The oxidation of carbon monoxide proceeds as follows: 2CO( g) + O2(g) 2CO2(g) Which of the following will cause an increase in the equilibrium concentration of CO? The oxidation of carbon monoxide proceeds as follows: 2CO( g) + O2(g) 2CO2(g) Which of the following will cause an increase in the equilibrium concentration of CO? adding more O 2 to the system adding a catalyst removing CO 2 from the system as it is formed add CO 2 to the system
The oxidation of carbon monoxide proceeds as follows:
2CO( g) + O2(g) 2CO2(g)
Which of the following will cause an increase
in the equilibrium concentration of CO?
The oxidation of carbon monoxide proceeds as follows:
2CO( g) + O2(g) 2CO2(g)
Which of the following will cause an increase
in the equilibrium concentration of CO?
adding more O 2 to the system
adding a catalyst
removing CO 2 from the system as it is formed
add CO 2 to the system
To solve this problem we have to use Le Chatelier's principle .
According to this principle if any changes is made in the reaction i.e concentration, volume , pressure , temperature then the equilibrium will shift in the opposite direction to balance the condition .
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