Which of the following reactions will have the value of enthalpy of neutralisation as `-57.1"kJ mol"^(-1)` ?

The enthalpy of neutralization is about 57.3 kJ for the pair

Acetic acid ( ethanoic acid ) and hydrochloric acid react with KOH solution. The enthalpy of neutralisation of ethanoic acis is -55.8kJ mol^(-1) while that of hydrochloric acid is -57.3kJ mol^(-1) . Can you think of how are these different?

What would be the heat released when an aqueous solution containing 0.5 mol if HNO_(3) is mixed with 0.3 mol of OH^(-1) (enthalpy of neutralisation is -57.1 kJ )

A reaction is at equilibrium at 100^(@)C and the enthalpy change for the reaction is "42.6 kJ mol"^(-1) . What will be the value of DeltaS in "J K"^(-1)"mol"^(-1) ?

In a hypothetical reaction X to Y , the activation energy for the forward backward reactions are 15 and 9 kJ mol^(-1) respectively. The potential energy of X is 10 kJ mol^(-1) . Which of the following statement is/are correct? (i) The threshold energy of the reaction is 25 kJ mol^(-1) (ii) The potential energy of Y is 16 kJ mol^(-1) (iii) Heat of reaction is 6 kJ mol^(-1) The reaction is endothermic.

Bond dissociation enthalpies of H_(2(g)) and N_(2(g)) are "426.0 kJ mol"^(-1) and "941.8 kJ mol"^(-1) , respectively, and enthalpy of formation of NH_(3(g))" is "-"46 kJ mol"^(-1) . What are the enthalpy of atomisation of NH_(3(g)) and the average bond enthalpy of N-H bond respectively ( in kJ "mol"^(-1) )?

The fat, C_(57)H_(104)O_(6)(s) , is metabolized via the following reaction. Given the enthalpies of formation, calculate the energy (kJ) liberated when 1.0 g of this fat reacts. C_(57)H_(104)O_(6)(s)+80 O_(2)(g)rarr57CO_(2)(g)+52 H_(2)O(l) Delta_(f)H^(@)(C_(57)H_(104)O_(6),s)=-70870" kJ"//"mol, "Delta_(f)H^(@)(H_(2)O,l)=-285.8 " kJ"//"mol" , Delta_(f)H^(@)(CO_(2),g)=-393.5 " kJ"//"mol"

For an endothermic reaction, where Delta H represents the enthalpy of reaction in kJ mol^(-1) , the minimum value for the energy of activation will be

A catalyst lowers the activation energy of a reaction form 20 kJ mol^(-1) to 10 kJ mol^(-1) . The temperature at which the uncatalyzed reaction will have the same rate as that of the catalyzed at 27^(@)C is

The enthalpy of solution of sodium chloride is 4 kJ mol^(-1) and its enthalpy of hydration of ion is -784 kJ mol^(-1) . Then the lattice enthalpy of NaCl (in kJ mol^(-1) ) is