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2. Calculate the value of the equilibrium constant (Kc) for the reaction shown, if NO2(g) was found to be 95.54 % decomposed at 45.00 °C when its initial concentration was 5.725 mol/L. The initial concentration of the reaction products is 0 mol/L. 2NO2(g)...

3. Calculate the value of the equilibrium constant (Kc) for the reaction displayed if the following equilibrium concentration data were measured at 723.0 K: [N2(g)] = 2.936 mol/L, [H2(g)] = 2.933 mol/L, [NH3(g)] = 3.443 mol/L. N2(g)+3H2(g) = 2NH3(g)

4. The initial concentration for the compounds involved in the reaction shown were determined to be [ClF(g)] = 0.5789 mol/L, [F2(g)] = 0.5980 mol/L, [Cl2(g)] = 0.05037 mol/L. Calculate the value of the equilibrium constant (Kc) at 2500 K if the equilibriu...