Potassium oxide reacts with water to produce of potassium hydroxide. Please provide a balanced equation, and determine how much potassium oxide is needed to produce 80.5g of potassium hydroxide?

K2O + HOH ==> 2KOH

mols KOH needed = grams/molar mass = ?
mols K2O = (1/2)*mols KOH from the coefficients in the balanced equation.
grams K2O needed = mols K2O x molar mass K2O = ?

To determine the balanced equation for the reaction between potassium oxide (K2O) and water, we need to consider the oxidation states of the elements involved. Potassium has a +1 oxidation state, and oxygen has a -2 oxidation state. Therefore, the oxidation state of oxygen in water (H2O) is -2, and since hydrogen (H) has a +1 oxidation state, the oxidation state of hydrogen in water is +1.

The reaction can be represented as follows:

K2O + H2O → 2 KOH

Now, let's calculate the molar mass of KOH. The molar mass of potassium (K) is approximately 39.10 g/mol, the molar mass of oxygen (O) is approximately 16.00 g/mol, and the molar mass of hydrogen (H) is approximately 1.01 g/mol.

The molar mass of KOH is:
39.10 g/mol (K) + 16.00 g/mol (O) + 1.01 g/mol (H)
= 56.11 g/mol

Using the molar mass of KOH, we can calculate the number of moles of KOH produced from 80.5 g of potassium hydroxide:

Number of moles = Mass / Molar Mass
Number of moles of KOH = 80.5 g / 56.11 g/mol

Now, to find the number of moles of K2O needed, we compare the balanced equation:

1 mole of K2O reacts to produce 2 moles of KOH

So, the number of moles of K2O needed is half of the number of moles of KOH:

Number of moles of K2O = (Number of moles of KOH) / 2

Finally, to find the mass of K2O needed, we can multiply the number of moles of K2O by its molar mass:

Mass of K2O needed = Number of moles of K2O * Molar mass of K2O

By following these steps, you can calculate the mass of potassium oxide needed to produce 80.5 g of potassium hydroxide.