Search found 5 matches

by JNie1L
Sun Jan 12, 2020 11:29 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: 5G.9
Replies: 3
Views: 60

Re: 5G.9

Only D and E will be the same. D and E are the expressions for K in both the forward and reverse reactions. K is always constant at a certain temperature, so those values will stay constant. A, B, and C are all dependent on the amount of moles or specific partial pressures and will differ between th...
by JNie1L
Sun Jan 12, 2020 11:21 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Types of Equilibrium Constants
Replies: 7
Views: 52

Re: Types of Equilibrium Constants

When working with aqueous solutions use Kc because it is referring to molarity or concentration. When working with gases use Kp because each gas has its own partial pressure.
by JNie1L
Sun Jan 12, 2020 11:15 pm
Forum: Ideal Gases
Topic: Ideal gas law exceptions
Replies: 3
Views: 33

Re: Ideal gas law exceptions

Yes, the ideal gas law is best represented with noble gases. Non-noble gases can be approximated using the ideal gas law, and here is also a version with corrections:
RT = (P + a(n/V)^2) (V/n - b)
by JNie1L
Sun Jan 12, 2020 11:10 pm
Forum: Ideal Gases
Topic: ICE Table
Replies: 9
Views: 99

Re: ICE Table

An ICE table is used to calculate the concentrations of substances when not given all the equilibrium concentrations. We use the Kc and set it equal to the ratio of concentrations. The ICE table tracks the initial, change, and final concentrations of the equilibrium concentrations.
by JNie1L
Sun Jan 12, 2020 11:01 pm
Forum: Ideal Gases
Topic: K and Units
Replies: 7
Views: 42

Re: K and Units

Since K is a ratio and regarded as a constant, it doesn't use units. However, molarity or concentration has units of moles/L.

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