276084 One faraday of current was passed through the electrolytic cells placed in series containing solution of $\mathrm{Ag}^{+}, \mathrm{Ni}^{2+}$ and $\mathrm{Cr}^{3+}$ respectively. The ratio of amounts of $\mathrm{Ag}, \mathrm{Ni}$ and $\mathrm{Cr}$ deposited will be
(At. wt. of $\mathrm{Ag}=108, \mathrm{Ni}=59, \mathrm{Cr}=52$ )

276020 How many gram of cobalt metal will be deposited, when a solution of cobalt(II) chloride is electrolyzed with a current of 10 amperes for 109 minutes (1 Faraday $=96,500$ $\mathrm{C}$; Atomic mass of $\mathrm{Co}=\mathbf{5 9} \mathrm{u})$

275993 Given below are half cell reactions
$\mathrm{MnO}_{4}^{-}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O}$
$\mathrm{E}_{\mathrm{Mn}^{2+} / \mathrm{MnO}_{4}^{-}}^{0}=-1.510 \mathrm{~V}$
$\frac{1}{2} \mathrm{O}_{2}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow \mathrm{H}_{2} \mathrm{O}$
$\mathrm{E}_{\mathrm{O}_{2} / \mathrm{H}_{2} \mathrm{O}}^{\mathrm{0}}=1.223 \mathrm{~V}$
Will the permanganate ion, $\mathrm{MnO}_{4}^{-}$liberate $\mathrm{O}_{2}$ from water in the presence of an acid?

276021 When 965 coulombs of electricity is passed through a solution of silver nitrate, the amount of silver deposited is

276084 One faraday of current was passed through the electrolytic cells placed in series containing solution of $\mathrm{Ag}^{+}, \mathrm{Ni}^{2+}$ and $\mathrm{Cr}^{3+}$ respectively. The ratio of amounts of $\mathrm{Ag}, \mathrm{Ni}$ and $\mathrm{Cr}$ deposited will be
(At. wt. of $\mathrm{Ag}=108, \mathrm{Ni}=59, \mathrm{Cr}=52$ )

276020 How many gram of cobalt metal will be deposited, when a solution of cobalt(II) chloride is electrolyzed with a current of 10 amperes for 109 minutes (1 Faraday $=96,500$ $\mathrm{C}$; Atomic mass of $\mathrm{Co}=\mathbf{5 9} \mathrm{u})$

275993 Given below are half cell reactions
$\mathrm{MnO}_{4}^{-}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O}$
$\mathrm{E}_{\mathrm{Mn}^{2+} / \mathrm{MnO}_{4}^{-}}^{0}=-1.510 \mathrm{~V}$
$\frac{1}{2} \mathrm{O}_{2}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow \mathrm{H}_{2} \mathrm{O}$
$\mathrm{E}_{\mathrm{O}_{2} / \mathrm{H}_{2} \mathrm{O}}^{\mathrm{0}}=1.223 \mathrm{~V}$
Will the permanganate ion, $\mathrm{MnO}_{4}^{-}$liberate $\mathrm{O}_{2}$ from water in the presence of an acid?

276021 When 965 coulombs of electricity is passed through a solution of silver nitrate, the amount of silver deposited is

276084 One faraday of current was passed through the electrolytic cells placed in series containing solution of $\mathrm{Ag}^{+}, \mathrm{Ni}^{2+}$ and $\mathrm{Cr}^{3+}$ respectively. The ratio of amounts of $\mathrm{Ag}, \mathrm{Ni}$ and $\mathrm{Cr}$ deposited will be
(At. wt. of $\mathrm{Ag}=108, \mathrm{Ni}=59, \mathrm{Cr}=52$ )

276020 How many gram of cobalt metal will be deposited, when a solution of cobalt(II) chloride is electrolyzed with a current of 10 amperes for 109 minutes (1 Faraday $=96,500$ $\mathrm{C}$; Atomic mass of $\mathrm{Co}=\mathbf{5 9} \mathrm{u})$

275993 Given below are half cell reactions
$\mathrm{MnO}_{4}^{-}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O}$
$\mathrm{E}_{\mathrm{Mn}^{2+} / \mathrm{MnO}_{4}^{-}}^{0}=-1.510 \mathrm{~V}$
$\frac{1}{2} \mathrm{O}_{2}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow \mathrm{H}_{2} \mathrm{O}$
$\mathrm{E}_{\mathrm{O}_{2} / \mathrm{H}_{2} \mathrm{O}}^{\mathrm{0}}=1.223 \mathrm{~V}$
Will the permanganate ion, $\mathrm{MnO}_{4}^{-}$liberate $\mathrm{O}_{2}$ from water in the presence of an acid?

276021 When 965 coulombs of electricity is passed through a solution of silver nitrate, the amount of silver deposited is

276084 One faraday of current was passed through the electrolytic cells placed in series containing solution of $\mathrm{Ag}^{+}, \mathrm{Ni}^{2+}$ and $\mathrm{Cr}^{3+}$ respectively. The ratio of amounts of $\mathrm{Ag}, \mathrm{Ni}$ and $\mathrm{Cr}$ deposited will be
(At. wt. of $\mathrm{Ag}=108, \mathrm{Ni}=59, \mathrm{Cr}=52$ )

276020 How many gram of cobalt metal will be deposited, when a solution of cobalt(II) chloride is electrolyzed with a current of 10 amperes for 109 minutes (1 Faraday $=96,500$ $\mathrm{C}$; Atomic mass of $\mathrm{Co}=\mathbf{5 9} \mathrm{u})$

275993 Given below are half cell reactions
$\mathrm{MnO}_{4}^{-}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O}$
$\mathrm{E}_{\mathrm{Mn}^{2+} / \mathrm{MnO}_{4}^{-}}^{0}=-1.510 \mathrm{~V}$
$\frac{1}{2} \mathrm{O}_{2}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow \mathrm{H}_{2} \mathrm{O}$
$\mathrm{E}_{\mathrm{O}_{2} / \mathrm{H}_{2} \mathrm{O}}^{\mathrm{0}}=1.223 \mathrm{~V}$
Will the permanganate ion, $\mathrm{MnO}_{4}^{-}$liberate $\mathrm{O}_{2}$ from water in the presence of an acid?

276021 When 965 coulombs of electricity is passed through a solution of silver nitrate, the amount of silver deposited is