What is the total pressure, in atmospheres, of a 10.0 L container that contains 10 moles of nitrogen gas and 10 moles of oxygen gas at 300 K?

I tried using PV=nRT and added both P together but kept getting the wrong answer.
n=10, T=300 K, V=1x10^-3 m^3

To find the total pressure of the gas mixture in the 10.0 L container, you need to use the ideal gas law equation, PV = nRT. However, before you can calculate the total pressure, you need to combine the nitrogen and oxygen gases into a single equation.

First, let's find the partial pressure of each gas using the ideal gas law:

For nitrogen gas (N₂):
n = 10 moles
V = 10.0 L
T = 300 K
R = 0.0821 L·atm/(mol·K)

P(N₂) = nRT/V
P(N₂) = (10 mol)(0.0821 L·atm/(mol·K))(300 K) / (10.0 L)
P(N₂) = 24.63 atm

Similarly, for oxygen gas (O₂):
n = 10 moles
V = 10.0 L
T = 300 K
R = 0.0821 L·atm/(mol·K)

P(O₂) = nRT/V
P(O₂) = (10 mol)(0.0821 L·atm/(mol·K))(300 K) / (10.0 L)
P(O₂) = 24.63 atm

Now, to find the total pressure, you can simply add the partial pressures of nitrogen and oxygen:

Total Pressure = P(N₂) + P(O₂)
Total Pressure = 24.63 atm + 24.63 atm
Total Pressure = 49.26 atm

Therefore, the total pressure of the gas mixture in the 10.0 L container is 49.26 atmospheres.

To find the total pressure of the container, you need to calculate the partial pressures of nitrogen gas and oxygen gas and then add them together.

First, let's calculate the partial pressure of nitrogen gas. We know that the number of moles of nitrogen gas (n) is 10 and the volume of the container (V) is 10.0 L. However, the ideal gas law equation (PV = nRT) you used requires the volume to be in cubic meters (m^3). So, we need to convert the volume from liters (L) to cubic meters (m^3).

1 L = 0.001 m^3 (conversion factor)

Therefore, V = 10.0 L x 0.001 m^3/L = 0.01 m^3

Now, we can use the ideal gas law equation to calculate the partial pressure of nitrogen gas:

PV = nRT

P(nitrogen) x V = n(nitrogen) x R x T

P(nitrogen) = (n(nitrogen) x R x T) / V

n(nitrogen) = 10 moles
R = 0.0821 L.atm/(mol.K) (universal gas constant)
T = 300 K

P(nitrogen) = (10 moles x 0.0821 L.atm/(mol.K) x 300 K) / 0.01 m^3

Now, let's calculate the partial pressure of oxygen gas using the same process:

n(oxygen) = 10 moles

P(oxygen) = (10 moles x 0.0821 L.atm/(mol.K) x 300 K) / 0.01 m^3

Finally, you can add the partial pressures of nitrogen gas and oxygen gas to find the total pressure in atmospheres:

Total pressure = P(nitrogen) + P(oxygen)

A.24.6L

B.49.3L
C.2460L
D.4930L