(a) What is reversible process in Thermo-dynamics? (b) Name the therm

1.	(a) What is reversible process in Thermo-dynamics? (b) Name the thermodynamic process for which (i) q = 0 (ii) ∆U = 0 (iii) ∆v = 0(iv) ∆P = 0 (c) Water decomposes by absorbing 286.2 kJ of electrical energy per mole. When H2 and O2 combine to form one mole of H2O, 286.2 kJ of heat is produced, which thermodynamic law is proved? Write its statement.
Answer» (a) Reversible Process: It is defined as a system where change takes place infinitesimally slow and the direction of which at any point can be reversed by infinitesimal change in the state of the system. (b) (i) For q = 0, heat is constant, so the process is adiabatic process. (ii) For ∆U = 0, internal energy is constant which takes place at constant temperature, so, the process is isothermal process. (iii) For ∆V = 0, volume is constant, so the process is isochoric process. (iv) For ∆P = 0, pressure is constant, so the process is isobaric process. (c) H₂O(g) → H₂ (g) + \(\frac{1}{2}\)O₂(g); ∆_rH^Θ = 286.2 kJ mol⁻¹ H₂ (g) + \(\frac{1}{2}\)O₂ (g) → H₂O(s); ∆_rH^Θ = −286.2 kJ mol⁻¹ It is referred to as first law of thermodynamics. According to this law, “energy can neither be created nor be destroyed but can be converted from one form to another"

(a) What is reversible process in Thermo-dynamics? (b) Name the thermodynamic process for which (i) q = 0 (ii) ∆U = 0 (iii) ∆v = 0(iv) ∆P = 0 (c) Water decomposes by absorbing 286.2 kJ of electrical energy per mole. When H2 and O2 combine to form one mole of H2O, 286.2 kJ of heat is produced, which thermodynamic law is proved? Write its statement.

Answer»

(a) Reversible Process: It is defined as a system where change takes place infinitesimally slow and the direction of which at any point can be reversed by infinitesimal change in the state of the system.

(b) (i) For q = 0, heat is constant, so the process is adiabatic process.

(ii) For ∆U = 0, internal energy is constant which takes place at constant temperature, so, the process is isothermal process.

(iii) For ∆V = 0, volume is constant, so the process is isochoric process.

(iv) For ∆P = 0, pressure is constant, so the process is isobaric process.

(c) H₂O(g) → H₂ (g) + \(\frac{1}{2}\)O₂(g);

∆_rH^Θ = 286.2 kJ mol⁻¹

H₂ (g) + \(\frac{1}{2}\)O₂ (g) → H₂O(s);

∆_rH^Θ = −286.2 kJ mol⁻¹

It is referred to as first law of thermodynamics. According to this law, “energy can neither be created nor be destroyed but can be converted from one form to another"

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