if 10 mol of hydrogen reacted with oxygen, what volume of liquid water could be produced?
2H2 + O2 ==> 2H2O
Assuming the 10 moles H2 had all the oxygen needed to react completely, then 10 moles H2 x (2 moles H2O/2 moles H2) = 10 moles H2 x 2/2 = 10 x 1/1 = 10 moles H2O? 10 moles x 18.015 g/mol = 180.15 grams. If we use the density of water as 1.00 g/mL, then 180.15 g H2O = ?? mL.Check me out on that.
I am not sure I need help. thanks.
To determine the volume of liquid water that could be produced when 10 moles of hydrogen react with oxygen, you need to use the balanced chemical equation for the reaction between hydrogen and oxygen to form water.
The balanced chemical equation for the reaction is:
2H₂ + O₂ → 2H₂O
From this equation, you can see that for every 2 moles of hydrogen (H₂) reacted, 2 moles of water (H₂O) are produced.
Since we have 10 moles of hydrogen, we can use this ratio to find the moles of water produced:
10 moles H₂ * (2 moles H₂O / 2 moles H₂) = 10 moles H₂O
Thus, the reaction will produce 10 moles of water (H₂O).
To calculate the volume of water produced, we need to consider the molar volume of water at standard temperature and pressure (STP), which is 22.4 liters/mol.
The volume (V) of a certain number of moles (n) of a gas or liquid can be calculated using the formula:
V = n * Molar Volume
Using this formula, we can calculate the volume of water produced:
V = 10 moles H₂O * 22.4 liters/mol = 224 liters
Therefore, if 10 moles of hydrogen react with oxygen, the volume of liquid water produced would be 224 liters.