In an experiment, hydrogen sulfide gas is collected in a 1.25 L flask at 21.0 $\degree$C and 758 torr.How many grams of H₂S (34.08 g/mol) are obtained?

Question

Quizplus · Accepted Answer

First, convert the given conditions to standard units: temperature to Kelvin (T = 273 + 21 = 294 K) and pressure to atm (P = 758 torr * (1 atm / 760 torr) = 0.997 atm). Use the ideal gas law PV = nRT, where P = pressure in atm, V = volume in L, n = number of moles, R = ideal gas constant (0.0821 L·atm/(mol·K)), and T = temperature in Kelvin. Solve for n (moles of H2S): n = PV / RT = (0.997 atm * 1.25 L) / (0.0821 L·atm/(mol·K) * 294 K) = 0.0517 moles. Then, convert moles to grams: mass = n * molar mass = 0.0517 moles * 34.08 g/mol = 1.76 g.

In an Experiment, Hydrogen Sulfide Gas Is Collected in a 1.25