Consider the following reaction at 298 K.32O2( g)⇌O3( g)⋅KP=2.47×10−29.ΔrG⊕ for the reaction is _______ kJ. (Given R =8.314JK−1 mol−1)

51. What is the ΔH° at 298 K of the given reaction?*- 3.8 kJ/mol3.8 J/mol0Cannot defined

Calculate ΔrG(in kJ/mol) for given reaction at 300 KN2(g) + O2(g) ⇌ 2NO(g)the partial pressure of N2, O2 & NO are 10–4 bar, 10–2 bar and 10–5 bar respectively when mixed together at 300 K.Given : 2.303 RT = 5750 J/molAt 300 K standard enthalpy of formation of NO(g) = 90.5 kJ mol–1,Standard molar entropy data at 300 K :S°(N2, g) = 190 J K–1 mol–1S°(NO, g) = 210 J K–1 mol–1S°(O2,g) = 205 J K–1 mol–1 ?

The equilibrium constant, KC, for the following reaction at 726.85 °C is 2.71 × 102.2SO2(g) + O2(g) ⇌ 2SO3(g)The KP for this reaction at the same temperature is

For a certain reaction at 300 K, K=10, then ΔG∘ for the same reaction is _______ ×10−1 kJ mol−1

The value of ΔH° for the reaction below is - 790 kJ.2S(s) + 3O2(g) → 2SO3(g)The enthalpy change accompanying the reaction of 0.95 g of S is ________kJ.Question 4Select one:a.23b.-23c.-12d.12e.-790