<span title="Electrochemistry....................?">Electrochemistry............</span>

Question

What volume of F2 gas, at 25°C and 1.00 atm, is produced when molten KF is electrolyzed by a current of 13.1 A for 2.45 h?

What mass of potassium metal is produced?

Answer 1

2 F- &gt;&gt;&gt;&gt; F2 + 2e-

13.1 x 8820 s = 115542 Coulombs

115542 / 96500 = 1.20 Faradays

1.20 F( 1 mole F2 / 2 Faradays) = 0.60 mole

V = nRT / p = 0.60 x 0.0821 x 298 K / 1.00 =14.7 L

K+ + 1 e- &gt;&gt; K

1.20 F ( 1 moles K / 1 Faraday) = 1.20 mol

Mass K = 1.20 x 39.1 = 46.9 g