__Category__: Chemical Engineering Math"Published in Newark, California, USA"

At 3000K and 1 atm, CO

_{2}is 40% dissociated to CO and O

_{2}. Calculate its percentage dissociation when the pressure is increased to 2 atm.

__Solution__:

Consider the chemical reaction above as follows

For gases, the equilibrium constant of the above reaction is

At the start of the reaction, the total pressure of CO

_{2}which is the total pressure of gas mixture is equal to1 atm. At equilibrium, the partial pressure of gases are as follows:

Hence, the equilibrium constant for the reaction above is

_{2}dissociated, then the partial pressure of gases are as follows:

If the pressure is increased to 2 atm, then the partial pressure of gases will be multiplied by 2. Substitute the value of partial pressure of gases at the chemical equilibrium equation above, we have

Since the above equation cannot be factored by factoring and even synthetic division, then we have to do the trial and error method until we get zero at the right side of the equation. The best way is to use Excel program in solving for the value of x because we can input the formula and we can assign any values of x in the spreadsheet as follows

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From the Excel spreadsheet, the value of x which is the partial pressure of CO

_{2}dissociated is 0.33648572 atm since the right side of the equation is very close to zero.

Therefore, the percent of dissociation of CO

_{2}is