If 10 g of oxygen gas is in a 2.00 L container at 50°C, what is the pressure in the container? Round to one decimal place.

Question

High School

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Answer :

graciaguimi graciaguimi · Answer 1 · 2024-02-19T09:57:33-05:00

To solve for the pressure, we can use the ideal gas law:

PV = nRT

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

First, we need to convert the mass of oxygen to moles. The molar mass of oxygen is 32 g/mol, so:

n = m/M = 10 g / 32 g/mol = 0.3125 mol

Next, we need to convert the temperature to Kelvin. We can do this by adding 273.15 to the Celsius temperature:

T = 50°C + 273.15 = 323.15 K

Now we can plug in the values we have into the ideal gas law:

PV = nRT

P(2.00 L) = (0.3125 mol)(0.08206 L·atm/mol·K)(323.15 K)

Solving for P, we get:

P = (0.3125 mol)(0.08206 L·atm/mol·K)(323.15 K) / (2.00 L)

P ≈ 4.98 atm

Therefore, the pressure in the container is approximately 4.98 atm, rounded to one decimal place.