Given #K_c = 0.36# at #2000^@ "C"# for #"N"_2"O"_4(g) rightleftharpoons "NO"_2(g)#, if the initial concentration of #"NO"_2# is #"1 M"#, what are the equilibrium concentrations of #"N"_2"O"_4(g)# and #"NO"_2(g)#?
The equilibrium constant expression is given by
We'll do our I.C.E. chart in the form of bullet points, for fun. Then, our initial concentrations are
INITIAL
CHANGE
And so the final concentrations are
FINAL
Plugging these into the equilibrium constant expression gives us
Use the quadratic equation:
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At equilibrium, the concentration of "N"_2"O"_4(g) will be approximately 0.426 M, and the concentration of "NO"_2(g) will be approximately 0.574 M.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
- Find the equilibrium constant for a 3-electron transfer process, whose standard emf is #"0.59 V"# at #"298.15 K"#? #F = "96485.33 C/mol e"^(-)#
- Given #K_c = 0.36# at #2000^@ "C"# for #"N"_2"O"_4(g) rightleftharpoons "NO"_2(g)#, if the initial concentration of #"NO"_2# is #"1 M"#, what are the equilibrium concentrations of #"N"_2"O"_4(g)# and #"NO"_2(g)#?
- Consider this equilibrium: I2(s) + H2O(l) ⇌ H+(aq) + I-(aq) + HOI(aq). What is the Keq expression for this equilibrium?
- Using the appropriate values of #K_(sp)# and #K _f#, what is the equilibrium constant for the following reaction: #PbCl_2(s) + 3OH^(-)(aq) rightleftharpoons Pb (OH)_3^(-)(aq) + 2Cl^(-)(aq)# ?
- How does #H_3COCH_2CH_2CO_2H# dissociate as an acid?

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