`2(Ag)toB(g), deltaH=-20kcal//mol`. In a closed rigid container, 0.2mole of `A(g)` at constant temperature `727^(@)C` convert into B(g) then, change in heat energy in the process will be:
`(R=2cal//"mole"-K)`

5 mole H_(2)O(l) at 373 K and 1 atm is converted into H_(2)O(g) at 373 K and 5 atm . DeltaG for this process is [Given: R = 2 cal/K-mol]

For the reaction A(g)+2B(s)toC(l)+D(g)," "Delta H=-40 kJ//"mole" 10 mole of each A and B are mixed in a closed rigid container and allowed to react at 300 K. Calculate the heat transfer (in kJ) occurs in the process. [Use : R=8.3 "J"//"K-mole" ]

1672 cal of heat is given to one mole of oxygen at 0^(@)C keeping the volume constant. Rise in temperature is (R = 2 cal/mole/ ""^(@) K)

2A(s)hArrB(g)+2C(g)+3D(g) Total pressure developed in closed container by decomposition of A at equibrium is 12 atm at 727^(@)C . Calculate DeltaG^(@) (in kcal), of the reaction at 727^(@)C . ( R=2 cal//"mole"-K,In 2=0.7, In =1.1 ) Round off your answer to integer (without sign).

1672cal of heat is given to one mole of oxygen at 0^(@)C keeping the volume constant. Raise in temperature is (c_(p)=0cal//gm^(0)k and R=2cal//"mole"//K)

For the reaction : 2A(g)+B(g)toC(g) Change in enthalpy is 30 "kcal"//"mole whereas" DeltaU " is " 32 "kcal"//"mole" at certain temperature. Calculate the work done (in kcal) when 4 mole of A reacts with excess of B at constant pressure and same temperature.

The equilibrium constant of the reaction A_(2)(g)+B_(2)(g)hArr2AB(g) at 100^(@)C is 50. If a one litre flask containing one mole of A_(2) is connected to a two litre flask containing two moles of B_(2) , how many moles of AB will be formed at 373 K ?