What is the mass of water that results from combining 2.0g of hydrogen with 16.0g of oxygen?
To find the mass of water formed when hydrogen and oxygen combine, we first need to determine the ratio in which they combine. The chemical equation for the reaction between hydrogen and oxygen to form water is:
2H₂ + O₂ → 2H₂O
From the equation, we can see that 2 moles of hydrogen combine with 1 mole of oxygen to produce 2 moles of water.
To calculate the amount of water formed, we can use the concept of molar mass:
1 mole of H₂O = 2(1.01 g/mol) + 16.00 g/mol = 18.02 g/mol
From the equation, 2 moles of water are produced for every 2 moles of H₂O.
Therefore, the mass of water formed is:
2 moles of H₂O × 18.02 g/mol = 36.04 g
Hence, when 2.0g of hydrogen and 16.0g of oxygen are combined, the mass of water formed is 36.04g.
To find the mass of water that results from combining hydrogen and oxygen, we need to keep in mind the law of conservation of mass, which states that mass cannot be created or destroyed in a chemical reaction. In this case, we need to determine the mass of water formed from the given masses of hydrogen and oxygen.
The molecular formula for water is H2O. It indicates that water is composed of two hydrogen atoms (H) and one oxygen atom (O). The molar mass of hydrogen (H) is approximately 1.008 g/mol, and the molar mass of oxygen (O) is approximately 16.00 g/mol.
First, we need to determine the number of moles of hydrogen and oxygen in the given masses. To do this, we can use the formula:
Number of moles = Mass (g) / Molar mass (g/mol)
Number of moles of hydrogen = 2.0g / 1.008 g/mol = 1.98 mol
Number of moles of oxygen = 16.0g / 16.00 g/mol = 1.00 mol
Next, using the balanced chemical equation for the reaction:
2 H2 + O2 -> 2 H2O
We see that 2 moles of hydrogen combine with 1 mole of oxygen to form 2 moles of water. Since the stoichiometry ratio is 2:1, we can conclude that if we have 1 mole of oxygen, we would need 2 moles of hydrogen to form 2 moles of water.
Since we have 1.98 moles of hydrogen and 1.00 mole of oxygen:
The limiting reactant would be oxygen because it is the reactant that runs out first. Therefore, it determines the maximum amount of product that can be formed.
To calculate the amount of water formed, we can use the ratio obtained from the balanced equation:
1.00 mol of oxygen * (2 mol of water / 1 mol of oxygen) = 2.00 mol of water
Finally, we can find the mass of water formed by multiplying the number of moles of water by its molar mass:
Mass of water = Number of moles * Molar mass
Mass of water = 2.00 mol * 18.02 g/mol = 36.04 g
Therefore, the mass of water that results from combining 2.0g of hydrogen with 16.0g of oxygen is approximately 36.04 grams.