Given the half-cell reaction, \(2 Br \rightarrow Br _{2}\), how many moles of electron will be required to produce \(0.56 dm ^{3}\) of bromine at s.t.p.? [molar volume of gas at s.t.p. \(=22.4 dm ^{3}\) ].
A. \(0.05\) B. \(0.10\) C. \(0.20\) D. \(1.00\)
Correct Answer: A
Explanation
\(2 Br -\rightarrow Br _{2}+2 e ^{-}\) \(22.4 dm ^{3}\) of bromine is produced using two moles of electrons. To produce \(0.56 dm ^{3}\), mole of electron required is \(\left(\frac{2}{22.4} \times 0.56\right)=0.05\)