Question

a gas sample containing 0.2820 moles of a compund is trapped in a 2.461 liter vessel at a temperature of 25.2 celsius. What is the pressure of the vessel if it behaves as an ideal gas?

Answer 1

To find the pressure of the vessel, we can use the ideal gas law equation. Plugging in the given values, we can find the pressure to be 2.3527 atm.

Step-by-step explanation:

To find the pressure of the vessel, we can use the ideal gas law equation:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

In this case, we are given the number of moles (0.2820 moles), the volume (2.461 liters), and the temperature (25.2 Celsius).

We need to convert the temperature to Kelvin by adding 273.15 to get 298.35 K.

Plugging in the values into the ideal gas law equation:

P * 2.461 = 0.2820 * 0.0821 * 298.35

Solving for P:

P = (0.2820 * 0.0821 * 298.35) / 2.461

P = 2.3527 atm