the equlibrium equation is (I2)^2(CO2)^5/(CO)^5.
If the (CO) starts at 1.0 M and decreases to 0.25 M at equilibrium, give the value of Keq.
How would i do that??
Have you omitted something? Where does the I2 come in? And how does the CO get to CO2? The equation must be somthing like this.
5CO + ?? ==> 5CO2 + I2
I2O5=??
If you have a question to post, I suggest you go to the top of the page, click on post a new question and post it. Posting on another question piggy-back style often leads to it being overlooked. What about I2O5. Do you want the name? Its density. Its color? what? I would name it diiodidopentoxide or diiodine pentoxide.
To find the value of Keq (equilibrium constant) using the given equation, you need to determine the concentrations of the reactants and products at equilibrium.
In this case, the equilibrium equation is:
Keq = (I2)^2 (CO2)^5 / (CO)^5
Given that the initial concentration of (CO) is 1.0 M and it decreases to 0.25 M at equilibrium, you will use these values to calculate Keq.
Step 1: Write down the equation using the given concentrations at equilibrium:
Keq = (I2)^2 (CO2)^5 / (0.25)^5
Step 2: Simplify the equation:
Keq = (I2)^2 (CO2)^5 / 0.0009765625
Step 3: Convert the decimal into fraction for easier calculations:
Keq = (I2)^2 (CO2)^5 / 1/1024
Step 4: Calculate the value Keq using the given equation and any additional information you have about the concentrations of (I2) and (CO2) at equilibrium.
Note: Since the concentrations of (I2) and (CO2) at equilibrium are not provided, you will need that information or additional equations to determine their values.
Once you have the concentrations, simply substitute them into the equation and calculate Keq.