Experimentally it was found that a metal oxide has formula M0.98O.Metal M, is present as M2+and M3+ in its oxide. Fraction of the metal which exists as M3+ would be: (2013)
7.01 %
4.08 %
6.05 %
5.08 %
A gaseous hydrocarbon gives upon combustion 0.72 g . of water and 3.08 g. of CO2.The empirical formula of the hydrocarbon is. (2013)
C2H4
C3H4
C6H5
C7H8
Consider the following reaction,
xMnO4- + yC2O42- + zH+ → xMn2+ +2yCO2+z/2 H2O
The values of x, y and z in the reaction are, respectively (2007)
5,2 and 16
2,5 and 8
2,5 and 16
5, 2 and 8
In the reaction,
2AI(s) +6HCl(aq) 2Al3+(aq) + 6Cl- (aq) + 3H2 (g) (2007)
11.2 L H2 (g) at STP is produced for every mole HCl (aq) consumed.
6 L HCl(aq) is consumed for every 3L H2 (g) produced.
33.6 L H2(g) is produced regardless of temperature and pressure for every mole Al that reacts.
67.2 H2(g) at STP is produced for every mole Al that reacts.
The density (in g mL-1) of a 3.60 M sulphuric acid solution that is 29% H2SO4 (molar mass = 98 g mol-1) by mass will be. (2007)
1.45
1.64
1.88
1.22
Consider a titration of potassium dichromate solution with acidified Mohr’s salt solution using diphenylamine as indicator. The number of moles of Mohr’s salt required per mole of dichromate is. (2007)
3
4
5
6
Density of a 2.05M solution of acetic acid in water is 1.02 g/mL. The molality of the solution is. (2006)
2.28 mol kg-1
0.44 mol kg-1
1.14 mol kg-1
3.28 mol kg-1
How many moles of magnesium phosphate, Mg3(PO4)2 will contain 0.25 mole of oxygen atoms? (2006)
1.25 10-2
2.5 10-2
0.02
3.125 10-2
If we consider that ⅙, in place of 1/12, mass of carbon atom is taken to be the relative atomic mass unit, the mass of one mole of the substance will (2005)
Be a function of the molecular mass of the substance
Remain unchanged
Increase two fold
Decrease twice
Two solutions of a substance (non electrolyte) are mixed in the following manner. 480 ml of 1.5 M first solution + 520 ml of 1.2 M second solution. What Is the Molarity of the final mixture. (2005)
2.70 M
1.344 M
1.50 M
1.20 M
The pair of the compounds in which both the metals are in the highest possible oxidation state is (2004)
[Fe(CN)6]3- , [Co(CN)6]3-
CrO2Cl2 , MnO4-
TiO3 , MnO2
[Co(CN)6]3- , MnO3
The ammonia evolved from the treatment of 0.30 g of an organic compound for the estimation of nitrogen was passed in 100 mL of 0.1 M sulphuric acid. The excess of acid required 20 mL of 0.5 M sodium hydroxide solution for complete neutralization. The organic compound is (2004)
Urea
Benzamide
Acetamide
Thiourea
To neutralize completely 20 mL of 0.1M aqueous solution of phosphorous acid (H3PO3), the value of 0.1 M aqueous KOH solution required is. (2004)
40mL
20mL
10mL
60mL
6.02 1020 molecules of urea are present in 100 mL of its solution. The concentration of urea solution is. (2004)
0.02M
0.01M
0.001M
0.1M
25 mL of a solution of barium hydroxide on titration with a 0.1 molar solution of Hydrochloric acid gave a litre value of 35 ml. The molarity of barium hydroxide solution was. (2003)
0.14
0.28
0.35
0.07
What volume of Hydrogen gas, at 273 K and 1 atm, pressure will be consumed in obtaining 21.6 g of elemental boron (atomic mass = 10.8) from the reduction of boron trichloride by hydrogen ? (2003)
67.2L
44.8L
22.4L
89.6L
Mixture of X = 0.02 mol of [Co(NH3)5SO4]Br and 0.02 mol of [Co(NH3)5Br]SO4 was prepared in 2 litre of solution.
1 litre of mixture X + excess AgNO3 Y
1 litre of mixture X + excess BaCl2 Z
No. of moles of Y and Z are. (2003)
0.01,0.01
0.02,0.01
0.01,0.02
0.02,0.02
Number of atoms in 558.5 gram Fe (at. Wt. of Fe = 55.85 g mol-1) is. (2002)
Twice that in 60 g carbon
6.023 1022
Half that in 8 g He
558.5 6.023 1023
With the increase of temperature, which of these changes ? (2002)
Molality
Weight fraction of solute
Molarity
Mole fraction
In a compound C,H and N atoms are present in 9:1:3.5 by weight. Molecular weight of the compound is 108. Molecular formula of compound is. (2002)
C2H6N2
C3H4N
C6H8N2
C9H12N3
