The molar heat capacity `(C_(P))` of `CD_(2)O` is 10 cals at 1000 K. The change in entropy associated with cooling of 32 g of `CD_(2)O` vapour form 1000 K to 100 K at constant pressure will be : (D= deuterium, at mass =2u)

Molar heat capacity of CD_(2)O (deuterated form of formaldehyde) at constant pressure in 9 cal mol^(-1) K^(-1) at 1000K . Calculate the entropy change associated with cooling of 3.2 g of CD_(2)O vapour from 1000 to 900K .

Molar heat capacity of CD_(2)O (deuterated form of formaldehyde) at constant pressure in 9 cal mol^(-1) K^(-1) at 1000K . Calculate the entropy change associated with cooling of 3.2 g of CD_(2)O vapour from 1000 to 900K .

When two moles of an ideal gas (C_(p.m.)=(5)/(2)R) heated form 300K to 600K at constant pressure, the change in entropy of gas (DeltaS) is:

When two moles of an ideal gas (C_(p.m.)=(5)/(2)R) heated form 300K to 600K at constant pressure, the change in entropy of gas (DeltaS) is:

When two moles of an ideal gas (C_(p.m.)=(5)/(2)R) heated form 300K to 600K at constant pressure, the change in entropy of gas (DeltaS) is:

The entropy change for cooling 1.6 g of an organic compound (mol. Wt. 32, molar heat capacity at constant pressure, 59 JK^(-) mol^(-) ) from 1000 K to 800 K is :

At 1 atm and 298K DeltaH^(0) value of the reaction 2H_(2)(g)+O_(2)(g)to2H_(2)O(l) is -572 kJ. Calculate the change in entropy of the system and surroundings for this reaction. Is this reaction spontaneous at that temperature and pressure? Given: Standard molar entropies of H_(2)(g),O_(2)(g)&H_(2)O(l) at 298K are 130.6, 205.0 and 69.90 J*K^(-1)*mol^(-1) respectively.

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

The entropy change accompanying the heating of one mole of helium gas, assuming ideal behaviour from a temperature of 300 K to a temperature of 1000 K at constant pressure.