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.

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml