Answer:
In order to determine how many grams of water are needed to form 27.3 grams of oxygen gas, we first need to balance the equation. Once the equation is balanced, we can use stoichiometry to determine the amount of water needed. To balance the equation, we need to add coefficients in front of the reactants and products until the number of atoms of each element is equal on both sides of the equation. Once we do this, the balanced equation looks like this:
2 H2O(l) → 2 H2(g) + O2(g)
Now that the equation is balanced, we can use the molar masses of the reactants and products to determine how many grams of water are needed. The molar mass of water is 18.02 g/mol, the molar mass of hydrogen gas is 2.02 g/mol, and the molar mass of oxygen gas is 32.00 g/mol. So, we can set up a conversion factor using the molar ratios from the balanced equation. We know that for every 2 moles of water, we produce 2 moles of hydrogen