For the conversion of 1 mole of `SO_(2)(g)` into `SO_(3)(g)` the enthalpy of reaction at constant volume. `DeltaU`, at 298 K is `-97.027kJ`. Calculate the enthalpy of reaction, `DeltaH`, at constant pressure.

For the conversion of 1 mole of SO_2(g) to SO_3(g) the heat of reaction at constant volume ( Delta U^@ ) at 298K is -97.027 KJ Calculate the enthalpy change ( Delta H^@ )

The enthalpy of formation of methane at constant pressure and 300 K is-78.84 kJ. What will be the enthalpy of formation at constant volume?

The enthalpy change for the reaction N2(g) + 3 H2(g) → 2 NH3(g) is -91.8 kJ at 298 K. Calculate the enthalpy of formation of ammonia?

The enthalpy of formation of CH_(4(g)) , at constant pressure is -76 kJ,at 300 K. What will be its enthalpy of formation at constant volume?

Change in enthalpy and change in internal energy are state functions. The value of DeltaH, DeltaU can be determined by using Kirchoff's equation. I mole of naphthalene (C_(10)H_(8)) was burnt is oxygen gas at 25^(@)C at constant volume. The heat evolved was found to be 5138.8kJ. Calculate the heat of reaction at constant pressure

Change in enthalpy and change in internal energy are state functions. The value of DeltaH, DeltaU can be determined by using Kirchoff's equation. I mole of naphthalene (C_(10)H_(8)) was burnt is oxygen gas at 25^(@)C at constant volume. The heat evolved was found to be 5138.8kJ. Calculate the heat of reaction at constant pressure

For the reaction 1/8 S_(8)(s) + 3/2O_(2)(g) rightarrow SO_(3)(g), the difference of heat change at constant pressure and constant volume at 27 ^(@)C will be.

For the reaction 1/8 S_(8)(s) + 3/2O_(2)(g) rightarrow SO_(3)(g), the difference of heat change at constant pressure and constant volume at 27 ^(@)C will be.