The chemical reaction:
CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) ; Δh= -890.4kJ is
Since heat is released as shown in the reaction with a negative sign, the above reaction is exothermic.
On which of the following factors the enthalpy change of a reaction is NOT dependent?
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.
In an endothermic reaction, the value of ΔH is always
According to me, for an endothermic reaction ,the value of ∆H is always >0 .
What is the value of the enthalpy of neutralization for all strong acids and bases?
For all acids and base, enthalpy of neutralisation is -57.1 kJ
The values of ΔH for endothermic and exothermic reactions are
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.
What is the relation between ΔH and ΔU ?
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.
The difference between Cp and Cv is equal to
Cp-Cv = R
R is gas constant whose value is 8.314 J/K/mol
Which of the following reactions is an endothermic process?
For endothermic reactions, enthalpy is with no-ve sign in the end of reaction.
What is the value of γ for a monoatomic gas?
For monatomic species, γ = 1.67
The condition in which q will be equal to ΔH of a system is
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