Question

How many moles of chlorine gas at 120.0 °C and 33.3 ATM would occupy a vessel of 25.5 L?​

Answer 1

PV = nRT

P = 33.3 atm

V = 25.5 L

n = ? mol

R = 0.08206 L•atm/K•mol

T = 120.0 °C + 273.15 = 393.15 K

Solve for moles:

n = PV/RT

n = (33.3 atm × 25.5 L)/(0.08206 L•atm/K•mol × 393.15 K)

= 26.3 mol Cl₂

Answer 2

Temperature (T) = 120°C

= (120+273) K

= 393 K

Pressure (P) = 33.3 atm

Volume (V) = 25.5 L

Gas Constant (R) = PV/T

= (1*22.4)/273

= 0.082 atm.L/K.mol

Law= PV = nRT

= (33.3*25.5)

= (n*0.082*393)

= 849.15

= 32.226n

= 26.349n

= 26.3 mol Cl₂

therefore, the number of moles are 26.3 mol Cl₂.