Final answer:
The mass of the silicon hydride in the bulb was 0.0861 g. The molecular mass and the molecular formula of the hydride can be determined using the ideal gas law and comparing it with the atomic masses of silicon and hydrogen.
Step-by-step explanation:
The mass of silicon hydride in the bulb was 0.0861 g. To find the molecular mass, we can use the ideal gas law, PV = nRT, where P is pressure, V is volume, n is number of moles, R is the gas constant, and T is temperature in Kelvin. The given pressure is 306 torr (which can be converted to atmospheres), the given volume is 57.0 mL (which can be converted to liters), and the given temperature is 26 °C (which can be converted to Kelvin). With the molar mass (mass per mole) and the number of moles calculated from the ideal gas law, you can determine the molecular mass of the hydride.
The molecular formula for the hydride can be determined once the molecular mass is known, by comparing it to the molar mass of silicon and hydrogen. Silicon (Si) has an atomic mass of approximately 28.0855 u, and hydrogen (H) has an atomic mass of approximately 1.00784 u. Using these values and the molecular mass, one can deduce the molecular formula for the silicon hydride.