up-increases leave the box blank for no change) down-decreases, a) increasing the concentration of CO b) increasing the concentration of CO2 c) decreasing the the volume of the system y Hint PreviousCheck Answer NextExit
Explanation / Answer
The given system is an equilibrium and when a change in the equilibrium's condition is applied, the system being a dynamic one responds to this applied change by altering the rates of the forward or backward reaction establishing a new state of dynamic equilibrium for that new condition. This is Le Chatlier's principle.
a) Increasing the concentration of CO means an increase in reactant concentration. The system responds to this stress by increasing the forward reaction rate so that more of CO is consumed thus resulting in the formation of more quantities of carbon dioxide.
b) Increasing the concentration of carbon dioxide tips the equilibrium to the left as greater quantities of the product is added externally. To compensate this, the system increases reverse reaction rate thus decomposing the carbon dioxide to give more carbon monoxide and oxygen.
c) When the volume of the system is decreased, the pressure exerted by the gases increase. To compensate this, the equilibrium goes more towards the reaction which produces less moles of gases. In this case, the forward reaction involves three equivalents of gases combining to give 2 equivalents while the reverse reaction involves two equivalents decomposing to give three equivalents. Thus upon decreasing the volume, the forward reaction will be favoured.
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