How many grams of O_2(g) are needed to react completely with 4.46 g of H_2(g) according to the following balanced chemical equation: 2H_2(g) + O_2(g)--> 2H_2_O(g)
the reaction equation is in moles
convert the H2 into moles
you need half as many O2 moles
convert the O2 into grams
To determine the number of grams of O2 needed to react completely with 4.46 g of H2, we can follow these steps:
Step 1: Determine the molar mass of H2
The molar mass of H2 is the sum of the atomic masses of hydrogen (H) multiplied by the number of hydrogen atoms in one molecule of H2.
Molar mass of H2 = 2 g/mol
Step 2: Convert the mass of H2 to moles
We can use the molar mass of H2 to convert the given mass of H2 to moles.
Number of moles of H2 = mass of H2 / molar mass of H2
Number of moles of H2 = 4.46 g / 2 g/mol
Number of moles of H2 = 2.23 mol
Step 3: Determine the stoichiometric ratio between H2 and O2
From the balanced chemical equation, we can see that the stoichiometric ratio between H2 and O2 is 2:1.
This means that for every 2 moles of H2, 1 mole of O2 is required for complete reaction.
Step 4: Calculate the moles of O2 required
Since we know the number of moles of H2, we can calculate the corresponding number of moles of O2 required.
Number of moles of O2 = (Number of moles of H2) / 2
Number of moles of O2 = 2.23 mol / 2
Number of moles of O2 = 1.115 mol
Step 5: Convert the moles of O2 to grams
Finally, we can use the molar mass of O2 to convert the number of moles to grams.
Molar mass of O2 = 32 g/mol (16 g/mol for each oxygen atom)
Mass of O2 = (Number of moles of O2) * (molar mass of O2)
Mass of O2 = 1.115 mol * 32 g/mol
Mass of O2 = 35.68 g
Therefore, 35.68 grams of O2 are needed to react completely with 4.46 grams of H2.