Chemical Equilibrium: Calculating Number of Moles at Equilibrium
How can we calculate the number of moles of HI that are at equilibrium?
Given that there are 1.25 mol of H2 and 1.25 mol of I2 in a 5.00-L flask at 448 °C with a Kc value of 50.2, how do we determine the number of moles of HI at equilibrium?
Calculating the Number of Moles of HI at Equilibrium
For this chemical equilibrium problem, first, we need to write the balanced equation for the given reaction, which is H2 + I2 ⇌ 2HI. Then, we would create an ICE table to track the initial concentration, change in concentration, and equilibrium concentration of each component. The equation and ICE table would look like this:
I C E
1.25 mol 0 mol 0.625 mol
1.25 mol 0 mol 0.625 mol
0 mol +2x 2x
Next, we would use the equilibrium constant expression, Kc = [HI]2 / [H2][I2], and substitute the equilibrium concentrations into the equation to solve for x. After solving for x, we can determine that the equilibrium concentration of HI is 1.000 mol in a 5.00-L flask.
Understanding Chemical Equilibrium Calculation
In this chemical equilibrium scenario, the key is to utilize the equilibrium constant, Kc, as a guide to determine the concentration of each component at equilibrium. The ICE table serves as a systematic approach to track the changes in concentration as the reaction reaches equilibrium.
By diligently following the steps outlined in the solution, we can accurately calculate the number of moles of HI that are at equilibrium with the initial concentrations of H2 and I2 provided in the problem. This calculation showcases the dynamic nature of chemical reactions and how equilibrium is achieved.
Furthermore, understanding the concept of equilibrium and how to calculate it is crucial in the field of chemistry, as it helps in predicting the behavior of reactions and the concentrations of reactants and products in a system. Mastery of equilibrium calculations is essential for students and professionals alike to navigate the complexities of chemical processes.
So, by applying the principles of chemical equilibrium and following the step-by-step calculation method, we can determine the precise number of moles of HI at equilibrium in the given scenario, enhancing our comprehension of chemical dynamics.