Gases are sold in large cylinders for laboratory use. What pressure, in atmospheres, will be exerted by 2,500 g of oxygen gas (O₂)when stored at 22°C in a 40.0 L cylinder? A)3.55 atm B)1,510 atm C)47.3 atm D)7.56 * 10⁴ atm E)10.2 atm

Question

Quizplus · Accepted Answer

We can use the Ideal Gas Law to solve this problem:

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 the temperature in Kelvin.

First, we need to find the number of moles of oxygen gas:

n = m/M

where m is the mass of oxygen gas (2500 g) and M is the molar mass of oxygen (32.00 g/mol).

n = 2500 g / 32.00 g/mol = 78.125 mol

Next, we can rearrange the Ideal Gas Law to solve for pressure:

P = nRT/V

P = (78.125 mol)(0.08206 L∙atm/(mol∙K))(295 K)/(40.0 L)

P = 47.3 atm

Therefore, the pressure exerted by 2,500 g of oxygen gas in a 40.0 L cylinder at 22°C is 47.3 atm, which corresponds to choice C.

Gases Are Sold in Large Cylinders for Laboratory Use