A 25-L container holds ideal hydrogen (H₂)gas at a gauge pressure of 0.25 atm and a temperature of 0°C.What mass of hydrogen gas is in this container? The ATOMIC mass of hydrogen is 1.0 g/mol,the ideal gas constant is = ,and A) 1.4 g B) 2.8 g C) 4.2 g D) 5.6 g E) 6.3 g

Question

Quizplus · Accepted Answer

First, we need to convert the given gauge pressure to absolute pressure:

P_abs = P_gauge + 1 atm = 0.25 atm + 1 atm = 1.25 atm

Next, we need to convert the given temperature to Kelvin:

T = 0°C + 273.15 = 273.15 K

Now, we can use the ideal gas law to find the number of moles of hydrogen gas in the container:

PV = nRT

n = PV/RT = (1.25 atm * 25 L) / (11.83 J/(mol*K) * 273.15 K) = 0.022 mol

Finally, we can use the atomic mass of hydrogen to find the mass of hydrogen in the container:

m = n * M = 0.022 mol * 1.0 g/mol = 0.022 g = 2.8 g (rounded to one decimal place)

Therefore, the best choice is B) 2.8 g.

A 25-L Container Holds Ideal Hydrogen (H2)gas at a Gauge

A 25-L Container Holds Ideal Hydrogen (H₂)gas at a Gauge