How many grams of F₂ gas are there in a 5.00 L cylinder at 5.327 bar and 23 °C? A) 19.5 g B) 41.1 g C) 500 g D) 2.96 × 10⁴ g

Question

Quizplus · Accepted Answer

To solve this problem, we can use the ideal gas law equation: 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. We can rearrange this equation to solve for n: n = PV/RT First, we need to convert the given pressure of 5.327 bar to units of atm: 5.327 bar x 1 atm/1.01325 bar = 5.259 atm Next, we need to convert the temperature of 23 °C to units of Kelvin: 23 °C + 273.15 = 296.15 K Now we can plug in the given values and solve for n: n = (5.259 atm x 5.00 L) / (0.08206 L atm/mol K x 296.15 K) n = 0.973 mol Finally, we can convert moles to grams using the molar mass of F₂ gas: molar mass = 157.03 g/mol mass = n x molar mass mass = 0.973 mol x 157.03 g/mol mass = 152.9 g Therefore, there are 152.9 g of F₂ gas in the cylinder. The closest answer choice is B, which is 41.1 g.

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