1.520g of the hydroxide of a metal on ignition gave 0.995 g of oxide. The equivalent mass of metal is:
1. 1.520
2. 0.995
3. 19.00
4. 9.00
0.5 g of fuming H2SO4 (oleum) is diluted with water. This solution is completely neutralised by 26.7 mL of 0.4 N NaOH. The percentage of free SO3 in the sample is:
1. 30.6%
2. 40.6%
3. 20.6%
4. 50%
The chloride of a metal contains 71% chlorine by mass and the vapour density of it is 50. The atomic mass of the metal will be:
1. 29
2. 58
3. 35.5
4. 71
The correct order of reducing power of halide ions is:
1. Cl- > Br- > I- > F-
2. Cl- > I- > Br- > F-
3. Br- > Cl- > I- > F-
4. I- > Br- > Cl- > F-
The reaction during which nitrogen gets oxidised is-
1. N2
2. NO
3. NO2
4. N
The oxidation state of Ni in Ni(CO)4 is:
1. zero
2. +4
3. +8
4. +2
In the preparation of chlorine from HCl; MnO2 acts as:
1. Reducing agent
2. Oxidising agent
3. Catalytic agent
4. Dehydrating agent
The oxidation number of carbon in C3O2 and Mg2C3 are respectively:
1. -4/3, +4/3
2. +4/3, -4/3
3. -2/3, +2/3
4. -2/3, +4/3
The oxidation number and covalency of sulphur in the sulphur molecule (S8) are respectively:
1. 0 and 2
2. +6 and 8
3. 0 and 8
4. +6 and 2
Hypochlorite disproportionate to give -
1. Cl- and Cl
2. Cl and Cl
3. Cl and Cl-
4. Cl and Cl-
When Cl2 is converted into Cl- & Cl then n-factor of Cl2 will be:
1. 3/5
2. 5/3
3. 7/2
4. 2
MnO2 + 4HCl MnCl2+2H2O+Cl2, the equivalent wt. of HCl will be (MMol wt of HCl)
1. M
2. M/2
3. 2M
4. M/4
In the following unbalanced reaction
A2+ + B3+ A4+ + B
The total number of e- transferred during reaction is
1. 2
2. 3
3. 6
4. 8
In the given reaction,
xBrO3- + yCr+3 + zH2O Br2 + CrO42- + H+
The coefficients x, y, and z are respectively-
1. 6, 10, 11
2. 6, 10, 20
3. 6, 8, 22
4. 6, 10, 22
In the following reaction
Al + Fe3O4 Al2O3 + Fe
The total number of electrons transferred will be-
1. 6
2. 8
3. 8/3
4. 24
x gram of pure As2S3 is completely oxidised to respective highest oxidation states by 50 ml of 0.1 M hot acidified KMnO4 then x mass of As2S3 taken is : (Molar mass of As2S3 = 246)
1. 22.4 g
2. 43.92 g
3. 64.23 g
4. None
In the reaction Na2S2O3 + 4Cl2 + 5H2O → Na2SO4 + H2SO4 + 8HCI the equivalent weight of Na2S2O3 will be
1. M/4
2. M/8
3. M/1
4. M/2
(M= molecular weight of Na2S2O3)
An excess of NaOH was added to 100 mL of a ferric chloride solution. This caused the precipitation of 1.425 g of Fe(OH)3. Calculate the normality of the ferric chloride solution
(1) 0.20 N
(2) 0.50 N
(3) 0.25 N
(4) 0.40 N
In the reaction CrO5 + H2SO4 → Cr2(SO4)3 + H2O + O2
The number of moles of O2 liberated by one mole of CrO5 will be -
1. 5/2
2. 5/4
3. 9/2
4. None of the above
0.4g of a polybasic acid HnA (all the hydrogens are acidic) requires 0.5g of NaOH for complete neutralization. The number of replaceable hydrogen atoms in the acid and the molecular weight of 'A' would be : (Molecular weight of the acid is 96 gms.)
1. 1, 95
2. 2, 94
3. 3, 93
4. 4, 92
If 10 gm of V2O5 is dissolved in acid and is reduced to V2+ by zinc metal, how many moles of I2 could be reduced by the resulting solution if it is further oxidized to VO2+ ions?
[Assume no change in state of Zn2+ions] (V = 51, O =16, I = 127) :
1. | 0.11 mole of I2 | 2. | 0.22 mole of I2 |
3. | 0.055 mole of I2 | 4. | 0.44 mole of I2 |
0.70 g of mixture (NH4)2 SO4 was boiled with 100 mL of 0.2 N NaOH solution till all the NH3(g) evolved and get dissolved in solution itself. The remaining solution was diluted to 250 mL. 25 mL of this solution was neutralized using 10 mL of a 0.1 N H2SO4 solution. The percentage purity of the (NH4)2 SO sample is
(1) 94.3
(2) 50.8
(3) 47.4
(4) 79.8
One gm. of a metal carbonate gave 0.56 gm. of its oxide on heating. The equivalent mass of the metal is
1. 40
2. 30
3. 20
4. 10
The number of moles of MnO-4 required to oxidise one mole of ferrous oxalate completely in an acidic medium is-
1. 0.6 mole
2. 0.4 mole
3. 7.5 moles
4. 0.2 mole
The number of mole of KMnO4 that will be needed to react with one mole of sulphite ion in acidic solution is:
(1)
(2)
(3)
(4) 1
A brown ring complex compound is formulated as The oxidation state of iron is
1. 1
2. 2
3. 3
4. 0
In an alkaline medium ClO2 oxidize H2O2 in O2 and reduces itself in Cl– . How many moles of H2O2 will be oxidized by one mole of ClO2?
1. | 1.0 | 2. | 1.5 |
3. | 2.5 | 4. | 3.5 |
One mole of N2H4 loses 10 mole of electrons to form a new compound Y. Assuming that all nitrogen appear in the new compound, what is the oxidation state of N2 in Y ? (There is no change in the oxidation state of hydrogen)
1. + 3
2. – 3
3. – 1
4. + 5
When is fused with KOH, a coloured compound is formed, the product and its colour is [IIT Screening 2003]
(1) , purple green
(2) , purple
(3) , brown
(4) black
Read the following statements (S) and Explanation (E). Choose the correct answers from the codes (1), (2), (3) and (4):
S : is monobasic Lewis acid but salt exist.
E : reacts with to give .
1. S is correct but E is wrong
2. S is wrong but E is correct
3. Both S and E are correct and E is correct explanation of S
4. Both S and E are correct but E is not correct explanation of S