The heat of combustion of napthalene `{C_(10)H_(8)(s)}` at constant volume was measured to be `-5133 kJ mol^(-1)` at 298 K. Calculate the value of enthalpy change (Given `R=8.314 JK^(-1)mol^(-1)`)

The heat of combustion of solid naphthalene. (C_(10)H_(10)) at constant volume was -4984kJmol^(-1) " at " 298K. Calculate the value of enthalpy change. Given: C_(10)H_(8_((s)))+120_(2_((g)))rarr10CO_(2_((g)))+4H_(2)O_((l)),DeltaU=-4984 kJ.mol^(-1) DeltaU=-4984 kJmol^(-1),R=8.314JK^(-1)mol^(-) T=298K

The heat of combustion of C_10H_8(s) at constant volume is -5133kJ mol_-1 at 298K. Calculate the value of enthalpy change. (R=8.314 JK_-1 mol_-1)

The heat of combustion of gaseous methan (CH_(4)) at constant volume is measured in a bomb calorimeter at 298 K and is found to be -885.4 kJ mol^(-1) .Find the value of enthalpy change.

The combustion of benzene(/) gives CO_2(g) and H_2O(l) Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol^(-1) at 25^@C , heat of combustion (in kJ mol^(-1) ) of benzene at constant pressure will be (R = 8.314 JK^(-1) mol^(-1))

The standard free energy change of a reaction is DeltaG^(@)=-kJ//mol^(-1) at 298 K. Calculate the value of log_(10)K_(p) (R=8.314JK^(-1)mol^(-1))

The standard free energy change of a reaction is DeltaG^(@)=-115kJ//mol^(-1) at 298 K. Calculate the value of log_(10)K_(p) (R=8.314JK^(-1)mol^(-1))