Q. No.What is the alteration in the oxidation state of carbon in the given reaction?
\(\mathrm{{CH_4}_{(g)} + 4{Cl_2}_{(g)} \rightarrow {CCl_4}_{(l)} + 4 HCl_{(g)}}\)
1.
0 to +4
2.
–4 to +4
3.
0 to –4
4.
+4 to +4
The incorrect oxidation number of the underlined atom in the following species is:
| 1. | Cu2O is -1 | 2. | Cl\(O_{3}^{-}\) is +5 |
| 3. | K2Cr2O7 is +6 | 4. | HAuCl4 is +3 |
From the following, identify the reaction having the top position in the EMF series (standard reduction potential) according to their electrode potential at 298 K.
| 1. | Mg2++ 2e– → Mg(s) | 2. | Fe2+ + 2e– → Fe(s) |
| 3. | Au3++ 3e– → Au(s) | 4. | K++ 1e – → K(s) |
The standard electrode potential (E°) values of Al3+/ Al, Ag+ / Ag, K+ / K, and Cr3+ / Cr are –1.66 V, 0.80 V, –2.93 V, & –0.79 V respectively. The correct decreasing order of the reducing power of the metals is:
| 1. | Ag > Cr > Al > K | 2. | K > Al > Cr > Ag |
| 3. | K > Al > Ag > Cr | 4. | Al > K > Ag > Cr |
The correct example of metal displacement reaction among the following is:
| 1. | \(\mathrm{Fe}+2 \mathrm{HCl} \rightarrow \mathrm{FeCl}_2+\mathrm{H}_2 \uparrow \) |
| 2. | \(2 \mathrm{~Pb}\left(\mathrm{NO}_3\right)_2 \rightarrow 2 \mathrm{PbO}+4 \mathrm{NO}_2+\mathrm{O}_2 \uparrow \) |
| 3. | \( 2\text {KClO}_3 \xrightarrow {\Delta}2 \text {KCl} + 3 \text O_2 \) |
| 4. | \(\mathrm{Cr}_2 \mathrm{O}_3+2 \mathrm{Al} \xrightarrow {\Delta} \mathrm{Al}_2 \mathrm{O}_3+2 \mathrm{Cr}\) |
Disproportionation reactions are:
| (a) | |
| (b) | |
| (c) | |
| (d) |
| 1. | (a) and (d) only | 2. | (a) and (b) only |
| 3. | (a), (b) and (c) | 4. | (a), (c) and (d) |
| 1. | Lithium is the strongest reducing agent among the alkali metals. |
| 2. | Alkali metals react with water to form their hydroxides. |
| 3. | The oxidation number of K in KO2 is +4. |
| 4. | Ionisation enthalpy of alkali metals decreases from top to bottom in the group. |
On the basis of standard electrode potentials, predict which of the following reaction can not occur?
| 1. | \(\mathrm{2 {CuSO}_{4}({aq})+2 {Ag}({s}) → 2 {Cu}({s})+{Ag}_{2} {SO}_{4}({aq})} \) |
| 2. | \(\mathrm{{CuSO}_{4}({aq})+{Zn}({s})} \) \(\mathrm{→ {ZnSO}_{4}({aq})+{Cu}({s})} \) |
| 3. | \(\mathrm{{CuSO}_{4}({aq})+{Fe}({s})} \) \(\mathrm{→ {FeSO}_{4}({aq})+{Cu}({s})} \) |
| 4. | \(\mathrm{{FeSO}_{4}({aq})+{Zn}({s})} \) \(→ \mathrm{{ZnSO}_{4}({aq})+{Fe}({s})} \) |
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