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What is the value of Kc here?

Answer 1

Serenity Allen

#K_c = "0.006 94"#

The formula for your chemical reaction is

#"N"_2"O"_4 ⇌ "2NO"_2#

#K_c = (["NO"_2]^2)/(["N"_2"O"_4])#

To address this issue, we can set up an ICE table.

#color(white)(mmmmmmml)"N"_2"O"_4 ⇌ "2NO"_2# #"I/mol·L"^"-1": color(white)(mll)0.0300color(white)(mmll)0# #"C/mol·L"^"-1":color(white)(mml) "-"xcolor(white)(mmm)"+2"x# #"E/mol·L"^-1": color(white)(m)0.0236color(white)(mml)2x#

From the #"N"_2"O"_4# concentrations, we see that

#0.0300 - x = 0.0236#

∴ #x = "0.0300 - 0.0236 = 0.0064"#

So, #["NO"_2]_text(eq) = 2xcolor(white)(l) "mol/L" = "(2 × 0.0064) mol/L" = "0.0128 mol/L"#

#K_"c" = 0.0128^2/0.0236 = "0.006 94"#

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Answer 2

Cameron Andrews

To determine the value of Kc, we need the balanced chemical equation and the concentrations of reactants and products at equilibrium. Could you please provide more context or specify the chemical reaction in question?

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Answer from HIX Tutor

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.