An ideal gas composed of a mixture of oxygen and nitrogen is at a pressure of 1.50 atmospheres and a temperature of 25.0°C. What is the molar density?

Question

An ideal gas composed of a mixture of oxygen and nitrogen is at a pressure of 1.50 atmospheres and a temperature of 25.0°C. What is the molar density?

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Solution

To solve this problem, we need to use the ideal gas law equation, which is PV = nRT.

Here, P = pressure = 1.50 atm T = temperature = 25.0°C = 298.15 K (converted from Celsius to Kelvin by adding 273.15) R = ideal gas constant = 0.0821 L·atm/(K·mol) (we use this value because our pressure is given in atm and we want the molar density in mol/L)

We are asked to find the molar density, which is n/V.

Rearranging the ideal gas law equation, we get n/V = P/RT.

Substituting the given values into this equation, we get:

n/V = 1.50 atm / (0.0821 L·atm/(K·mol) * 298.15 K)

After performing the calculation, we find that the molar density of the gas is approximately 0.061 mol/L.

This problem has been solved

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An ideal gas composed of a mixture of oxygen and nitrogen is at a pressure of 1.50 atmospheres and a temperature of 25.0°C. What is the molar density?

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