What mass of water is needed to react completely with the Na2O2?
Answer in units of g.
To find the mass of water needed to react completely with Na2O2, we need to determine the balanced chemical equation for the reaction between Na2O2 and water.
The formula for sodium peroxide is Na2O2, which consists of two sodium ions (Na+) and one peroxide ion (O2-). When Na2O2 reacts with water (H2O), it undergoes hydrolysis, producing sodium hydroxide (NaOH) and hydrogen peroxide (H2O2).
The balanced chemical equation for the reaction is:
Na2O2 + H2O → 2NaOH + H2O2
From the balanced equation, we can see that one mole of Na2O2 reacts with one mole of H2O to produce two moles of NaOH and one mole of H2O2.
To find the mass of water needed, we need to determine the molar ratio between Na2O2 and H2O. The molar mass of Na2O2 is calculated as follows:
Na: 2(22.99 g/mol) = 45.98 g/mol
O: 2(16.00 g/mol) = 32.00 g/mol
Na2O2: 45.98 g/mol + 32.00 g/mol = 77.98 g/mol
To perform the calculation, we need to convert the given mass of Na2O2 into moles. Let's assume we have "x" grams of Na2O2.
Moles of Na2O2 = Mass (g) / Molar mass (g/mol)
Moles of Na2O2 = x g / 77.98 g/mol
According to the balanced equation, the molar ratio between Na2O2 and H2O is 1:1. Therefore, the moles of H2O needed are also "x g / 77.98 g/mol".
Finally, we need to convert moles of H2O to grams by using the molar mass of water:
H: 2(1.01 g/mol) = 2.02 g/mol
O: 16.00 g/mol
H2O: 2.02 g/mol + 16.00 g/mol = 18.02 g/mol
Mass of water needed = Moles of H2O × Molar mass of H2O
Mass of water needed = (x g / 77.98 g/mol) × 18.02 g/mol
Simplifying the expression:
Mass of water needed = (x × 18.02 g) / 77.98
Therefore, the mass of water needed to react completely with Na2O2 is given by the expression (x × 18.02 g) / 77.98, where "x" represents the mass of Na2O2 in grams.