How much energy (in `KJ` ) is available for sustaining muscular and nervous activity from the combustion of `1.0` mole of glucose molecules under standard conditions at `37^(0)C` (body temperature)? The standard entropy and enthalpy of reaction are `+200`J/K -mol and `-2808`kJ/mol,respectively.

Animals operate under conditons of constant pressure and most of the process tht maintain life are isothermal ( in a broad sense) . How much energy is available for sustaining this type of muscular and nervous activity from the combustion of 1mol of glucose molecules under standard conditons at 37^(@) C (blood temperature) ? The entropy change is +182.4 JK^(-1) for the reaction stated above DeltaH_("combustion") [glucose]=-2808 KJ

Calculate the entropy change in surroundings when 1.00 mole of H_2O(l) is formed under standard conditions. Delta_fH^@ = -286 kJ mol^(-1)

When 0.36 g of glucose was burned in a bomb calorimeter ( Heat capacity 600 JK^(-1) )the temperature rise by 10 K. Calculate the standard molar enthalpy of combustion (MJ/mole).

Calculate the entropy change in surroundings when 1.00 mol of H_(2)O(l) is formed under standard conditions, Delta_(r )H^(Θ) = -286 kJ mol^(-1) .

The standard enthalpy of formation of octane (C_(8)H_(18)) is -250kJ //mol . Calculate the enthalpy of combustion of C_(8)H_(18) . The enthalpy of formation of CO_(2)(g) and H_(2)O(l) are -394 kJ//mol and -286kJ//mol respectively.

The standard enthalpy or the decomposition of N_2 O_5 to NO_2 is 58.04 kJ and standard entropy of this reaction is 176.7 J/K. The standard free energy change for this reaction at 25^@ C is_____________.

IF the melting point of ice is 273 K and molar enthalpy of usion for ice = 6.0 kJ mol^(-1) , the change in entropy for the fusion of 1 mole of ice will be

Calculate the standard heat of formation of carbon disulphide (l) . Given that the standard heats of combusion of carbon (s) , sulphur (s) and acrbon disulphide (l) are -390, 290.0 , and -1100.0kJ mol^(-1) . Respectively.

The enthalpy and entropy of a reaction are -5.0 kJ//mol and -20 JK^(-1) mol^(-1) respectively and are independent of temperature . What is the highest temperature unto which the reaction is feasible ?

One mole of ethanol is produced reacting graphite , H_2 and O_2 together . The standard enthalpy of formation is -277.7 " kJ mol"^(-1) Calculate the standard enthalpy of the reaction when 4 moles of graphite is involved.