How many moles of potassium oxide will be formed when 1.52 moles of potassium reacts with oxygen according to the following equation:
4k + o2 -> 2k2o

0.76 mol.

Explanation:

From the balanced equation: 4K + O₂ → 2K₂O,It is clear that 4.0 moles of K react with 1.0 mole of oxygen to produce 2.0 moles of K₂O.We can use cross multiplication to get the no. of moles of potassium oxide will be formed when 1.52 moles of potassium reacts with oxygen:

4.0 moles of K will produce → 2.0 moles of K₂O.

1.52 moles of K will produce → ??? moles of K₂O.

∴ The no. of moles of potassium oxide will be formed when 1.52 moles of potassium reacts with oxygen = (1.52 mol)(2.0 mol)/(4.0 mol) = 0.76 mol.

Given data,temperature, t = 230°c = 503 kconsider the chemical reaction,ch₃oh(l) + 1/2 o₂(g)  → ch₂o(g) + h₂o(l)calculate the enthalpy change for the reaction: δh⁰rxn =  σnδh⁰f(products) -  σmδh⁰f(reactants)substitute the values from the table: δh⁰rxn = { -115.9 + (-285.8)} - {0+(-238.7)}              = -163.0 kjcalculate the entropy change for the reaction.δs⁰rxn = (219 + 70) - (127.2 + 1/2 x 205.2) = 59.2 j/kconsider the expression for free energy: δg⁰rxn =  δh⁰rxn - t  δs⁰rxnsubstitute the values in the above equationδg⁰rxn = -163 x 10³ - (503 x 59.2)              = -192777.6 j              = -192.777 kj