what temperature must be maintained in insure that a 1.00 L flask containing 0.04 moles of oxygen will show a continuous pressure of 745 mm Hg?
To determine the temperature required to maintain a specific pressure in a gas sample, we can use the Ideal Gas Law equation: PV = nRT.
Where:
P = Pressure of the gas (in this case, 745 mm Hg)
V = Volume of the gas (1.00 L)
n = Number of moles of the gas (0.04 moles)
R = Ideal Gas Constant (0.0821 L·atm/(mol·K))
T = Temperature of the gas (in Kelvin)
First, let's convert the pressure from mm Hg to atm.
1 atm = 760 mm Hg
745 mm Hg * (1 atm / 760 mm Hg) = 0.9789 atm (approximately)
Now, we can rearrange the equation to solve for T:
T = (PV) / (nR)
T = (0.9789 atm * 1.00 L) / (0.04 moles * 0.0821 L·atm/(mol·K))
Calculating:
T = 29.93 Kelvin
Therefore, the temperature that must be maintained is approximately 29.93 Kelvin.