`300K` এবং `20atm`-এ `N_(2)` গ্যাসের `2.8g` ইসাওথার্মালভাবে প্রসারিত করার অনুমতি দেওয়া হয়েছিল

The values of K_(p)//K_(c) for the following reactions at 300 K are, respectively : (At 300 K, RT = 24.62 d m^(3) atm mol^(-1) ) N_(2)(g)+O_(2)(g)hArr 2 NO(g) N_(2)O_(4)(g)hArr2 NO_(2)(g)

ii. One mole of N_(2)O_(4)(g) at 100 K is kept in a closed container at 1.0 atm pressure. It is heated to 300 K , where 30% by mass of N_(2)O_(4)(g) decomposes to NO_(2)(g) . The resultant pressure will be

For the reaction: CO(g) +H_(2)O(g) hArr CO_(2)(g) +H_(2)(g) (Delta_(r)H)_(300K) = 41.2 kJ mol^(-1) (Delta_(r)H)_(1200K) =- 33.0 kJ mol^(-1) (Delta_(r)S)_(300K) = -4.2 xx 10^(-2) kJ mol^(-1) (Delta_(r)S)_(1200K) =- 3.0 xx10^(-2) kJ mol^(-1) Predict the direction of spontaneity of the reaction at 300K and 1200K . also calculated log_(10)K_(p) at 300K and 1200K .

For N_(2(g) at 1 atm to N_(2)(g) at 0.5 atm, What would be the change in entropy ?

Density of dry air ( only N_(2) and O_(2)) is 1.24g litre^(-1) at 760 m m and 300 K . Find the partial pressure of N_(2) gas in aire. ( Take R=(1)/(12) litre litre atm // mol K, mol. Wt. of N_(2) =28)