Answer:
There will be formed 39.1935 grams H2O formed
Explanation:
<u>Step 1:</u> The balanced equation
2H2 + 02 → 2H20
<u>Step 2</u>: Given data
mass of hydrogen = 14.8 grams
Molar mass of hydrogen = 2.02 g/mole
mass of oxygen = 34.8 grams
Molar mass of oxygen = 32 g/mole
<u>Step 3: </u>Calculate moles
moles = mass / Molar mass
moles of hydrogen = 14.8g/ 2.02 g/mole = 7.33 moles
moles of oxygen = 34.8g / 32g/mole = 1.0875 moles
For 2 moles hydrogen consumed, we need 1 mole of oxygen.
This means oxygen is the limiting reagens and will be consumed completely. Hydrogen is the reactant in excess, there will remain 5.155 moles of hydrogen
<u>Step 4:</u> Calculate moles of H2O
We see that for 2 moles of H2 consumed, there is needed 1 mole of O2, to produce 2 moles of H2O.
For 1.0875 moles of oxygen consumed, there will be produced 2.175 moles of H2O
<u>Step 5:</u> Calculate mass of water
Mass of H2O = moles of H2O * Molar mass of H2O
Mass of H2O = 2.175 moles * 18.02 g/moles 39.1935 grams
There will be formed 39.1935 grams H2O formed
