Final answer:
The pressure inside the gas canister at 500°C is approximately 2.59 bar, calculated using the combined gas law equation P1/T1 = P2/T2, and converting temperatures to Kelvin.
Step-by-step explanation:
The student is asking how to calculate the pressure of H2 gas in a canister when it is heated from 25°C to 500°C, assuming constant volume. This can be determined using the ideal gas law, specifically the combined gas law, which relates pressure, volume, and temperature of a gas.
To find the new pressure at 500°C, we will use the equation P1/T1 = P2/T2, where P1 is the initial pressure and P2 is the final pressure, while T1 and T2 are the initial and final temperatures in Kelvin, respectively. Since the volume and the amount of gas are constant, we can relate the initial and final states of the gas in the canister.
Let's convert the temperatures to Kelvin first. The initial temperature (T1) is 25°C, which is 298.15 K (25 + 273.15), and the final temperature (T2) is 500°C, which is 773.15 K (500 + 273.15). Now, we can plug in the values: P1 = 1 bar, T1 = 298.15 K, T2 = 773.15 K.
The equation becomes 1 bar / 298.15 K = P2 / 773.15 K. Solving for P2 gives P2 = (1 bar / 298.15 K) × 773.15 K, which calculates to approximately 2.59 bar.
Therefore, the pressure inside the canister at 500°C is about 2.59 bar.