Final answer:
The volume of 454 grams of hydrogen gas at 1.05 atm and 25 degrees Celsius is approximately 5,022.68 liters, calculated by first converting the mass to moles and then using the ideal gas law.
Step-by-step explanation:
The question asks what volume 454 grams of hydrogen gas will occupy at 1.05 atm and 25 degrees Celsius. To solve this, we need to use the ideal gas law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. First, we need to convert the mass of hydrogen to moles using the molar mass of hydrogen (approximately 2.02 g/mol).
Here is the calculation:
- Number of moles (n) = mass (g) / molar mass (g/mol) = 454 g / 2.02 g/mol ≈ 224.75 mol
- Convert temperature to Kelvin: T = 25°C + 273.15 = 298.15 K
- Use the ideal gas constant in L·atm/mol·K: R = 0.0821 L·atm/mol·K
- Finally, rearrange the ideal gas law to solve for V (volume): V = nRT / P
- V = (224.75 mol)(0.0821 L·atm/mol·K)(298.15 K) / 1.05 atm
- V ≈ 5,022.68 L
The volume that 454 grams of hydrogen would occupy at 1.05 atm and 25 degrees Celsius is approximately 5,022.68 liters.