Hydrogen and oxygen gas combine explosively to produce water. Write a balanced chemical equation for this process. If 10 mol of hydrogen reacted with oxygen, what volume of liquid water could be produced?
2H2 + O2 ==> 2H2O
10 mol hydrogen, if it has all the oxygen needed, will produce, according to the coefficients in the balanced equation, 10 moles H2O.
A mole of H2O has a mass of 18 g; therefore, it should produce 180 g H2O and if water has a density of 1.00 g/mL, that will be 180 mL H2O.
To write a balanced chemical equation for the combination of hydrogen and oxygen to produce water, we first need to determine the chemical formula for each substance.
The chemical formula for hydrogen gas is H2, meaning it consists of two hydrogen atoms bonded together. The chemical formula for oxygen gas is O2, meaning it consists of two oxygen atoms bonded together.
Now, let's write the balanced chemical equation for the reaction:
2H2 + O2 → 2H2O
This equation indicates that two molecules of hydrogen gas react with one molecule of oxygen gas to produce two molecules of water.
To find the volume of liquid water that could be produced when 10 mol of hydrogen reacts with oxygen, we need to use stoichiometry and the molar ratio between hydrogen and water.
From the balanced chemical equation, we can see that for every 2 moles of hydrogen gas, we obtain 2 moles of water.
Given that we have 10 moles of hydrogen gas, we can calculate the number of moles of water formed:
10 moles of H2 → 10 moles of H2O
Since the molar ratio is 1:1, we know that the number of moles of water formed is also 10.
Now, to determine the volume of water, we need to use the molar volume of water, which is approximately 18 mL/mol at standard temperature and pressure (STP).
Volume of water = Number of moles of water × Molar volume of water
Volume of water = 10 mol × 18 mL/mol
So, the volume of liquid water that could be produced when 10 mol of hydrogen reacts with oxygen is 180 mL.