Chlorine gas (Cl2) can be produced from a solution containingCl ions; e.g., from

Question

Chlorine gas (Cl2) can be produced from a solution containingCl ions; e.g., from Na+Cl, by electrolysis. What must be the current through an electrolytic cell toproduce 1.0 kg of Cl2 gas in 7 hours? Use a charge of1.6x10-19 C, Avogadro’s number6.02x1023, and an atomic mass of 35.5 g forChlorine. Answer in units of A.

Explanation / Answer

Chlorine gas(Cl2) can be produced from a solution containing Clions; e.g., from Na+Cl, by electrolysis. What must bethe current through an electrolytic cell to produce 1.0 kg of Cl2 gas in 7hours? Use a charge of 1.6x10-19 C, Avogadro’s number6.02x1023, and an atomic mass of 35.5 g for Chlorine. Answer in units of A. {Chemical Equation} = { 2*Cl- ---> Cl2+ 2*e-} {Mass Of Cl2 Produced In 7 Hours} = (m_Cl2) =       = 1.0 kg       = 1000 g {Moles Of Cl2 Produced In 7 Hours} = (M_Cl2) =     = (m_Cl2)/(2*35.5 g/mole)       = (1000)/(2*35.5)       = 14.0845 moles Cl2 {Moles Of Electrons Produced In 7 Hours} = (M_e) =       = 2*(M_Cl2)       = 2*(14.0845)       = 28.169 moles e {Number Of Electrons Produced In 7 Hours} = (n_e) =       = (M_e)*(6.02e+23electrons/mole)       = (28.169)*(6.02e+23)      = 1.69577e+25electrons {Charge Of Electrons Produced In 7 Hours} = (Q_e) =       = (n_e)*(1.6e-19Coulombs/electron)       = (1.69577e+25)*(1.6e-19)       = 2713232 Coulombs {Current} = I =       = (Q_e)/(7 hours)       = (2713232)/((7 hours)*(3600 sec/hour))       = 107.7 Amps .

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