Question

What volume, in l, would 10.0 moles of nitrous oxide occupy at 65.1 °c with a pressure of 7.85 atm?

Answer 1

To find the volume occupied by 10.0 moles of nitrous oxide at 65.1 °C and 7.85 atm, convert the temperature to Kelvin and then use the ideal gas law with the values plugged in to calculate the volume.

Step-by-step explanation:

To calculate the volume occupied by 10.0 moles of nitrous oxide at a given temperature and pressure, we use the ideal gas law which is PV = nRT, where P is pressure, V is volume, n is number of moles, R is the ideal gas constant, and T is temperature in Kelvin.

First convert the temperature from Celsius to Kelvin by adding 273.15: T = 65.1 °C + 273.15 = 338.25 K.

Using the ideal gas law:

1. Use the given values: n = 10.0 moles, P = 7.85 atm, T = 338.25 K, and R = 0.08206 L-atm/mol-K.
2. Plug into the equation: V = \( \frac{nRT}{P} \) = \( \frac{10.0 moles \times 0.08206 L-atm/mol-K \times 338.25 K}{7.85 atm} \).
3. Perform the calculation to find V.

The calculated volume will give you the volume in liters that the 10.0 moles of nitrous oxide will occupy.