how many grams of H are needed to produce 1.80grams of H2O
1.8 g H2O x (1 mol/18g) = 0.1 mol H2O. There are two moles H per mol H2O; therefore, 0.2 mol of H atoms.
0.2 x (1 g H/1 mol H) = 0.2 grams H needed.
To determine how many grams of hydrogen (H) are needed to produce 1.80 grams of water (H2O), we need to understand the molecular formula of water. Water consists of two hydrogen atoms and one oxygen atom, so we can rewrite the equation as:
2H2 + O2 → 2H2O
From the balanced equation, we can see that two moles of water (H2O) are produced from four moles of hydrogen gas (H2). Given the molar mass of hydrogen (H) is 1.008 grams/mol, we can find the molar mass of water (H2O) by adding its constituent elements' molar masses.
The molar mass of oxygen (O) is 16.00 grams/mol, and since there is one oxygen atom in one molecule of water, the molar mass of water is:
Molar mass (H2O) = (2 × molar mass (H)) + molar mass (O)
= (2 × 1.008 g/mol) + 16.00 g/mol
≈ 18.016 g/mol
Now, we can use the molar mass of water (H2O) to calculate the number of moles of water produced when we have 1.80 grams of it:
Number of moles = Mass / Molar mass
= 1.80 g / 18.016 g/mol
≈ 0.0999 ≈ 0.10 mol (rounded to two decimal places)
From the balanced equation, we know that for every 2 moles of water, we also need 4 moles of hydrogen gas. Therefore, we can set up the following proportion:
4 moles H2 / 2 moles H2O = x moles H / 0.10 moles H2O
Simplifying the proportion:
x = (4/2) × 0.10
x = 0.20 mol H
Finally, we can calculate the mass of hydrogen (H) needed using its molar mass:
Mass = Number of moles × Molar mass
= 0.20 mol × 1.008 g/mol
≈ 0.2016 g ≈ 0.20 grams
Therefore, approximately 0.20 grams of hydrogen (H) are needed to produce 1.80 grams of water (H2O).