2.0 x 10^-5 grams of hydrogen gas at 155 degree calsius exert a pressure of 322.5 torr on the walls of a small cylindrical tube. What is the volume of the tube?
To find the volume of the tube, we can use the Ideal Gas Law equation:
PV = nRT
Where:
P = pressure in atmospheres
V = volume in liters
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature in Kelvin
First, let's convert the given pressure from torr to atm:
1 atm = 760 torr
322.5 torr * (1 atm / 760 torr) = 0.424 atm
Next, let's convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
155°C + 273.15 = 428.15 K
Now, we need to calculate the number of moles, n, using the given mass and molar mass of hydrogen gas. The molar mass of hydrogen (H₂) is 2 grams/mol.
n = mass / molar mass
n = 2.0 x 10^-5 g / 2 g/mol = 1.0 x 10^-5 mol
Now, we can rearrange the Ideal Gas Law equation to solve for V:
V = (nRT) / P
V = (1.0 x 10^-5 mol * 0.0821 L·atm/mol·K * 428.15 K) / 0.424 atm
Simplifying the equation:
V = 0.4287 L
Therefore, the volume of the tube is approximately 0.4287 liters.
Use PV = nRT and solve for volume in L.
Remember P must be in atm and T in kelvin. n = grams/molar mass.