Calculating Gas Pressure in a Flask
How do we calculate the pressure of the gas in a flask based on the given data?
A 1.55 g sample of CO2 is contained in a 547 mL flask at 26.0°C. What is the pressure of the gas?
Calculating Gas Pressure in a Flask
To calculate the pressure of the gas in a flask based on the given data, we can use the ideal gas law equation. The formula is:
P = nRT/V
Where:
P = Pressure
n = Number of moles of gas
R = Ideal gas constant
T = Temperature
V = Volume of gas
In this case, the mass of CO2 is 1.55 g, the volume of the flask is 547 mL, and the temperature is 26.0°C. Let's break down the steps to find the pressure of the gas:
Step 1: Calculate the number of moles of CO2
Step 2: Find the gas constant R
Step 3: Convert the temperature to Kelvin
Step 4: Calculate the pressure using the ideal gas law equation
Detailed Explanation:
Step 1: Calculate the number of moles of CO2. The molar mass of CO2 is 44.01 g/mol. So, the number of moles of CO2 present in the sample is 0.03525 mol.
Step 2: Find the gas constant R. The value of the gas constant R is 0.0821 L·atm/mol·K.
Step 3: Convert the temperature from Celsius to Kelvin. The temperature of 26.0°C is equivalent to 299.15 K.
Step 4: Calculate the pressure using the ideal gas law equation. By substituting the values into the formula, we find that the pressure of the gas in the flask is 2.20 atm.
Therefore, the pressure of the gas in the flask containing the CO2 sample is 2.20 atm. This calculation was done using the ideal gas law equation by determining the number of moles of CO2, finding the gas constant, converting the temperature to Kelvin, and finally solving for pressure.