the following reaction occurred at 45 degrees
all gases h2+f2=2hf
the equlibrium conc in a 5ml container are h2=.0500m, f2=.0100m and hf =.400m. if .200ml of f2 is added calculate the concentrations and pressures of all gases once equlibrium is rfeestablished
q = [hf]^2/[h2][f2]=.4^2/(.05)(.21)=15.238
k=[hf]/[h2][f2]= .4^2/(.05)(.01)=320
then i am lost
I strongly suggest you find the caps key and use it. If you are working on equilibrium problems SURELY you've had enough chemistry to know that lower case and upper case mean something different. See CO, Co, co. You have used m; I assume that should be M since you didn't find the caps key for anything else. m = molality; M = molarity.
Your Q is ok and K is ok. Q<K which means the reaction will shift to the right upon addition of the extra F2.
So how much F2 is added? Whatever 0.200 ml means. Convert that value, whatever it is, to molarity = M.
The new equilibrium is this.
.........H2 + F2 ==> 2HF
E(old)..0.05..0.01...0.400
I....0.0500..0.0100..0.400
add........0.200ml converted to M.
C.......-x....-x.....+2x
E...0.05-x...(?-x)...0.4+2x
Plug the E line into the Keq expression and solve for x, then evaluate the other concentrations.
Post your work if you get stuck.
To calculate the concentrations and pressures of all gases once equilibrium is reestablished, you can use the concept of the equilibrium constant (K).
In this reaction, the equilibrium constant (K) is given as:
K = [HF]^2 / ([H2] * [F2])
Given that the equilibrium concentrations in a 5ml container are:
[H2] = 0.0500 M
[F2] = 0.0100 M
[HF] = 0.400 M
To find the new concentrations and pressures after adding 0.200 ml of F2, you need to consider the changes in the concentrations.
Since the total volume of the container is 5 ml and you're adding 0.200 ml, the new total volume will be 5.2 ml.
To find the new concentrations, you can use the following equation:
[new concentration] = [initial concentration] * ([total volume] - [added volume]) / [total volume]
For H2:
[H2] = 0.0500 M * (5.2 ml - 0 ml) / 5.2 ml
For F2:
[F2] = 0.0100 M * (5.2 ml - 0.200 ml) / 5.2 ml
For HF:
[HF] = 0.400 M * (5.2 ml - 0 ml) / 5.2 ml
Once you calculate the new concentrations for each gas, you can use the ideal gas law to calculate the pressures of each gas.
The ideal gas law equation is:
PV = nRT
Since you have the new concentrations and the total volume of the container, you can rearrange the equation as follows:
P = (n/V) * RT
Assuming the temperature (T) is constant, you can calculate the pressures of each gas using the new concentrations and the ideal gas law equation.
It's important to note that this explanation assumes that the reaction is taking place in an ideal gas mixture and at constant temperature.