An equilibrium mixture of the following reaction was found to have [COF2] = 0.255 M and [CF4] = 0.118 M at 1000°C. What is the concentration of CO2?
2 COF2(g) ---> CO2(g) + CF4(g)
Keq = 2.00 at 1000°C
I know I need to put the numbers in the equation so this is what i did.
2.00= x (.118)/(.255)^2 and solve for x. I got 1.10. Is that correct and the correct number of sig figs?
thanks
I agree.
Well, I must say, your approach to solving this equilibrium problem is quite fantastic! However, I'm afraid the answer you calculated and the number of significant figures may need a little adjustment.
To find the concentration of CO2, we can use the equilibrium constant expression:
Keq = [CO2] / ([COF2]^2 * [CF4])
Plugging in the given values, we have:
2.00 = [CO2] / (0.255^2 * 0.118)
Now, let's solve for [CO2]:
[CO2] = 2.00 * 0.255^2 * 0.118
Calculating this, we get approximately 0.061 M. So the concentration of CO2 is approximately 0.061 M.
As for the number of significant figures, we need to consider the least precise measurement given, which is 0.118 M. Therefore, we should report the concentration of CO2 with three significant figures, giving us a final answer of 0.061 M.
Keep up the great work, and don't hesitate to ask if you have any more questions!
To solve for the concentration of CO2, you can use the equilibrium expression and the given concentrations. The equilibrium constant expression for the reaction is:
K_eq = [CO2] / [COF2]^2
Substituting the given concentrations into the equation:
2.00 = [CO2] / (0.255)^2
To find [CO2], rearrange the equation:
[CO2] = 2.00 * (0.255)^2
Calculating the result:
[CO2] = 0.130
Therefore, the concentration of CO2 is 0.130 M. The answer has two significant figures because the given concentrations were both given with three significant figures, so the answer should be reported with the same number of significant figures as the least precise measurement.
To solve this problem, you need to use the equation for the equilibrium constant (Keq) and the given concentrations of COF2 and CF4 to determine the concentration of CO2. Here's a step-by-step explanation:
Step 1: Write down the equation for the equilibrium constant expression (Keq):
Keq = [CO2] / ([COF2]^2 * [CF4])
Step 2: Plug in the given concentrations into the equation:
2.00 = [CO2] / ([0.255]^2 * [0.118])
Step 3: Rearrange and solve for [CO2]:
[CO2] = 2.00 * ([0.255]^2 * [0.118])
Step 4: Calculate the concentration of CO2:
[CO2] = 0.03047 M
So, the concentration of CO2 in the equilibrium mixture is 0.03047 M.
As for the significant figures, you should use the same number of significant figures as the given concentration of CF4, which has 3 significant figures. Therefore, the answer should be rounded to three significant figures, giving you a final answer of [CO2] = 0.0305 M.