if 25.0g of O2 gas has a temperature of 400k and a pressure of 610 mm Hg, what is its volume?
Use PV = nRT
To find the volume of gas, we can use the ideal gas law equation, which states:
PV = nRT
Where:
P = pressure of the gas
V = volume of the gas
n = number of moles of the gas
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature of the gas in Kelvin
In this case, we know the following values:
P = 610 mm Hg
T = 400 K (Kelvin)
n is unknown, and that's what we need to find it.
R = 0.0821 L·atm/mol·K
To find the number of moles (n), we can use the formula:
n = mass / molar mass
Molar mass of O2 = 32 g/mol (16 g/mol for each oxygen atom)
n = 25.0 g / 32 g/mol
n = 0.78125 mol (approximately)
Now, we have all the values needed to find the volume (V).
PV = nRT
V = (nRT) / P
V = (0.78125 mol * 0.0821 L·atm/mol·K * 400 K) / (610 mm Hg)
Note: We need to convert mm Hg to atm since the ideal gas constant is in atm.
1 atm = 760 mm Hg
V = (0.78125 mol * 0.0821 L·atm/mol·K * 400 K) / (610 mm Hg * (1 atm / 760 mm Hg))
V ≈ 0.831 L (rounded to three decimal places)
So, the volume of the O2 gas is approximately 0.831 L.