Final answer:
The question asks for the pressure of 0.555 mol of nitrous oxide (N₂O) at 28 degrees Celsius in a 7.0 L container, which can be found using the ideal gas law.
Step-by-step explanation:
The question involves determining the pressure of a fixed amount of gas contained in a given volume at a certain temperature. This is a classic application of the ideal gas law, which is represented by the equation PV = nRT, where P stands for pressure, V for volume, n for number of moles, R for the ideal gas constant, and T for temperature in Kelvins.
To solve for the pressure (P) of 0.555 mol of N₂O at 28 degrees Celsius in a 7.0 L container, we will convert the temperature to Kelvins by adding 273.15 to the Celsius temperature (28 + 273.15 = 301.15 K) and then use the ideal gas constant (R) value of 0.0821 L⋅atm⋅mol⁻¹⋅K⁻¹. The calculation is as follows:
P = (nRT)/V = (0.555 mol × 0.0821 L⋅atm⋅mol⁻¹⋅K⁻¹ × 301.15 K) / (7.0 L)
When we calculate this, we find the answer for the pressure of the nitrous oxide in the container.