2H2O --> 2H2 + O2
if 30 mL of hydrogen in the above reaction, how many milliliters of oxygen are produced?
Christie, what's your problem? I've answered this question. If you can't find it perhaps I can.
To determine the number of milliliters (mL) of oxygen produced in the given reaction, you need to use the balanced equation, which shows the stoichiometric ratio of the reactants and products.
The balanced equation is: 2H2O --> 2H2 + O2
According to the equation, 2 moles of water (H2O) produce 1 mole of oxygen (O2).
To solve the problem, follow these steps:
Step 1: Convert the given volume of hydrogen (H2) to moles.
Since the equation states that 2 moles of water produce 2 moles of hydrogen, the molar ratio is 2:2. Therefore, the moles of hydrogen are equal to the moles of water.
Given volume of hydrogen (H2) = 30 mL
The molar volume of any gas at standard temperature and pressure (STP) is 22.4 L (or 22.4 x 1000 mL).
30 mL is equivalent to 30/1000 L = 0.03 L.
Now, convert the volume (L) of hydrogen gas to moles using the molar volume:
Moles of hydrogen (H2) = volume (L) / molar volume (L/mol)
= 0.03 L / 22.4 L/mol
≈ 0.001339 mol
Step 2: Calculate the moles of oxygen produced.
The stoichiometric ratio of water to oxygen is 2:1. This means that 2 moles of water produce 1 mole of oxygen.
Since the moles of hydrogen produced are equal to the moles of water, the moles of oxygen produced will be half the moles of hydrogen.
Moles of oxygen (O2) = 0.001339 mol / 2
≈ 0.0006695 mol
Step 3: Convert moles of oxygen to volume (mL).
To convert the moles of oxygen to volume at STP, again use the molar volume of any gas:
Volume (L) of oxygen = moles of oxygen x molar volume (L/mol)
= 0.0006695 mol x 22.4 L/mol
≈ 0.01499 L
Now, convert the volume (L) of oxygen to milliliters (mL):
Volume (mL) of oxygen = 0.01499 L x 1000 mL/L
≈ 14.99 mL
Therefore, approximately 14.99 mL of oxygen are produced in the given reaction.