A learner investigates the relationship between the pressure and volume of an enclosed DIATOMIC gas at 25 °C. He records the volume of the gas for different pressures in the table below.

Question

Use the conditions at a pressure of 80 kPa and the number of moles of the enclosed gas is Answer 1 Question 4 x 10-4 mol
A learner investigates the relationship between the pressure and volume of an enclosed DIATOMIC gas at 25 °C.

Answer 1

He records the volume of the gas for different pressures in the table below:

| Pressure (kPa) | Volume (mL) |
|----------------|-------------|
| 50 | 100 |
| 80 | 75 |
| 100 | 60 |
| 120 | 50 |

Using the conditions at a pressure of 80 kPa and the number of moles of the enclosed gas is 4 x 10^-4 mol, we can calculate the volume of the gas at this pressure using the ideal gas law formula:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature

First, we need to convert the pressure from kPa to atm (1 atm = 101.3 kPa):

P = 80 kPa / 101.3 kPa/atm = 0.79 atm

Next, we can rearrange the formula to solve for V:

V = nRT / P

Plugging in the values:

V = (4 x 10^-4 mol) x (0.0821 L atm/mol K) x (25°C + 273) / 0.79 atm
V = (0.00004) x (0.0821) x (298) / 0.79
V = 0.00816 L = 8.16 mL

Therefore, the volume of the gas at a pressure of 80 kPa and 25°C with a number of moles of 4 x 10^-4 mol is 8.16 mL.