20.0 L of methane (CH4) undergoes complete

combustion at 0.961 atm and 20◦C. How much
CO2 is formed?
Answer in units of L.

See the problem below.

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To calculate the amount of CO2 formed during the combustion of methane, we need to know the balanced chemical equation for the reaction. The balanced equation for the complete combustion of methane is:

CH4 + 2O2 -> CO2 + 2H2O

From the equation, we can see that for every mole of methane (CH4) consumed, one mole of carbon dioxide (CO2) is produced.

To find the moles of methane, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)

First, let's convert the temperature from Celsius to Kelvin:

T(K) = T(°C) + 273.15
T(K) = 20 + 273.15 = 293.15 K

Next, let's calculate the number of moles of methane using the ideal gas law equation. Rearranging the equation to solve for n:

n = PV / RT

Substituting the given values:

n = (0.961 atm) * (20.0 L) / ((0.0821 L·atm/(mol·K)) * (293.15 K))

Calculating:
n ≈ 0.810 moles of methane

Since the balanced equation shows that one mole of methane produces one mole of carbon dioxide, we can conclude that 0.810 moles of carbon dioxide (CO2) are produced.

To convert moles of CO2 to volume (in L), we can use the ideal gas law equation once again:

V = nRT / P

Substituting the values:

V = (0.810 moles) * (0.0821 L·atm/(mol·K)) * (293.15 K) / (1 atm)

Calculating:
V ≈ 19.4 L of CO2

Therefore, approximately 19.4 L of CO2 are formed during the complete combustion of 20.0 L of methane.