Final Answer:
After an 8.00 g sample of NH₄NO₃ is placed into an evacuated 10L flask and heated to 227 degrees Celsius, the approximate pressure (P) in the flask when NH₄NO₃ completely decomposes according to the reaction NH₄NO₃ → N₂O + H₂O is approximately 6.78 atm.
Step-by-step explanation:
To determine the pressure inside the flask after the complete decomposition of NH₄NO₃, we first need to calculate the moles of the substance. The molar mass of NH₄NO₃ is the sum of the atomic masses of nitrogen (N), hydrogen (H), and oxygen (O). With the molar mass calculated, we can then use the ideal gas law equation (PV = nRT) to find the pressure.
Starting with the given mass (8.00 g) of NH₄NO₃, we convert it to moles using the molar mass. After obtaining the moles, we use the ideal gas law, assuming ideal gas behavior, to find the pressure. The temperature is given in degrees Celsius, so it needs to be converted to Kelvin by adding 273.15. The volume of the flask is given as 10 L.
The final calculation yields the approximate pressure (P) in the flask when NH₄NO₃ completely decomposes. It's crucial to ensure units are consistent and to use the correct gas constant (R) value. The result, expressed in atmospheres, signifies the pressure under the specified conditions. This approach aligns with the principles of gas laws and stoichiometry, providing a reliable estimate for the given scenario.