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प्रश्न
Identify A to E and also explain the reactions involved.
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उत्तर
A = \[\ce{Cu}\]
B = \[\ce{Cu(NO3)2}\]
C = \[\ce{[Cu(NH3)4]}\]
D = \[\ce{CO2}\]
E = \[\ce{CaCO3}\]
F = \[\ce{Cu2[Fe(CN)6]}\]
G = \[\ce{Ca (HCO3)2}\]
\[\ce{CuCO3 -> CuO + CO2}\]
\[\ce{CuO + CuS -> \underset{(A)}{Cu} + SO2}\]
\[\ce{Cu + 4HNO3 (Conc) -> Cu \underset{(B)}{(NO3)2} + 2NO + 2H2O}\]
\[\ce{\underset{(B)}{Cu^2+} + NH3 -> \underset{(C)}{[Cu(NH3)4]}}\]
\[\ce{Ca(OH)2 + \underset{(D)}{CO2} -> \underset{(E)}{CaCO3} + H2O}\]
\[\ce{CaCO3 + CO2 + H2O -> Ca(HCO3)2}\]
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संबंधित प्रश्न
How would you account for the following: Transition metals form complex compounds.
|
`E_((M^(2+)/M)` |
Cr | Mn | Fe | Co | Ni | Cu |
| -0.91 | -1.18 | -0.44 | -0.28 | -0.25 | -0.34 |
From the given data of E0 values, answer the following questions :
(1) Why is `E_(((Cu^(2+))/(Cu)))` value exceptionally positive
(2) Why is `E_(((Mn^(2+))/(Mn)))` value is highly negative as compared to other elements
(3) Which is the stronger reducing agents Cr2+ or Fe2+ ? Give Reason.
How is the variability in oxidation states of transition metals different from that of the non-transition metals? Illustrate with examples.
How is the variability in oxidation states of transition metals different from that of the non-transition metals? Illustrate with examples.
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