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From the following balanced equation,

\[ 2H_2(g) + O_2(g) \rightarrow 2H_2O(g) \]

How many grams of \( H_2O \) can be formed from 5.58 g \( H_2 \)?

Select the correct answer below:

A. 49.9 g
B. 0.624 g
C. 99.8 g
D. 5.54 g

Answer :

From 5.58 g of H2, 49.9 g of H2O can be formed.

To solve this problem, we need to use stoichiometry, which is a method for calculating the quantities of reactants and products in a chemical reaction. The balanced equation tells us that 2 moles of H2 react with 1 mole of O2 to produce 2 moles of H2O. Therefore, the ratio of H2O to H2 is 2:2 or 1:1.

To calculate the grams of H2O produced from 5.58 g of H2, we need to convert the mass of H2 to moles using its molar mass of 2.016 g/mol.

moles of H2 = mass of H2 / molar mass of H2
moles of H2 = 5.58 g / 2.016 g/mol
moles of H2 = 2.77 mol

Since the ratio of H2O to H2 is 1:1, we know that the number of moles of H2O produced is also 2.77 mol. To convert this to grams of H2O, we can use its molar mass of 18.015 g/mol.

mass of H2O = moles of H2O x molar mass of H2O
mass of H2O = 2.77 mol x 18.015 g/mol
mass of H2O = 49.9 g

Therefore, the answer is 49.9 g of H2O can be formed from 5.58 g of H2.

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