Second law of thermodynamics deals with the spontanelty of a process.
Iron is extracted from the ore `Fe_2O_3`. Using the date given above suggest whether the decomposition of `Fe_2O_3` is feasible or not. Substantiate. `(DeltaH^@= 824 kJ//mol, DeltaS^@ + 0.276 kJ//mol K, T = 298 K).

Assertion: If pure haematite is used as an ore for iron extraction, there is no need of roasting Reason: In the extraction of iron, final product in roasting is Fe_2O_3

The enthalpy change in a process is the same, whether the process is carried out in a single step or inseveral steps. a) Identify tha law stated here. b) Calculate the enthalpy of formation of CH_4 from the following data : i) C_((s))+O_(2(g))rightarrowCO_(2(g)) DeltaH = -393.7kJ/mol ii) H_(2(g))+frac{1}{2}O_(2(g))rightarrowH_2O_((l)) DeltaH = -285.8kJ/mol iii) CH_(4(g))+2O_(2(g))rightarrowCO_(2(g)) DeltaH =-890.4kJ/mol

Electricity and carbon monoxide (CO) and reducing agents used to extract metals from their ores. a) Which of these is used to extract sodium from sodium chloride. Why? b) Which reducing agent is used to extract iron from haematite (Fe_2 O_3) .

Calculate (a) Delta G^0 and (b) the equilibrium constant for the formation of NO_2 from NO and O_2 at 298 K NO_(g)+1 / 2 O_2 (g) hArr NO_2(g) where Delta G_f^0 (NO_2) =52.0 k J / mol Delta G_f^0(NO) =87.0 k J / mol Delta G_f^0(O_2) =0 k J / mol