Test: Measurement of du & dh - NEET MCQ

Since heat is released as shown in the reaction with a negative sign, the above reaction is exothermic.

Enthalpy change for any process is a state function. It depends only on the initial and final conditions.
Similarly, Enthalpy change of a reaction does not depend upon different intermediate reactions.
△H=H_p−H_r

According to me, for an endothermic reaction ,the value of ∆H is always >0 .

For all acids and base, enthalpy of neutralisation is -57.1 kJ

For endothermic reaction, ∆H = positive value since heat is absorbed during the course of reaction. For exothermic, ∆H = negative value as heat is released during the course of reaction.

Enthalpy is a state function, and the change in enthalpy of a system is equal to the sum of the change in the internal energy of the system ΔH = ΔU + ΔnRT and the PV work done. Enthalpy is a state function whose change indicates the amount of heat transferred from a system to its surroundings or vice versa, at constant pressure.

Cp-Cv = R
R is gas constant whose value is 8.314 J/K/mol

For endothermic reactions, enthalpy is with no-ve sign in the end of reaction. 

For monatomic species, γ = 1.67

Under the condition, the heat q of the reaction is equal to the enthalpy change ΔH of the system. Under constant pressure and temperature, the free energy in a reaction is known as Gibbs free energy G.
G = H - TS