Hydrogen and oxygen react to produce water according to the equation below.
2 H2 + O2 2 H2O
How many liters of hydrogen at STP are needed to produce 0.24 mol H2O?
You need t find the arrow key on your computer and use it. ==> or -->. Convert mols H2O to mols H2 using the coefficients in the balanced equation.
0.24 mol H2O x (2 mol H2/2 mol H2O) = 0.24 x 2/2 = 0.24 mols H2 neded.
volume = 0.24 mols H2 x (22.4 L/mol) = ?
To determine the number of liters of hydrogen gas (H2) needed to produce a given amount of water (H2O) at STP (standard temperature and pressure), we need to use the molar volume of gas at STP.
The molar volume of gas at STP is defined as 22.4 liters/mol.
Let's break down the problem step by step:
1. First, find the stoichiometric ratio between hydrogen gas (H2) and water (H2O) based on the balanced equation:
2 H2 + O2 -> 2 H2O
From the equation, we can see that 2 moles of hydrogen gas (H2) react to produce 2 moles of water (H2O). This means that the stoichiometric ratio of H2 to H2O is 2:2, or simply 1:1.
2. Next, determine the number of moles of hydrogen gas (H2) needed to produce 0.24 moles of water (H2O). Since the stoichiometric ratio is 1:1, the number of moles of H2 needed will be the same as the number of moles of H2O:
Number of moles of H2 = Number of moles of H2O = 0.24 mol
3. Finally, use the molar volume of gas at STP to convert the moles of hydrogen gas (H2) into liters:
Number of liters of H2 = number of moles x molar volume
Number of liters of H2 = 0.24 mol x 22.4 liters/mol
Calculating the result:
Number of liters of H2 = 5.376 liters
Therefore, 5.376 liters of hydrogen gas (H2) at STP are needed to produce 0.24 moles of water (H2O).