75.0 g of carbon is reacted with water at high temperature to produce water gas $(CO + H_{2})$ . Liberated CO is separated and used for refining of nickel by Mond process. Assuming 100% reaction and 100% recovery calculate moles of $[Ni (CO)_{4}]$ obtained.
[Atomic mass of Ni – 58.6 g mol^-1 ]

Question

75.0 g of carbon is reacted with water at high temperature to produce water gas $(CO + H_{2})$ . Liberated CO is separated and used for refining of nickel by Mond process. Assuming 100% reaction and 100% recovery calculate moles of $[Ni (CO)_{4}]$ obtained.

[Atomic mass of Ni – 58.6 g mol^-1 ]

TestHub · Accepted Answer

Water gas is formed by: C + H 2 ​ O → CO + H 2 ​ . Thus, 1 m o lCp ro d u ces 1 m o lCO . Moles of carbon = 12 75 ​ = 6.25 m o l , so CO f or m e d = 6.25 m o l . In the Mond process: N i + 4 CO → N i ( CO ) 4 ​ ; therefore, 4 m o lCO f or m 1 m o lN i ( CO ) 4 ​ . Moles of N i ( CO ) 4 ​ = 4 6.25 ​ = 1.5625 ≈ 1.56 m o l .

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