How many moles of propane are contained in a 5.00 L tank at 450 torr and 25°C?

PV = nRT

To calculate the number of moles of propane, we can use the ideal gas law, which is given by the equation:

PV = nRT

where:
P is the pressure in atm
V is the volume in liters
n is the number of moles
R is the ideal gas constant (0.0821 L·atm/(mol·K))
T is the temperature in Kelvin

First, we need to convert the given values to the appropriate units. The temperature should be in Kelvin, so we add 273.15 to get:
T = 25°C + 273.15 = 298.15 K

Next, we need to convert the pressure from torr to atm:
P = 450 torr / 760 torr/atm ≈ 0.592 atm

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

PV = nRT
(0.592 atm)(5.00 L) = n(0.0821 L·atm/(mol·K))(298.15 K)

Simplifying the equation:
2.960 = n(24.5476)

Now solve for n:
n ≈ 2.960 / 24.5476
n ≈ 0.1202 mol

Therefore, there are approximately 0.1202 moles of propane in the 5.00 L tank.

To determine the number of moles of propane in the 5.00 L tank at 450 torr and 25°C, we can use the ideal gas law. The ideal gas law equation is:

PV = nRT

Where:
P = Pressure of the gas (in atm)
V = Volume of the gas (in liters)
n = Number of moles of the gas
R = Ideal gas constant (0.0821 L·atm/mol·K)
T = Temperature of the gas (in Kelvin)

First, we need to convert the given pressure of 450 torr to atm. Since 1 atm = 760 torr, we can divide 450 torr by 760 torr to get the pressure in atm:

450 torr / 760 torr/atm ≈ 0.5921 atm

Next, we need to convert the given temperature of 25°C to Kelvin. The Kelvin scale is simply Celsius + 273.15. So:

25°C + 273.15 = 298.15 K

Now, we can substitute the given values into the ideal gas law equation:

(0.5921 atm)(5.00 L) = n(0.0821 L·atm/mol·K)(298.15 K)

Simplifying the equation:

2.9605 = n(24.4658)

Dividing both sides by 24.4658:

n ≈ 0.1209 mol

Therefore, there are approximately 0.1209 moles of propane in the 5.00 L tank at 450 torr and 25°C.

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