It is calculated that 0.0191 moles of CO2 are expected from a reaction at 25 degrees C and 1 atm. What volume of CO2 does this represent in cm3? (R = 0.0821 L atm / K / mol)
Use PV = nRT.
P is in atm. T in kelvin
To find the volume of CO2 in cm3, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = moles of gas
R = ideal gas constant (0.0821 L atm / K / mol)
T = temperature (in Kelvin)
First, let's convert the given temperature from degrees Celsius to Kelvin:
T(Kelvin) = T(Celsius) + 273.15
T(Kelvin) = 25 + 273.15
T(Kelvin) = 298.15 K
Now we have all the values we need to solve for volume. Rearranging the equation, we get:
V = (nRT) / P
Substituting the given values:
n = 0.0191 moles
R = 0.0821 L atm / K / mol
T = 298.15 K
P = 1 atm
V = (0.0191 mol * 0.0821 L atm / K / mol * 298.15 K) / 1 atm
V = 0.481 L
Finally, we need to convert liters to cm3. Since 1 L = 1000 cm3, we can multiply the volume in liters by 1000:
V(cm3) = V(L) * 1000
V(cm3) = 0.481 L * 1000
V(cm3) = 481 cm3
Therefore, 0.0191 moles of CO2 represents a volume of 481 cm3.
To calculate the volume of CO2 in cm3, we need to use the ideal gas law equation, which is:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L atm / K / mol)
T = temperature (in Kelvin)
First, we need to convert the given temperature from 25 degrees Celsius to Kelvin. To convert from Celsius to Kelvin, we add 273.15 to the Celsius temperature:
T = 25 + 273.15
T = 298.15 K
Now, we can substitute the given values into the ideal gas law equation:
PV = nRT
Let's rearrange the equation to solve for V:
V = (nRT) / P
Substituting the values:
V = (0.0191 moles * 0.0821 L atm / K / mol * 298.15 K) / 1 atm
V = 0.0191 * 0.0821 * 298.15 cm3
V ≈ 0.472 cm3
Therefore, the volume of CO2 that represents 0.0191 moles at 25 degrees Celsius and 1 atm is approximately 0.472 cm3.