Consider the oxidation of no to no2: no(g)+12o2(g)→no2(g) calculate δg∘rxn at 25∘c. express the free energy change in kilojoules to three significant figures

Given reaction is NO(g)+1/2 O₂(g)→NO₂(g)

ΔGf⁰ [NO₂(g)] = 51.9 kJ/mol

ΔGf⁰ [NO(g)] = 86.6 kJ/mol

ΔGf⁰ [O2(g)] = 0 kJ/mol

ΔG⁰rxn = ΔGf⁰(products) - ΔGf⁰( reactants)

= ΔGf⁰ [NO₂(g)] - {ΔGf⁰ [NO(g)]+ (1/2) ΔGf⁰ [O₂(g)]}

= 51.9 kJ/mol - { 86.6 kJ/mol + 0}

= -34.7 kJ/mol

Therefore, ΔG⁰rxn = -34.7 kJ/mol

The free energy change for the reaction has been -34.7 kJ/mol.

The oxidation has been defined as the loss of electrons by an atom. The change in the Gibbs free energy of the reaction has been given by:

The balanced equation has been given as:

The free energy for the compounds has been given in the image attached.

The change in the energy has been given as:

The free energy change for the reaction has been -34.7 kJ/mol.

Learn more about free energy change, here:

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answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.