Final answer:
To find the volume of H2 gas using the ideal gas law, you need to calculate the number of moles from the mass, convert temperature to kelvins, pressure to atmospheres, and then solve for volume. The calculation of 15.7399 liters does not match the provided answer choices, indicating a possible error.
Step-by-step explanation:
The question relates to finding the volume of H2 gas at a certain temperature and pressure, given its mass. To solve this problem, we will use the ideal gas law equation 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 kelvins.
- First, calculate the number of moles (n) of H2 using its molar mass (approximately 2.02 g/mol):
n = mass / molar mass = 13.4 g / 2.02 g/mol = 6.6337 moles. - Convert the temperature from degrees Celsius to kelvins: T(K) = 25.5 °C + 273.15 = 298.65 K.
- Convert the pressure from torr to atmospheres, because the ideal gas constant R is typically given in L·atm/(mol·K). 1 atm = 760 torr, so P(atm) = 830 torr / 760 torr/atm = 1.0921 atm.
- Use the ideal gas law to calculate the volume (V) of the gas: V = nRT / P = (6.6337 mol)(0.0821 L·atm/(mol·K))(298.65 K) / 1.0921 atm = 15.7399 liters.
However, none of the provided answer choices match this calculated volume, so there may be a mistake in the calculation or the question's values. Please double-check the values provided in the question and the calculation.