If air is 20% oxygen, and the reaction is
2C2H2 + 5O2 --> 4CO2 + 2H2O,
What volume of oxygen would be needed to completely burn 1.00 L of acetylene (C2H2)?
I got 2.50 L but I'm not sure it's right.
What volume of air would be needed to completely burn 1.00 L of acetylene gas?
I got 3.00 L.
What volume of air would be needed to burn 1.00 L of vaporized octane?
The reaction is:
2C8H18 + 25O2 --> 16CO2 + 18H2O
I got 15.0 L.
2.5L is right for a.
I don't agree with 3.00 L for b. What you want is ?Lair x 0.2 oxygen = 2.5 L oxygen.
?Lair = 2.5 Loxygen/0.2 oxygen = ? which I think is 12.5 L air. Check it.
12.5 L air x 0.2 oxygen = 2.5 L oxygen.
Do c the same way.
I'm not exactly sure how you do the first step.
Are you using the 2.5 L from a?
So would the answer to c be 62.5 L?
? L O2 = 1.00 L x 1 mol/22.4 L x 25 mol O2/2 mol C8H18 x 22.4 L/1 mol O2
= 12.5 L O2
?L air = 12.5 L (5)
=62.5 L air
okay thank you!
12.5 is correct
To determine the volume of oxygen needed to completely burn 1.00 L of acetylene (C2H2), you need to use the stoichiometry of the balanced chemical equation. Let's break down the steps to solve the problem:
Step 1: Write out the balanced chemical equation.
2C2H2 + 5O2 --> 4CO2 + 2H2O
Step 2: Determine the stoichiometric ratio between acetylene (C2H2) and oxygen (O2) in the equation.
From the balanced chemical equation, you can see that it takes 5 moles of oxygen to react with 2 moles of acetylene.
Step 3: Convert the volume of acetylene gas (1.00 L) to moles.
To do this, you will need to know the density of acetylene gas at the given conditions.
Step 4: Use the stoichiometric ratio to find the number of moles of oxygen needed.
Since the stoichiometric ratio is 2 moles of acetylene to 5 moles of oxygen, you can set up a ratio and solve for the number of moles of oxygen.
Step 5: Convert the number of moles of oxygen to volume.
Using the ideal gas law (PV = nRT), you can calculate the volume of oxygen needed. Since the pressure, temperature, and moles of gas are all constant, you can rearrange the equation to solve for volume.
Based on the given information, it is not possible to accurately determine the volume of oxygen needed or the volume of air needed to burn 1.00 L of acetylene gas or vaporized octane without additional information such as the density of the gases or the pressure and temperature conditions.