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A gas is held at a pressure of 3.2 atm and a temperature of 250 K, occupying a volume of 4.0 L. The gas has a mass of 99.8 g. What is the identity of the gas?

Use [tex]R = 0.0821 \, \text{L}\cdot\text{atm}/\text{K}\cdot\text{mol}[/tex].

Answer :

Final answer:

To identify the gas given pressure, volume, temperature, and mass, we use the ideal gas law to calculate moles and then determine the molar mass, which we can compare to known gases to discover the gas's identity.

Explanation:

To determine the identity of the gas, we will use the ideal gas law, which relates pressure (P), volume (V), temperature (T), and amount of gas (n) in moles, as represented by the equation PV = nRT. Given that the gas constant R is 0.0821 L·atm/K·mol, we can solve for the number of moles of the gas and then find its molar mass to identify the gas.

First, we calculate the number of moles (n) using the ideal gas law equation:
n = PV / (RT) = (3.2 atm × 4.0 L) / (0.0821 L·atm/K·mol × 250 K)

Now, knowing the number of moles and the mass of the gas (99.8 g), we calculate the molar mass of the gas:
Molar Mass (MM) = mass / moles

Once we have the molar mass, we can compare it to the known molar masses of different gases to determine the identity of the gas.

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Rewritten by : Jeany

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