Hydrogen and oxygen react according to the equation: 2H2 + O2 -> 2H2O.
According to Avogadro's law, how many liters of hydrogen are required to react with 2.0 L of oxygen at STP?
How do you set this equation up and find the answer???
When using volume only with gases, one can ignore going through the conversion to mols and just take the ratio as the volumes in the equation. You read the equation this way. 2 volumes of hydrogen react with 1 volume of oxygen. Therefore, 2.O L of oxygen at STP would react with ?? L of hydrogen at STP
I just wanted to say that DrBob222 made that question so simple to answer! Thank you so much! It is so much better than just telling the answer.
To determine how many liters of hydrogen are required to react with 2.0 L of oxygen at STP (Standard Temperature and Pressure), we can use the stoichiometry of the balanced chemical equation, as well as Avogadro's law.
Step 1: Note the balanced chemical equation: 2H2 + O2 -> 2H2O. This equation tells us that two moles of hydrogen react with one mole of oxygen to produce two moles of water.
Step 2: Convert the given volume of oxygen to moles using Avogadro's law. At STP, 1 mole of any gas occupies 22.4 L. Therefore, 2.0 L of oxygen can be converted to moles as follows:
2.0 L O2 * (1 mole O2 / 22.4 L) = 0.089 moles O2
Step 3: Use the stoichiometry of the balanced chemical equation to determine the mole ratio between oxygen and hydrogen. According to the equation, two moles of hydrogen react with one mole of oxygen. Therefore, we multiply the moles of oxygen by the ratio of hydrogen to oxygen:
0.089 moles O2 * (2 moles H2 / 1 mole O2) = 0.178 moles H2
Step 4: Convert the moles of hydrogen to liters using Avogadro's law. Since 1 mole of any gas occupies 22.4 L at STP, we can convert the moles of hydrogen to liters as follows:
0.178 moles H2 * (22.4 L / 1 mole H2) = 3.99 L H2 (rounded to two decimal places)
Therefore, approximately 3.99 liters of hydrogen are required to react with 2.0 liters of oxygen at STP.
To answer this question, we need to use Avogadro's law, which states that equal volumes of gases, at the same temperature and pressure, contain an equal number of molecules.
The balanced chemical equation given is: 2H2 + O2 -> 2H2O.
From the equation, we can see that for every 2 moles of hydrogen (H2), we need 1 mole of oxygen (O2) to react completely and form 2 moles of water (H2O). This ratio of 2:1:2 represents the molar ratio in the reaction.
Given that we have 2.0 L of oxygen (O2), we need to figure out the number of liters of hydrogen (H2) required. Since the ratio is 2:1, we can set up a proportion to solve for the unknown volume of hydrogen.
Here's how to set up the equation:
2.0 L O2 / 1 = x L H2 / 2
Simplifying this equation, we get:
2.0 L O2 = (x L H2) / 2
Now, cross multiply:
2.0 L O2 × 2 = x L H2
4.0 L O2 = x L H2
Therefore, 4.0 L of hydrogen (H2) are required to react with 2.0 L of oxygen (O2) at STP, according to Avogadro's law.