A 1.00-g sample of a gaseous compound of boron and hydrogen occupies 0.820 L at 1.00 atm and 3 $\degree$C. What is the molecular formula for the compound?

Question

Quizplus · Accepted Answer

Using the ideal gas law, PV = nRT, we can calculate the molar mass of the compound. Given P = 1.00 atm, V = 0.820 L, T = 273 + 31 = 304 K, and R = 0.0821 L·atm/mol·K, we find n = PV/RT = (1.00 * 0.820) / (0.0821 * 304) = 0.0328 mol. The molar mass is 1.00 g / 0.0328 mol = 30.5 g/mol, which corresponds to B₂H₆.

A 100-G Sample of a Gaseous Compound of Boron and Hydrogen