Using the equation 2H2 + O2 ==> 2H2O, determine how many grams of water is produced when 29 moles of oxygen is consumed
29 moles of O2 --> 58 moles of H2O
So, how many grams is that?
how did u get the H2O moles?
To calculate the number of grams of water produced when 29 moles of oxygen gas (O2) are consumed, we need to use the stoichiometry of the reaction:
2H2 + O2 → 2H2O
From the balanced equation, we can see that for every 1 mole of O2 consumed, 2 moles of H2O are produced.
Step 1: Calculate the moles of water produced
Since the stoichiometric ratio is 2 moles of H2O per 1 mole of O2, we can multiply the number of moles of O2 by the stoichiometric ratio:
29 moles O2 * (2 moles H2O / 1 mole O2) = 58 moles H2O
Step 2: Convert moles of water to grams
To calculate the mass of water, we need to know the molar mass of water (H2O), which consists of 2 hydrogen atoms (H) and 1 oxygen atom (O).
The molar mass of hydrogen (H) is approximately 1.01 g/mol, and the molar mass of oxygen (O) is approximately 16.00 g/mol.
Hence, the molar mass of water (H2O) is:
2 * (molar mass of hydrogen) + 1 * (molar mass of oxygen)
2 * 1.01 g/mol + 16.00 g/mol = 18.02 g/mol
Now, we can convert moles of water to grams using the molar mass:
58 moles H2O * (18.02 g/mol H2O) = 1043.16 grams of water
Therefore, when 29 moles of oxygen are consumed, approximately 1043.16 grams of water are produced.