Which element exhibits both positive and negative oxidation states?
Cs
Ne
I
F
The balanced equation for the reaction between chlorine and sulphur dioxide in water is-
Cl2(s) + SO2(aq) + 2H2O(I) →2Cl-(aq) + SO42-(aq) + 4H+(aq)
3Cl2(s) + SO2(aq) + 2H2O(I) →Cl-(aq) + SO42-(aq) + 3H+(aq)
Cl2(s) + 3SO2(aq) + H2O(I) →Cl-(aq) + 2SO42-(aq) + 4H+(aq)
2Cl2(s) + SO2(aq) + H2O(I) →2Cl-(aq) + SO42-(aq) + 4H+(aq)
The set of metals that can show disproportionation reaction is -
Cu, Na, Li
Mg, F, Ne
P, Cl, S
Mn, Cu, Ga
The maximum weight of nitric oxide that can be obtained starting only with 10.00 g of ammonia and 20.00 g of oxygen is -
9 g
15 g
12 g
11g
In Fe0.90O , Fe is present in +2 and +3 oxidation state. What is the mole fraction of Fe3+ in the compound ?
0.22
0.77
0.90
None
The correct decreasing order of following metals in which they displace each other from the solution of their salts is: Al, Cu, Fe, Mg and Zn.
1) Al> Zn > Fe > Cu > Mg
2) Zn > Fe > Cu > Mg > Al
3) Mg > Al > Zn > Fe > Cu
4) Fe > Mg > Zn > Al > Cu
The correct statement about the electrolysis of an aqueous solution of AgNO3 with Ag electrode is-
Ag+ion gets oxidised at cathode; Ag(s) is reduced at anode
H2O gets reduced at cathode; H2O gets oxidised at anode
Ag+ion gets reduced at cathode; H2O gets oxidised at anode
Ag+ion gets reduced at cathode; Ag(s) gets oxidised at anode
The reactions of electrolysis for a dilute solution of H2SO4 with platinum electrode are-
H+ ion reduce at cathode; H2O oxidised at anode
H+ ion reduce at cathode; SO42- ion oxidised at anode
H2O ion reduce at cathode; H2O oxidised at anode
H2O ion reduce at cathode; H+ ion oxidised at anode
The correct statement about electrolysis of an aqueous solution of CuCl2 with Pt electrode is-
Cu2+ ion reduced at the cathode; Cl- ion oxidized at the anode
Cu2+ ion reduced at the anode; Cl- ion oxidized at the cathode
Cu2+ ion reduced at the cathode; H2O ion oxidized at the anode
H2O ion reduced at the cathode; Cl- ion oxidized at the anode
The oxidizing agent and reducing agent in the given reaction are
3N2H4l+4ClO3aq-→6NOg+4Claq-+6H2Ol
Oxidising agent = N2H4; Reducing agent = ClO3-
Oxidising agent = ClO3-; Reducing agent = N2H4
Oxidising agent = N2H4 ; Reducing agent = N2H4
Oxidising agent = ClO3- ; Reducing agent = ClO3-
The oxidising agent and reducing agent in the given reaction are
Cl2O7g+4H2O2aq+2OHaq-→2ClO2aq-+4O2g+5H2Ol
Oxidizing agent = H2O2; Reducing agent = Cl2O7
Oxidizing agent = Cl2O7; Reducing agent = H2O2
Oxidizing agent = H2O2; Reducing agent = H2O2
None of the above
Given a galvanic cell with the following reaction
Zn(s) + 2Ag+(aq) →Zn+2(aq) + Ag(s)
The negatively charged electrode will be-
Zn
Ag
Both
The oxidation states of the central atom in the given species are, respectively:
H4P2O7 and H2S2O7
0 and +6
+3 and +4
+4 and +2
+5 and +6
KI3 , H2S4O6
The oxidation numbers of iodine and sulphur in the above compounds are, respectively?
1. 13; 42. 2.5; 133. 13; 2.54. 2.5; 3
The metal displacement reaction among the following is -
Fe+2HCl→FeCl2+H2↑
2Pb(NO3)2→2PbO+4NO2+O2↑
2KClO3→∆2KCl+3O2
Cr2O3+2Al→∆Al2O3+2Cr
2 Na(s) + H2(g) → 2 NaH (s)The incorrect statement among the following regarding above mentioned reaction is-
2Cu2O(s) + Cu2S(s) → 6Cu(s) + SO2(g)The correct statement among the following regarding above mentioned reaction is-
The species among the following that does not show a disproportionation reaction is-
ClO–, ClO2–, \(ClO_{3}^{-}\) and ClO4–
ClO–
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