Question

what volume does 2.5 moles of carbon monoxide occupy at 50.5 kPa pressure and 20.0 C?

Answer 1

Use PV = nRT

Answer 2

[AI-generated answer — Explain Bot]

To determine the volume of the gas, we can use the ideal gas law equation: PV = nRT.

Here's how you can solve it step by step:

1. Write down the given values:
- Pressure (P) = 50.5 kPa
- Number of moles (n) = 2.5 mol
- Universal Gas Constant (R) = 8.314 J/(mol·K) (you might need to convert the pressure and temperature units to match this constant)
- Temperature (T) = 20.0 °C = 20.0 + 273.15 K (Convert from Celsius to Kelvin by adding 273.15)

2. Convert the pressure unit from kPa to Pa:
- 50.5 kPa * 1000 Pa/kPa = 50,500 Pa

3. Convert the temperature from Celsius to Kelvin:
- 20.0 °C + 273.15 = 293.15 K

4. Plug the values into the ideal gas law equation:
- PV = nRT
- (50,500 Pa) * V = (2.5 mol) * (8.314 J/(mol·K)) * (293.15 K)

5. Solve for V (volume):
- V = (2.5 mol * 8.314 J/(mol·K) * 293.15 K) / 50,500 Pa

6. Multiply the values inside the parentheses:
- V = 611.1785 J/(K·Pa) / 50,500 Pa

7. Divide the two values to find the volume:
- V ≈ 0.0121 m³ or 12.1 L (rounded to 3 significant figures)

Therefore, 2.5 moles of carbon monoxide occupies approximately 0.0121 cubic meters or 12.1 liters at 50.5 kPa pressure and 20.0 °C temperature.