If 75.0 grams of water is decomposed into hydrogen and oxygen, how many grams of hydrogen should be formed?
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t4er
To determine how many grams of hydrogen should be formed when 75.0 grams of water is decomposed, we need to consider the chemical equation for the decomposition of water.
The balanced equation for the decomposition of water is:
2H₂O → 2H₂ + O₂
From the equation, we can see that for every 2 moles of water (H₂O), 2 moles of hydrogen (H₂) are formed.
To calculate the number of moles of water, we need to divide the mass of water by its molar mass. The molar mass of water (H₂O) is approximately 18.015 g/mol.
Moles of water = Mass of water / Molar mass of water
= 75.0 g / 18.015 g/mol
≈ 4.16 mol
Since 2 moles of water yields 2 moles of hydrogen, we can expect that 4.16 moles of water will produce 4.16 moles of hydrogen.
To calculate the mass of hydrogen, we multiply the moles of hydrogen by its molar mass. The molar mass of hydrogen (H₂) is approximately 2.016 g/mol.
Mass of hydrogen = Moles of hydrogen × Molar mass of hydrogen
= 4.16 mol × 2.016 g/mol
≈ 8.37 g
Therefore, approximately 8.37 grams of hydrogen should be formed when 75.0 grams of water is decomposed.
To determine the grams of hydrogen formed when 75.0 grams of water is decomposed, we need to consider the chemical formula of water (H2O) and the law of conservation of mass.
The chemical formula of water (H2O) indicates that one molecule of water consists of two hydrogen atoms and one oxygen atom. According to the law of conservation of mass, the total mass of the reactants must be equal to the total mass of the products.
To find the mass of hydrogen formed, we can use the molar mass of water and the molar ratio between hydrogen and water.
First, let's calculate the molar mass of water (H2O):
- The molar mass of hydrogen (H) is approximately 1.008 grams/mole.
- The molar mass of oxygen (O) is approximately 16.00 grams/mole.
Thus, the molar mass of water (H2O) is:
(2 * 1.008 g/mol of H) + (16.00 g/mol of O) = 18.016 g/mol of H2O.
Next, we can use the molar mass of water to calculate the number of moles of water present in 75.0 grams:
75.0 g / (18.016 g/mol of H2O) = 4.16 moles of H2O.
Since the molar ratio between hydrogen and water is 2:1 (2 moles of H per 1 mole of H2O), we multiply the number of moles of water by the molar ratio to obtain the number of moles of hydrogen:
4.16 moles H2O * (2 moles H / 1 mole H2O) = 8.32 moles of H.
Finally, we can convert moles of hydrogen to grams using the molar mass of hydrogen:
8.32 moles H * (1.008 g/mol of H) = 8.39 grams of H.
Therefore, when 75.0 grams of water is decomposed, approximately 8.39 grams of hydrogen should be formed.