How many grams of H2O are needed if 41.85g of O2 are to be produced from the reaction below?

2K2O2 + 2H2O = 4KOH + O2

mols O2 = grams/molar mass O2 = ?

Using the balanced equation, convert mols O2 to mols H2O. You can seee that 1 mol O2 requires 2 mols H2O.
Then convert mols H2O to grams H2O. grams H2O = mols x molar mass = ?

To determine the amount of H2O needed to produce a certain amount of O2, we need to use the balanced equation and the concept of stoichiometry.

In this balanced equation, it shows that 2 moles of K2O2 react with 2 moles of H2O to produce 4 moles of KOH and 1 mole of O2.

To find the amount of H2O needed to produce 41.85g of O2, we can follow these steps:

Step 1: Calculate the molar mass of O2.
The molar mass of O2 is 32.00 grams/mole (16.00 grams/mole * 2 O atoms).

Step 2: Convert the given mass of O2 to moles.
Divide the given mass of O2 (41.85g) by the molar mass of O2 (32.00 grams/mole) to get the number of moles.

41.85g / 32.00 grams/mole ≈ 1.31 moles

Step 3: Use the stoichiometry ratio to find the moles of H2O.
According to the balanced equation, 2 moles of K2O2 react with 2 moles of H2O to produce 1 mole of O2.
So, the ratio of H2O to O2 is 2:1.

Multiply the number of moles of O2 (from Step 2) by the stoichiometric ratio to find the moles of H2O.

1.31 moles * (2 moles H2O / 1 mole O2) ≈ 2.62 moles H2O

Step 4: Convert moles of H2O to grams.
Multiply the number of moles of H2O (from Step 3) by the molar mass of H2O (18.02 grams/mole) to get the mass of H2O.

2.62 moles H2O * 18.02 grams/mole ≈ 47.19 grams

Therefore, approximately 47.19 grams of H2O are needed to produce 41.85 grams of O2.