Final answer:
The question involves calculating the number of moles of CO₂ in a gas mixture using the ideal gas law and known conditions. By subtracting the known moles of other gases from the total moles obtained using the gas law, the moles of CO₂ can be found.
Step-by-step explanation:
The student is asking about determining the number of moles of carbon dioxide (CO₂) in a gas mixture using the ideal gas law. The ideal gas law is represented as PV=nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we must calculate the total number of moles of the gases we know, which are N₂, O₂, and CH₄. After summing these moles, we convert the temperature to Kelvin by adding 273.15 to the Celsius temperature. We then rearrange the ideal gas equation to solve for the total moles (n) of the gas mixture using the provided volume (V), temperature (T), pressure (P), and the ideal gas constant (R). We subtract the known moles from the total moles to find the number of moles of CO₂.
The ideal gas constant (R) is typically given as 0.0821 L·atm/mol·K when pressure is in atmospheres, volume is in liters, and temperature is in Kelvin.
- Add 273.15 to the Celsius temperature to convert to Kelvin (25°C + 273.15 = 298.15 K).
- Use the ideal gas law to find the total moles in the 9.04 L volume at 1.17 atm and 298.15 K.
- Subtract the sum of the known moles of N₂, O₂, and CH₄ from the total to find the moles of CO₂.
The complete question is: A mixture consisting of 0.120 mol n2, 0.018 mol o2, 0.112 mol ch4, and an unknown amount of co2 occupies a volume of 9.04 l at 25°c and 1.17 atm pressure. how many moles of co2 are there in this sample? is: