To find the pressure of the CO2 gas in the cylinder, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume (in liters)
n = number of moles
R = ideal gas constant
T = temperature (in Kelvin)
First, we need to calculate the number of moles of CO2 in the cylinder using the given mass and molar mass of CO2:
Molar mass of CO2 = 12.01 g/mol (C) + 2(16.00 g/mol) = 44.01 g/mol
Number of moles = mass / molar mass
Number of moles = 36.4 g / 44.01 g/mol = 0.827 moles
Next, we can rearrange the ideal gas law equation to solve for pressure:
P = nRT / V
P = (0.827 moles)(0.0821 L·atm/mol·K)(495 K) / 30.0 L
P = 12.8114 atm
Finally, we need to convert the pressure from atm to mmHg by using the conversion factor:
1 atm = 760 mmHg
P = 12.8114 atm * 760 mmHg/atm = 9745.024 mmHg
Therefore, the pressure of the CO2 gas in the cylinder is 9750 mmHg (4 significant figures).
If a cylinder contains 36.4 g of CO2 in 30.0 L at 495. K, what is the pressure (in mmHg)? Be sure your answer has the correct number of significant figures.
Note: Reference the Fundamental constants and Conversion factors for non-SI units tables for additional information.
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