The following equation represents the decomposition of a generic diatomic element in its standard state.1/2 X2(g) ---> X(g)Assume that the standard molar Gibbs energy of formation of X(g) is 5.45 kJ

The reaction below represents the decomposition of a generic diatomic molecule in its standard state.1/2 A2(g) → A(g)Assuming that the standard molar Gibbs energy of formation of A(g) is 8.12 kJ•mol–1 at 2500 Kand –72.20 kJ•mol–1 at 3500 K, determine the value of ΔH°rxn for these data assuming that ΔH°rxn is independent of temperature. Express your answer in kJ, in one decimal place.

The cell in which the following reaction occurs has at 298 K. The standard Gibbs energy will be

4. Give the thermochemical equation for the decomposition of ammonia, NH3.NH3 (g) —> 3/2 H2 (g)  + 1/2 N2 (g)                    ΔH = 29.61 kJ*3 pointsNH3 (g) —> 3/2 H2 + 1/2 N2 (g) + 29.61 kJNH3 (g) + 29.61 kJ —> 3/2 H2 + 1/2 N2 (g)NH3 (g) —> 3/2 H2 + 1/2 N2 (g) - 29.61 kJNH3 (g) - 29.61 kJ —> 3/2 H2 + 1/2 N2 (g)Is the reaction in no. 4  endothermic or exothermic?*2 pointsendothermicexothermic

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)

The following reaction is performed at 298 K. 2NO(g) + O2(g) ⇌ 2NO2(g), Kp = 1.6 × 1012The standard free energy of formation of NO(g) is 86.6 kJ/mol at 298 K. What is the standard free energy of formation of NO2(g) (in J mol–1) at 298 K ?