Gas Law Problem: Will the Flask Explode When Heated?
Based on the data provided, will the flask explode when heated to 680 °C? What is the final pressure of the nitrogen gas inside the flask?
Initial volume: 500 mL
Room temperature: 20 °C
Initial pressure: 635 mm Hg
Maximum pressure the flask can withstand: 3 atm
Answer
The final pressure of the nitrogen gas when heated to 680 °C is 2.71 atm. The flask will not explode under this heating.
When analyzing this gas law problem, we first need to establish the initial parameters. The initial volume of the nitrogen gas is given as 500 mL, the initial pressure is 635 mm Hg, and the room temperature is 20 °C. The maximum pressure the flask can withstand is 3 atm.
To determine if the flask will explode under heating to 680 °C, we need to calculate the final pressure of the nitrogen gas inside the flask. Using the ideal gas law equation, PV = nRT, we can solve for the final pressure.
Given that the volume remains constant (V1 = V2), we can simplify the equation to P2 = (P1 * T2) / T1. By substituting the given values, we find that the final pressure of the nitrogen gas is 2.71 atm when heated to 680 °C.
Since this final pressure is below the maximum pressure the flask can withstand (3 atm), the flask will not explode under this heating condition. Understanding how temperature affects gas pressure is crucial in evaluating such scenarios and ensuring safety.