<u>Answer:</u> The moles of added to the system is 7.13 moles
<u>Explanation:</u>
We are given:
Moles of at equilibrium = 1.00 moles
Moles of at equilibrium = 1.00 moles
Moles of at equilibrium = 2.40 moles
Moles of at equilibrium = 2.40 moles
Volume of the container = 4.00 L
Concentration is written as:
The given chemical equation follows:
The expression of for above equation follows:
Putting values in above equation, we get:
To calculate the number of moles for given molarity, we use the equation:
Molarity of CO = 0.791 mol/L
Volume of solution = 4.00 L
Putting values in above equation, we get:
Extra moles of CO = (3.164 - 2.40) = 0.764 moles
Let the moles of needed be 'x' moles.
Now, equilibrium gets re-established:
Initial: 1.00 1.00 2.40 2.40
At eqllm: (0.236+x) 0.236 3.164 3.164
Again, putting the values in the expression of , we get:
Hence, the moles of added to the system is 7.13 moles