Propane and oxygen react according to the following equation.

C3H8(g) + 5O2>>>3CO2(g) + 4H2O(g)

Calculate the volume of carbon dioxide and water vapour produced and the volume of oxygen
remaining, when 20.0 dm3
of propane reacts with 120.0 dm3
of oxygen. All gas volumes are
measured at the same temperature and preessure

To find the volume of carbon dioxide and water vapor produced, we need to use the stoichiometric coefficients from the balanced equation to determine the mole ratios.

Looking at the equation: C3H8(g) + 5O2(g) -> 3CO2(g) + 4H2O(g)

We can see that for every 1 mole of propane, we will produce 3 moles of carbon dioxide and 4 moles of water vapor.

Here's how we can calculate the volumes:

1. Calculate the moles of propane:
20.0 dm3 propane * (1 mole propane / 22.4 dm3 propane) = 0.893 moles propane

2. Using the mole ratio, calculate the moles of carbon dioxide:
0.893 moles propane * (3 moles CO2 / 1 mole propane) = 2.679 moles CO2

3. Convert moles of carbon dioxide to volume (dm3) using the molar volume at the given temperature and pressure (usually 22.4 dm3 at STP):
2.679 moles CO2 * 22.4 dm3 CO2/mol = 59.9656 dm3 CO2

4. Calculate the moles of water vapor:
0.893 moles propane * (4 moles H2O / 1 mole propane) = 3.572 moles H2O

5. Convert moles of water vapor to volume (dm3) using the molar volume at the given temperature and pressure:
3.572 moles H2O * 22.4 dm3 H2O/mol = 79.9968 dm3 H2O

6. Calculate the moles of oxygen used:
120.0 dm3 oxygen * (1 mole oxygen / 22.4 dm3 oxygen) = 5.357 moles oxygen

7. Using the mole ratio, calculate the moles of oxygen remaining:
5.357 moles oxygen - 5 moles oxygen (used for propane combustion) = 0.357 moles oxygen

8. Convert moles of oxygen remaining to volume (dm3) using the molar volume at the given temperature and pressure:
0.357 moles oxygen * 22.4 dm3 oxygen/mol = 7.9976 dm3 oxygen

Therefore, when 20.0 dm3 of propane reacts with 120.0 dm3 of oxygen, it produces 59.97 dm3 of carbon dioxide, 79.997 dm3 of water vapor, and leaves behind 7.998 dm3 of oxygen.

To calculate the volume of carbon dioxide and water vapor produced, as well as the volume of oxygen remaining, we need to use the stoichiometry of the reaction. The balanced equation tells us the molar ratios between the reactants and products.

From the balanced equation:
1 mol of propane (C3H8) reacts with 5 mol of oxygen (O2) to produce 3 mol of carbon dioxide (CO2) and 4 mol of water (H2O).

Step 1: Convert the volume of propane and oxygen to moles using the ideal gas law equation.
The ideal gas law equation is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.

Given:
Volume of propane (C3H8) = 20.0 dm^3
Volume of oxygen (O2) = 120.0 dm^3

Convert dm^3 to L:
20.0 dm^3 = 20.0 L
120.0 dm^3 = 120.0 L

Convert volume to moles using the ideal gas law:
n = PV / RT

For propane:
PV = nRT
n = (20.0 L) / (0.0821 L·atm/mol·K · T)

For oxygen:
PV = nRT
n = (120.0 L) / (0.0821 L·atm/mol·K · T)

Step 2: Calculate the moles of carbon dioxide (CO2) and water vapor (H2O) produced using the stoichiometric ratios from the balanced equation.

Using the molar ratios from the balanced equation:
1 mol of C3H8 produces 3 mol of CO2, and 1 mol of C3H8 produces 4 mol of H2O.

Let's say x represents the number of moles of C3H8. Therefore, the number of moles of CO2 and H2O produced will be 3x and 4x, respectively.

Step 3: Calculate the volume of CO2 and H2O produced by converting the moles to volume using the ideal gas law.

Volume of CO2 = moles of CO2 * RT / P
Volume of H2O = moles of H2O * RT / P

Step 4: Calculate the remaining volume of oxygen (O2) by subtracting the volume used from the initial volume of oxygen.

Volume of remaining O2 = Initial volume of O2 - Volume of CO2 - Volume of H2O

Finally, we can use these calculations to determine the specific volumes of carbon dioxide, water vapor, and the remaining oxygen when 20.0 dm^3 of propane reacts with 120.0 dm^3 of oxygen.

gas moles and volumes are directly related

you can use dm3 in the given equation