How many grams of water must decompose to produce 2 grams of hydrogen and 16 grams of oxygen?
18g of H2O or one mole of H20.
18 grams
To determine the number of grams of water required to produce a certain amount of hydrogen and oxygen, we need to use the ratio of the molar masses of water, hydrogen, and oxygen.
The molar mass of water (H2O) is approximately 18 grams/mol, consisting of 2 grams/mol of hydrogen and 16 grams/mol of oxygen.
To find the number of moles of hydrogen and oxygen produced, we divide the given masses by their respective molar masses:
Number of moles of hydrogen = 2 grams / 2 grams/mol = 1 mol
Number of moles of oxygen = 16 grams / 16 grams/mol = 1 mol
Since water consists of two moles of hydrogen and one mole of oxygen, we can conclude that the reaction requires twice as many moles of hydrogen as oxygen.
To determine the number of moles of water required for this reaction, we take the moles of oxygen and divide by two:
Number of moles of water = (1 mol of oxygen) / 2 = 0.5 mol
Finally, to find the mass of water required, we multiply the number of moles of water by its molar mass:
Mass of water = 0.5 mol × 18 grams/mol = 9 grams
Therefore, to produce 2 grams of hydrogen and 16 grams of oxygen, 9 grams of water must decompose.