Question

A 2.88g sample of C4H10 (molar mass = 58 g/mol) is contained in a rigid 2.23 L container at 0 °C. Determine the pressure inside of

the container.

Answer 1

The pressure inside the container is calculated using the ideal gas law, resulting in a pressure of 0.525 atmospheres.

Step-by-step explanation:

To determine the pressure inside the container, we can use the ideal gas law: PV=nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the ideal gas constant, and T is temperature in kelvins. First, we'll convert the mass of C4H10 to moles by dividing it by its molar mass (M=58 g/mol), and then convert the temperature from degrees Celsius to kelvins by adding 273 to it. Thus, T = 0 + 273 = 273 K. Next, we use the ideal gas constant R = 0.08206 (L•atm)/(K•mol).

Therefore, n = 2.88g / 58 g/mol = 0.0496 mol. Now, applying the ideal gas law,

P = (nRT)/V

P = (0.0496 mol * 0.08206 L•atm/K•mol * 273 K) / 2.23 L

P = 0.525 atm

The pressure inside the container is 0.525 atmospheres.