What is the pressure of a 1.0 L flask containing
Of He at 25°C? (R= 0.0821 L atm/ mol K)

Question

What is the pressure of a 1.0 L flask containing 
Of He at 25°C? (R= 0.0821 L atm/ mol K)

Quizplus · Accepted Answer

We can use the ideal gas law to solve for pressure:
PV = nRT
where P is pressure, V is volume, n is the number of moles of gas, R is the gas constant, and T is temperature in Kelvin.
First, we need to convert 25°C to Kelvin: 
25°C + 273.15 = 298.15 K
Next, we can calculate the number of moles of He in the flask using the mass given:
n = m/M
where m is the mass and M is the molar mass of He.
m = 11 g
M = 4.003 g/mol (from the periodic table)
n = 11 g / 4.003 g/mol = 2.75 mol
Now we can substitute the values into the ideal gas law and solve for P:
P = nRT/V
P = (2.75 mol)(0.0821 L atm/mol K)(298.15 K)/(1.0 L)
P = 3.69 atm, which rounds to 3.7 atm (answer choice B)

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