help please. I don't understand

Question

Sodium metal and chlorine gas can be produced industrially by passing an electric current through molten sodium chloride:

2 NaCl(l) ⟶ 2 Na(l) + Cl₂(g)

What volume of Cl at 293 K (20.°C) and 1.00 atm can be obtained from 68.0 g NaCl using this reaction?

(M_NaCl = 58.44 g/mol; R = 0.0821 L·atm/[K·mol])

V = 

 

Answer 1

The question should ask "what volume of Cl₂ gas can be produced", not what volume of Cl.

2NaCl(l) ==> 2Na(l) + Cl₂(g)

moles NaCl present = 68.0 g x 1 mol/58.44 g = 1.164 moles NaCl

moles of Cl₂ produced = 1.164 mol NaCl x 1 mol Cl₂ / 2 mol NaCl = 0.582 mol Cl₂ produced

To find the volume of Cl₂, we use the ideal gas law ... PV = nRT

P = pressure = 1.00 atm

V = volume = ?

n = moles = 0.582 mol

R = gas constant = 0.0821 Latm/Kmol

T = temperature in K = 293K

Solving for V we have V = nRT/P

V = (0.582)(0.0821)(293)/1.00

V = 14.0 L (3 sig. figs.)