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22/09/2021
See below.
The equilibrium constant of a reaction under the general form:
##A(g)+B(g)rightleftharpoonsC(g)+D(g)##
can be calculated by the general expression of ##K_(eq)## as follows:
##K_(eq)=([“Products”])/([“Reactants”])##
Therefore, ##K_(eq)=([C][D])/([A][B])=K_c##
If the reactants and products are gases, we can also calculate the equilibrium constant using pressures, in this case the equilibrium constant is called ##K_P##:
##K_P=(P_CxxP_D)/(P_AxxP_B)##
Note that, if any of the reactants or products are in the liquid or solid states, these are not included in the expression of the equilibrium constant.
For example, consider the following general reaction:
##A(g)+B(l)rightleftharpoonsC(g)+D(s)##
Thus, the equilibrium constant ##K_c## expression is written as:
##K_c=([C])/([A])##
or using pressures as:
##K_P=(P_C)/(P_A)##
Note that aqueous state is treated as gases, however, we don’t calculate ##K_P## in this case from pressures, therefore, we only find ##K_c##:
##A(aq)+B(aq)rightleftharpoonsC(aq)+D(aq)##
##K_c=([C][D])/([A][B])##
This lesson could be even discussed with more details. I recommend that you watch the following video which is one of an entire chapter of five videos on chemical equilibrium:Chemical Equilibrium | The Equilibrium Conditions.
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I want to thank your team (Jeff) for finding a new writer when you were unable to reach my existing writer to revise my paper. I appreciate your professionalism and efforts. Thanks
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