Answer :
To determine the mass of hydrogen required to react with 6.00 × 10^25 molecules of oxygen, we can use the balanced chemical equation and the concept of stoichiometry.
From the balanced equation:
2H2(g) + O2(g) → 2H2O(l)
We can see that for every 2 moles of H2, we need 1 mole of O2. This implies that the ratio of H2 to O2 is 2:1 in terms of moles.
Given that there are 6.00 × 10^25 molecules of oxygen, we can calculate the number of moles of oxygen:
Number of moles of O2 = (Number of molecules of O2) / Avogadro's number
= 6.00 × 10^25 / 6.02 × 10^23
≈ 9.97 moles of O2
According to the stoichiometry of the reaction, we know that 2 moles of H2 react with 1 mole of O2. Therefore, the number of moles of H2 required is half of the number of moles of O2:
Number of moles of H2 = 1/2 × Number of moles of O2
= 1/2 × 9.97
≈ 4.99 moles of H2
Finally, we can calculate the mass of hydrogen using its molar mass:
Mass of H2 = Number of moles of H2 × Molar mass of H2
= 4.99 × 2.016
≈ 10.07 grams of H2 (rounded to two decimal places)
Therefore, approximately 10.07 grams of hydrogen will be required to react with 6.00 × 10^25 molecules of oxygen.
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