How many moles of chlorine, Cl₂, gas is present if this gas is contained in a 9.22 L vessel at 1124 torr and 24 ° C?

Question

Quizplus · Accepted Answer

We can use the Ideal Gas Law to solve for the number of moles of chlorine gas: PV = nRT where P is the pressure (in atm), V is the volume (in L), n is the number of moles, R is the gas constant (0.08206 L·atm/mol·K), and T is the temperature (in K). We need to convert the given pressure to atm and the given temperature to K: 1124 torr = 1.47 atm 24 °C = 297 K Now we can plug in these values and solve for n: n = PV/RT n = (1.47 atm)(9.22 L)/(0.08206 L·atm/mol·K)(297 K) n = 0.559 mol Therefore, the answer is choice B: 0.559 moles Cl₂.

How Many Moles of Chlorine, Cl2, Gas Is Present If

How Many Moles of Chlorine, Cl₂, Gas Is Present If