Step-by-step explanation:
To calculate the partial pressure of CO2 and Ne, as well as the total pressure in the container, we can use the ideal gas law. The ideal gas law equation is given by:
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.
Let's calculate the partial pressure of CO2 and Ne, as well as the total pressure step by step:
1. Convert the given pressure from mmHg to atm: 770 mmHg ÷ 760 mmHg/atm = 1.0132 atm. So, the initial pressure is 1.0132 atm.
2. Convert the given temperature from Celsius to Kelvin: 27°C + 273.15 = 300.15 K. So, the temperature is 300.15 K.
3. Calculate the number of moles of CO2: The mass of CO2 is given as 0.633 g. We need to convert this mass to moles using the molar mass of CO2, which is 44.01 g/mol. Moles = mass / molar mass = 0.633 g / 44.01 g/mol ≈ 0.0144 mol.
4. Calculate the partial pressure of CO2: To find the partial pressure of CO2, we need to use the ideal gas law. Plugging in the values: P CO2 = (n CO2 * R * T) / V = (0.0144 mol * 0.0821 atm/mol K * 300.15 K) / 3.00 L ≈ 0.365 atm.
5. Calculate the partial pressure of Ne: The Ne gas is already present in the container, so we don't need to calculate its moles. The initial pressure of Ne is 1.0132 atm, as given.
6. Calculate the total pressure: To find the total pressure, we need to add the partial pressures of CO2 and Ne. Total Pressure = P CO2 + P Ne = 0.365 atm + 1.0132 atm = 1.3782 atm.
So, the partial pressure of CO2 is approximately 0.365 atm, the partial pressure of Ne is 1.0132 atm, and the total pressure in the container is approximately 1.3782 atm.
(Not really mines)