We know that the larger the denominator (reactants), the smaller K is. How large could that number be, roughly? And does a large number for K mean that equilibrium lies more with the products? And are the concentrations or activities mentioned in the exercises, or do you have to determine them yourself?
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K can be almost as large as desired, but can also approach 0 as desired.
This is particularly good when you look at the following reaction:
2 H2 + O2 —> 2 H2O
At 25 degrees Celsius, K has the value 1.3 x 10^80. This indicates that the equilibrium of the reaction at the temperature is very far on the product side, which we see ourselves. Water and no gas come from the tap.
At 6000 degrees Celsius, K has the value 0.3. In this case, the equilibrium is rather on the starting material side.
This shows that the equilibrium constant K is to be defined, inter alia, as a function of temperature, and that a K does not exist for a reaction.
K is defined by the Mass Effect Act. If K assumes the value 1, then counters and denominators must be the same size, i.e. the equilibrium is exactly in the middle (of educt and product is equal).
In the case of all less than 1, the denominator (=the starting materials) must be greater than the counter (=products), in this case the equilibrium is on the starting material side (there is more starting material than the product).
The counter must be larger than the denominator, so the equilibrium is on the product side (it is available to me as the starting material).
K will never be negative, but can reach as close as possible to the 0, or end up in exorbitantly large 10s pools. There’s no limit set up.
This is because in theory any chemical reaction is reversible, and thus an equilibrium constant K could be defined for each chemical reaction, which can be excessively large but also incredibly small.
Tasks can be either that K is given to you and you are to calculate equilibrium concentrations from reactant concentrations that are given, or that K and product concentrations are given to you and you are to calculate the reactant concentrations, or that everything is given to you and you are to calculate only K, there are many possible tasks and tasks.
Did it really explain very well. The temperature-dependent equilibrium constant: I should consider the ideal gas law where the temperature is in the formula or? So, of course, even if the task is to give this information out, right?
No, the temperature is not included here or “calculated”. This was an example of how large K can be, and that K (in the case) is dependent on the temperature in that the equilibrium concentrations change, and thus, logically, also K changes when an external force (principle of Le Chatelier) is applied to a system, since then the reaction in one direction can be favored or made more difficult.
K is therefore variable due to a temperature dependence of the reaction and not always a fixed value for a reaction. That’s what I wanted to say and show.
Thanks for additional information
K can accordingly also be calculated via the Gibbs energy and not exclusively via the Mass Effect Act:
K = e^-ΔG/RT
Right if you work with partial pressures, you can work with the addition of the ideal gas constant R and the temperature in Kelvin.
That’s what you do in gas phase reactions, but I’ve never used it so far.
https://de.wikipedia.org/wiki/mass effect law#Setting_des_mass effect law_f%C3%BCr_homogene_gas balances
According to the wiki, it is included for homogeneous gas equilibriums when one works with partial pressure instead of the activities…