Calculate the volume of `Cl_(2)` at `27^@ C` and `2 atm` produced during electrolysis of `MgCl_(2)` which produced `6.50 g Mg.` (`At. wt.` of `Mg = 24.3`)

Calculate the volume of Cl_(2) at NTP produced during electrolysis of MgCl_(2) which produces 6.50 g Mg. (At. Mass of Mg = 24.3)

Find the volume of Cl_(2) at NTP produced during electrolysis of MgCl_(2) which produces 6.6 g Mg . ("At.wt. of " Mg = 24.3)

The hydrolysis of Mg_(2)C_(3) produces

Name the product formed when Cl_(2) and H_(2) produced during the electrolysis of brine aremade to combine.

Calculatethemassof Mg andvolume of chlorine gas at STP produced during electrolysis of molten MgCl_2 by the passage of 2 amperes of current for 1 hour. Molar masses of Mg and Cl_2 are respectivley 24 g mol^(-1) and 71 g mol^(-1) .

1*2 g of Mg (At mass 24) will produce MgO equal to

1.2g of Mg (At. mass 24) will produce MgO equal to

How many amperes would be needed to produce 60.0 g of magnesium during the electrolysis of molten MgCl_(2) in 2 hours ?