For the reaction Fe2O3(s) + 3H2(g)2Fe(s) + 3H2O(g) H°rxn = 98.8 kJ and S°rxn = 142.5 J/K The standard free energy change for the reaction of 2.47 moles of Fe2O3(s) at 267 K, 1 atm would be kJ. This reaction is (reactant, product) favored under standard conditions at 267 K. Assume that H°rxn and S°rxn are independent of temperature.

Answer :

The value of standard Gibbs free energy is, 60.8 kJ

This reaction is reactant favored under standard conditions at 267 K.

Explanation :

As we know that,

where,

= standard Gibbs free energy  = ?

= standard enthalpy = 98.8 kJ = 98800 J

= standard entropy = 142.5 J/K

T = temperature of reaction = 267 K

Now put all the given values in the above formula, we get:

As we know that:

As, the value of is more than zero that means the reaction is non-spontaneous and reaction will be favored in the backward direction that means favored in reactants.

answer

i think the answer is a) as air pressure in an area increases, the density of the gas particles in that area decreases.

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it is a solid

explanation: