Chemical Equilibrium Constant K - Ice Tables - Kp and Kc
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- Опубліковано 20 сер 2024
- This chemistry video tutorial provides a basic introduction into how to solve chemical equilibrium problems. It explains how to calculate the equilibrium constant k value given the equilibrium concentrations and equilibrium partial pressures of all reactants and products. If explains how to calculate the equilibrium constant k for a new reaction by changing another reaction. Finally, it discusses how to calculate the equilibrium constant k using ice tables.
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Remember the units of Kc! If you ,for example, have the reaction
3H2 + N2 2NH3
And you are solving for Kc, place the concentrations in the formula.
(NH3 mol/l)^2 / (H2 mol/l)^3•(N2 mol/l)
Also you will have to deal with the mol/l part.
The exponents of the denominator will have to be deducted from the numerator.
So with only the units it will be
(mol/l)^2 / (mol/l)^3•(mol/l)^1
=(mol/l)^2 / (mol/l)^4
=(mol/l)^(2-4)
=(mol/l)^-2
I know this isn't the most important aspect of these calculations, but remember that Kc can and usually does have a unit after it. This unit can vary from calculation to calculation or in some cases there is no unit.
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I'm afraid kc is a unitless unit it has no dimension
@@dilshankavinda9911 The unit of Kc is (mol/L)^(order of the reaction)
@@killerfc a=yc a has no dimension which means kc has no dimension
@@dilshankavinda9911 I am sorry but I do not understand what you wrote. I think that Kc is just Molarity raised to different powers and as molarity has unit Kc also has it.
@@killerfc a=relative activity
y=activity constant
c=concentration
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