Given the following half-cell reaction; 2Cl(aq) → CI2(g) + 2e, how many mole of electrons will be required to produce 1.12dm3 of chlorine gas at s.t.p? (Molar volume of a gas at s.t.p. = 22.4dm 3)

Given the following half-cell reaction; 2Cl_(aq) → CI_2(g) + 2e, how many mole of electrons will be required to produce 1.12dm³ of chlorine gas at s.t.p? (Molar volume of a gas at s.t.p. = 22.4dm ³)

A 1.00
B 0.40
C 0.20
D 0.10
E 0.01

waec 1989 chemistry

The correct answer is D. 0.10

No explanation given

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