how many liters of oxygen are required to react completely with 3.6 liters of hydrogen to form water?

how do i do this problem... thanks:)

2H2+3FeO-->3Fe +Al2O3.

You can't make aluminum out of hydrogen.

In answer to your original question, volumes are proportional to moles, when Pressure and Temperature are constant. You need half as many moles of O2 as you do H2, when H2O is being made in the reaction
2 H2 + O2 = 2 H2O
The answer is therefore 1.8 liters.

To solve this problem, you need to use the balanced chemical equation for the reaction between hydrogen and oxygen to form water. The balanced equation is:

2H₂ + O₂ → 2H₂O

From the equation, we can see that 2 moles of hydrogen react with 1 mole of oxygen to form 2 moles of water. We can use this information to find the amount of oxygen needed to react with a given amount of hydrogen.

Step 1: Convert the given volume of hydrogen to moles.
Using the ideal gas law PV = nRT, where P is the pressure (assumed to be constant), V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature (also assumed to be constant), we can calculate the number of moles of hydrogen.
Assuming standard temperature and pressure (STP), where T = 273.15 K and P = 1 atm, the value of R is 0.0821 L·atm/mol·K.
Therefore, the number of moles of hydrogen = V / (R × T)
Given V = 3.6 L,
n(Hydrogen) = (3.6 L) / (0.0821 L·atm/mol·K × 273.15 K)

Step 2: Find the moles of oxygen required.
From the balanced equation, we know that 2 moles of hydrogen react with 1 mole of oxygen. Therefore, the moles of oxygen needed = (n(Hydrogen)) / 2.

Step 3: Convert the moles of oxygen to liters.
Using the relationship 1 mole = 22.4 L (at STP), we can calculate the volume of oxygen needed.
Volume of oxygen = (moles of oxygen) × (22.4 L/mol)

This calculation will give you the required number of liters of oxygen to react completely with 3.6 liters of hydrogen to form water.

To solve this problem, you need to know the balanced chemical equation for the reaction between hydrogen and oxygen to form water. The balanced equation is:

2H2 + O2 → 2H2O

From the balanced equation, you can see that 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water.

Start by converting the volume of hydrogen provided (3.6 liters) to moles. To do this, you need to know the molar volume of hydrogen at the given conditions, such as temperature and pressure. Let's assume standard temperature and pressure conditions where 1 mole of gas occupies 22.4 liters.

3.6 liters of H2 ÷ 22.4 liters/mole = 0.161 moles of H2

Now that you know the number of moles of hydrogen, you can determine the number of moles of oxygen required using the stoichiometry of the reaction. From the balanced equation, you know that 2 moles of H2 react with 1 mole of O2.

0.161 moles of H2 × 1 mole of O2 / 2 moles of H2 = 0.0805 moles of O2

Finally, you can convert the moles of oxygen to liters using the same molar volume of gases (22.4 liters/mole).

0.0805 moles of O2 × 22.4 liters/mole = 1.80 liters of O2

Therefore, to completely react with 3.6 liters of hydrogen to form water, you would need approximately 1.80 liters of oxygen.