Fill in a suitable numerical value or an expression to the blanks in the following sentences, describing the temperature and pressure dependences in the chemical reactions. In the cases of (e)(f), choose the appropriate phrase. Use gas constant R = 8.314 [JK-1mol-1], if necessary.

(A) Consider the influence of temperature in the reduction of cobalt oxide CoO (eq.(i))

CoO(s) + CO(g) Co(s) + CO₂(g) H = 44.1 [kJmol¹] (i)

(where (s) denotes solid phase, (g) denotes gas phase, and H denotes the enthalpy change under 1.013 10⁵ [Pa](= 1 [atm]) at 298 [K])

When the standard entropies S of CoOCOCo, and CO₂ are 53.0197.130.0, and 213.6 [JK¹mol¹] under 1.013 10⁵ [Pa](= 1 [atm]) at 298 [K], the change of entropy S and the change of standard Gibbs free energy G are determined to be ( a ) [JK¹mol¹] and ( b )[Jmol¹], respectivelyThe change of Gibbs free energy G in the reaction of eq. (i) is expressed as ( c ) by using partial pressure of CO and CO₂ (P_CO and P_CO2)and activity of CoO and Co (a_CoO and a_Co). If the solid activity is 1 under 5 mol% CO and 95 mol% CO₂ atmosphere, G is determined to be ( d ) [Jmol¹]which indicates that the reduction of CoO proceeds under this conditionsAccording to the vant Hoff equation (ii), which expresses the temperature dependency of equilibrium constant K, it can be found that the (eexothermicendothermic) reaction (i) will (fincreasedecrease) the productivity of Co with increasing the temperature at constant pressure.

(lnK/T)p = H/RT² (ii)