Answer :
49.9 grams of H[tex]_{2}[/tex]O can be from 5.58 grams of H[tex]_{2}[/tex] from the given balanced dequation. Option A) 49.9 g is the correct answer.
To determine the amount of H[tex]_{2}[/tex]O that can be formed from 5.58 g of H[tex]_{2}[/tex], we need to use the balanced equation and stoichiometry.
From the balanced equation 2H[tex]_{2}[/tex](g) + O[tex]_{2}[/tex](g) → 2H[tex]_{2}[/tex]O(g), we can see that for every 2 moles of H[tex]_{2}[/tex], 2 moles of H[tex]_{2}[/tex]O are produced.
To calculate the number of moles of H[tex]_{2}[/tex] in 5.58 g, we divide the mass by the molar mass of H[tex]_{2}[/tex], which is 2 g/mol. Therefore, 5.58 g H[tex]_{2}[/tex] corresponds to 5.58 g / 2 g/mol = 2.79 mol H[tex]_{2}[/tex].
Since the mole ratio between H[tex]_{2}[/tex] and H[tex]_{2}[/tex]O is 1:1, the number of moles of H[tex]_{2}[/tex]O formed will also be 2.79 mol.
To convert the moles of H[tex]_{2}[/tex]O to grams, we multiply the number of moles by the molar mass of H[tex]_{2}[/tex]O, which is approximately 18 g/mol. Thus, the mass of H[tex]_{2}[/tex]O formed is 2.79 mol × 18 g/mol = 50.22 g.
Therefore, the correct answer is Option A) 49.9 g.
You can learn more about balanced dequation at
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