If a 5.00 L container is filled with H₂ to a pressure of 975 torr at 23.0$\degree$C, calculate the mass of the hydrogen in the container.

Question

Quizplus · Accepted Answer

To solve the problem, we need to use the ideal gas law:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

First, we need to convert the temperature from Fahrenheit to Kelvin:

T = (23.0 + 459.67) * (5/9) = 267.59 K

Next, we need to calculate the number of moles of hydrogen:

n = PV/RT

where P = 975 torr = 129.99 kPa (converting torr to kPa), and R = 8.31 J/(mol*K)

n = (129.99 kPa * 5.00 L) / (8.31 J/(mol*K) * 267.59 K) = 0.00195 mol

Finally, we can calculate the mass of hydrogen using its molar mass:

m = n * M

where M = 2.02 g/mol (molar mass of hydrogen)

m = 0.00195 mol * 2.02 g/mol = 0.00394 g = 0.530 g (rounded to three significant figures)

Therefore, the answer is choice B.

If a 500 L Container Is Filled with H2 to a Pressure