The reaction of cyanamide, `NH_2CN(s)` with oxygen was carried out in a bomb calorimeter and `DeltaU` was found to be `- 742.7 kJ mol^-1` at 298 K. Calculate the enthalpy change for the reaction at 298 K.

The reaction of cyanamide, NH_2CN(s) with O_2 was carried out in a bomb calorimeter and Delta U was found to be -742.7 kJ mol^-1 at 298 K. Calculate enthalpy change for the reaction at 298K. NH_2CN(s)+3/2O_2(g)rarrN_2(g)+CO_2(g)+H_2O(l)

The heat of combustion of methane at constant volume measured in a bomb caloriemeter at 298K is found to be -885389 Jmol -1, Calculate the value of heat of combustion at constant pressure.

Enthalpy of formation of ammonia is - '46.0 kJ mol^(-1)'. The enthalpy change for the reaction: '2 NH_3(g) rarr N_2(g)+3 H_2(g)'

Enthalpy and entropy changes of a reaction are 40.63 kJ mol^_1 and 108.8 JK^-1 . Predict the feasibility of the reaction at 27^@C .

For the reaction: 2AZ_(g) + B_(g) rarr 2D_(g) DeltaU^@ = -10.5 kJ//mol DeltaS^@ = -44.1 kJ//mol at 298 K. Calculate DeltaG^@ for the reaction.