Write the equilibrium constant expression for the reaction below in terms of the
ID: 503727 • Letter: W
Question
Write the equilibrium constant expression for the reaction below in terms of the concentrations of the reactants and products: 2 N_2O_5(g) 4 NO_2(g) + O_2(g) Calculate the equilibrium constant for the reaction in question 1 if the concentrations of the species were known to be: [N_2O_5] = 0.0540 M [NO_2] = 0.0128 M [O_2] = 0.106 M A 2.00-L flask is filled with 0.200 moles of hydrogen iodide which decomposes 453 degree C. At equilibrium, [HI] = 0.078 M. Calculate K_c for this reaction: 2 HI(g) H_2(g) + I_2(g)Explanation / Answer
2N2O5 (g) <==> 4NO2 (g) + O2(g)
Kc = [NO2]^4[O2]/[N2O5]^2
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2.
Kc = (0.0128)^4(0.106)/(0.054)^2
= 9.75*10^-7
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