Hydrogen and oxygen gas combine explosively to produce water. Write a balanced chemical equation for this process. If 10 moles of hydrogen reacted with oxygen, what volume of liquid water could be produced?

2H2 + O2 ==> 2H2O

10 mol H2 x (2 mols H2O/2 mols H2) = 10 mol x 2/2 = ? mols H2O

grams H2O = ? mols H2O x molar mass H2O = ?
Assuming the density of water is 1.0 g/mL, then mL H2O = grams H2O.

To write a balanced chemical equation for the combination of hydrogen and oxygen to produce water, we need to follow a few steps.

Step 1: Write the chemical formulas for hydrogen, oxygen, and water.
Hydrogen: H2
Oxygen: O2
Water: H2O

Step 2: Write the unbalanced chemical equation by combining the reactants and products.
Unbalanced equation: H2 + O2 -> H2O

Step 3: Balance the equation by adjusting the coefficients to have an equal number of atoms on both sides of the equation.
Balanced equation: 2H2 + O2 -> 2H2O

Now, let's move on to the second part of the question, which is determining the volume of liquid water produced when 10 moles of hydrogen react with oxygen.

To calculate the volume of water, we need to apply the concept of the ideal gas law and the molar volume of gases at standard temperature and pressure (STP). The molar volume of a gas at STP is approximately 22.4 liters/mol.

Given:
Number of moles of hydrogen (H2) = 10 moles

According to the balanced chemical equation:
2 moles of hydrogen (H2) produce 2 moles of water (H2O)

Now we can set up a proportion to find the volume of water produced:

(10 moles H2) / (2 moles H2) = V water / (2 moles H2O)

Simplifying the proportion:
10 / 2 = V water / 2

V water = (10 / 2) * 2

V water = 10 liters

Therefore, if 10 moles of hydrogen react with oxygen to produce water, the volume of liquid water produced would be 10 liters.