2C2H6(g) + 7O2(g) = 4CO2(g) + 6H2O(g) How many L of oxygen gas is needed to produce 18.0 L of CO2

I guess that 22.909 L

Use the coefficients.

18 L CO2 x (7 mols O2/4 mols CO2) = 18 x 7/4 = ?
The answer is NOT 22.909.

To determine how many liters of oxygen gas (O2) is needed to produce 18.0 liters of carbon dioxide (CO2), we can use the balanced chemical equation provided:

2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(g)

From the equation, we can see that 7 moles of oxygen are required to produce 4 moles of carbon dioxide.

Now we can use the relationship between moles and volume. At standard temperature and pressure (STP), which is 0 degrees Celsius and 1 atmosphere pressure, 1 mole of any gas occupies 22.4 liters.

Using this information, we can set up a proportion to find the volume of oxygen gas needed:

(7 moles O2 / 4 moles CO2) = (x liters O2 / 18.0 liters CO2)

Cross multiplying gives:
7 moles O2 * 18.0 liters CO2 = 4 moles CO2 * x liters O2

126 moles O2 = 4 moles CO2 * x liters O2

Dividing both sides by 4 moles CO2 gives:
31.5 moles O2 = x liters O2

Therefore, you would need 31.5 liters of oxygen gas to produce 18.0 liters of carbon dioxide.

To answer this question, we need to use the balanced chemical equation provided. The coefficients in the balanced equation tell us the stoichiometric ratios between the reactants and products.

According to the balanced equation, the stoichiometric ratio between O2 (oxygen gas) and CO2 is 7:4. This means that for every 7 moles of O2, we obtain 4 moles of CO2.

To find the volume of O2 needed, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure (assumed to be constant)
V = volume of the gas
n = number of moles of the gas
R = ideal gas constant
T = temperature (assumed to be constant)

Since we are given the volume of CO2, we need to find the moles of CO2 produced using the given volume (18.0 L).

To do this, we can use the ideal gas law again to calculate the number of moles of CO2:

n = PV/RT

Now, we can set up a proportion using the stoichiometric ratio:

(4 moles CO2 / 7 moles O2) = (n moles CO2 / x moles O2)

Simplifying the proportion will give us the value of x, which represents the number of moles of O2 needed.

Finally, we can use the ideal gas law once more to calculate the volume of O2 needed:

V = (n moles O2) * (RT / P)

Substituting the value of x into the equation will give us the volume of O2 in liters.

Please note that the values for pressure (P) and temperature (T) are assumed to be constant, and the ideal gas constant (R) is a known constant. Make sure to use the appropriate units throughout the calculations.

By following this procedure, you should be able to determine the volume of oxygen gas (O2) needed to produce 18.0 liters of carbon dioxide (CO2) according to the given balanced chemical equation.