At 25.0oC, for the reaction 2NO2(g) ⇌ N2O4(g) the values of ΔHo and ΔSo are –58.03 kJ/ mol and –176.6 J K-1mol-1, respectively. Calculate the value of K at 25.0oC. Assuming ΔHo and ΔSo are temperature independent, estimate the value of K at 100.0oC.
Answer to relevant QuestionsConsider the relationship The equilibrium constant for some hypothetical process was determined as a function of temperature (in kelvins) with the results plotted below. From the plot, determine the values of ΔHo and ΔSo ...A sample of 1.75 moles of H2 (Cv = 20.5 J K-1mol-1) at 21oC and 1.50 atm undergoes a reversible adiabatic compression until the final pressure is 4.50 atm. Calculate the final volume of the gas sample and the work associated ...The enthalpy of vaporization of chloroform (CHCl3) is 31.4 kJ/ mol at its boiling point (61.7oC). determine ΔSsys, ΔSsurr, and ΔSuniv when 1.00 mole of chloroform is vaporized at 61.7oC and 1.00 atm. Consider the reactions Ni2+(aq) + 6NH3(aq) → Ni(NH3)62+(aq) (1) Ni2+(aq) + 3en(aq) → Ni(en)32+(aq) (2) Where en = H2NOCH2OCH2ONH2 The ΔH values for the two reactions are quite similar, yet Kreaction2 > Kreaction1. ...One mole of an ideal gas with a volume of 6.67 L and a pressure of 1.50 atm is contained in a vessel with a movable piston. The external pressure is suddenly increased to 5.00 atm and the gas is compressed isothermally (T = ...
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