Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after reactant or product is added. an up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. 2co(g) + o2(g) ↽â’â’⇀ 2co2(g) increasing the concentration of co increasing the concentration of co2

Based on Le Chatelier's principle, if the equilibrium of a given system is disturbed by inducing a change in the temperature, pressure or concentration, then the equilibrium will shift in a direction to undo the effect of the change induced.

The given equilibrium is:

2CO(g) + O2(g) ↔ 2CO2(g)

a) If the concentration of CO (reactant) is increased, then the equilibrium will shift to a direction which would lower the concentration of CO i.e. in the forward direction. Therefore,

[CO2] will increase

[CO] and [O2] will decrease

b) If the concentration of CO2 (product) is increased, then the equilibrium will shift to a direction which would lower the concentration of CO2 i.e. in the reverse direction. Therefore,

[CO2] will decrease

[CO] and [O2] will increase.

so what is the problem with your lab report and whats the subject of the lab report? i will you

the awnser is group 12