for the rxn. 2no2 equilibrium to 2 no +o2 kc for that is 1.8 ×10 ki power -6 at 185 degree Celsius at 185 degree the value of kc for no+1÷2o2 equilibrium to no2
Oh, the power of abbreviations when sending texts, and it then translates to posts on boards into gibberish.
To find the value of Kc for the reaction:
2NO2 ⇌ 2NO + O2
given that Kc = 1.8 × 10^-6 at 185 degrees Celsius, we can use the relationship between the forward and reverse reactions.
Kc is the equilibrium constant, which is defined as the ratio of the product concentrations to the reactant concentrations, each raised to their respective stoichiometric coefficients.
2NO2 ⇌ 2NO + O2
The reaction can also be written as:
2NO + 1/2O2 ⇌ 2NO2
To find the value of Kc for the reverse reaction, we take the reciprocal of the equilibrium constant for the forward reaction.
Kc(reverse) = 1/Kc(forward)
So, Kc(reverse) = 1/(1.8 × 10^-6)
Calculating this value, we get:
Kc(reverse) = 5.56 × 10^5
Therefore, at 185 degrees Celsius, the value of Kc for the reaction:
NO + 1/2O2 ⇌ NO2
is 5.56 × 10^5.