Final answer:
The warning on the ether can is due to its flammability and potential to explode if stored above 120 °F. Using the ideal gas law, one can calculate how the pressure inside an ether can increases with temperature. Additionally, the vapor pressure of ether and the effects of altitude on boiling point are explained.
Step-by-step explanation:
Answers to Physics Problems
For the warning on the can: Ether is highly flammable and its vapor pressure increases with temperature, leading to a risk of explosion if stored above certain temperatures or incinerated. The higher the temperature, the more the molecules inside the can move, increasing the internal pressure. Therefore, it is vital to store ether below 120 °F to prevent the can from rupturing or exploding.
To calculate the new pressure in the can on a hot day: We can use the ideal gas law, which states that P1/T1 = P2/T2, where P is the pressure, T is the temperature, and the subscripts 1 and 2 represent initial and final states, respectively. Given the initial conditions (P1 = 360 kPa and T1 = 297 K), and the final temperature (T2 = 323 K), we can solve for P2. Plugging in the values, P2 = (P1 × T2) / T1 = (360 kPa × 323 K) / 297 K, which yields the new pressure.
For the syringe filled with liquid ether at 20 °C: When temperature is constant and the plunger is withdrawn, the pressure of the produced vapor would be close to the vapor pressure of ether at that temperature. Since the temperature does not change and the volume of the vapor inhabitable space increases, initially, the created vapor pressure will equilibrate with the liquid ether's vapor pressure at 20 °C.
Why cooking an egg takes longer at higher altitudes: At higher altitudes, such as in Ft. Davis, Texas, the atmospheric pressure is lower. This causes water to boil at a lower temperature, reducing the heat available for cooking, thereby increasing the time it takes to cook an egg compared to at sea level.