|
Calculate the atomic mass (average) of chlorine using the following data :
|
|
1
|
1069
|
August 9, 2016
|
|
An organometallic compound on analysis was found to contain, C = 64.4%, H = 5.5% and Fe = 29.9%
|
|
1
|
16866
|
August 9, 2016
|
|
How many grams of $C{{l}_{2}}$ are required to completely react with 0.4 g of ${{H}_{2}}$ to yield HCl ?Also, calculate the amount of HO formed
|
|
0
|
1008
|
August 9, 2016
|
|
56 kg of ${{N}_{2}}$(g) and 10 kg of ${{H}_{2}}$(g) are mixed to produce N${{H}_{3}}$(g)
|
|
1
|
1029
|
August 9, 2016
|
|
If the density of methanol is 0.793 kg per litre. What is its volume needed for making 2.51 of its 0.25 M solution
|
|
0
|
1197
|
August 9, 2016
|
|
Use the data given in the following table to calculate the molar mass of naturally occurring argon isotopes:
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|
1
|
2967
|
August 9, 2016
|
|
Calculate the concentration of nitric acid in moles per litre in a sample which has a density, 1.41 g ${{ml}^{-1}}$ and the mass percent of nitric acid in it being 69%
|
|
0
|
3836
|
August 9, 2016
|
|
How much copper can obtained from 100 g of copper sulphate ?[At Mass of Cu = 63.5 u]
|
|
0
|
825
|
August 9, 2016
|
|
Density of water at room temperature is 1.0 g/ cc. How many molecules are there in one drop of water if its volume is 0.1 cc
|
|
0
|
2857
|
August 9, 2016
|
|
Calculate the volume of 34g of N${{H}_{3}}$ at STP
|
|
0
|
500
|
August 9, 2016
|
|
0.5 mole each of $H_{2}$S and S$O_{2}$ mixed together in a reaction flask, react according to equation :
|
|
1
|
414
|
August 9, 2016
|
|
Why are the atomic masses of most of the elements fractional?
|
|
0
|
1641
|
August 9, 2016
|
|
Calculate the number of atoms present in 1.4 g of ${{N}_{2}}$ molecule
|
|
0
|
440
|
August 9, 2016
|
|
Calculate the mass of 112 $c{{m}^{3}}$ of hydrogen gas at STP
|
|
0
|
617
|
August 9, 2016
|
|
Boron occurs in nature in the form of two isotopes ${{11}_{5}}$B and ${{10}_{5}}$B in ratio of 81% and 19% respectively. Calculate its average atomic mass
|
|
0
|
1562
|
August 9, 2016
|
|
How many electrons are present in 16g of C${{H}_{4}}$
|
|
0
|
471
|
August 9, 2016
|
|
Calculate molecular mass of glucose (Cg$H_{12}O_{6}$) molecule
|
|
0
|
486
|
August 9, 2016
|
|
Calculate the percentage of nitrogen in N${{H}_{3}}$
|
|
1
|
1139
|
August 9, 2016
|
|
Vitamin C is known to contain 1.29 X ${{10}^{24}}$ hydrogen atoms.Calculate the number of moles of hydrogen atoms
|
|
0
|
4367
|
August 9, 2016
|
|
A box contains some identical red coloured balls,labelled as A, each weighing 2 grams
|
|
1
|
1209
|
August 9, 2016
|
|
50.0 Kg of ${{N}_{2}}$(g) and 10.0 Kg of ${{H}_{2}}$(g) are mixed to produce N${{H}_{3}}$(g). Calculate the N${{H}_{3}}$(g) formed. Identify the limiting reagent in the production of N${{H}_{3}}$ in this situation
|
|
0
|
890
|
August 9, 2016
|
|
A mixture of oxalic acid and formic acid is heated with concentrated ${{H}_{2}}S{{O}_{4}}$ and gas evolved is collected
|
|
1
|
1626
|
August 9, 2016
|
|
State the law of Constant Composition. Illustrate with two examples
|
|
0
|
3967
|
August 9, 2016
|
|
What is the law of Multiple Proportions. Explain giving examples
|
|
0
|
4333
|
August 9, 2016
|
|
What weight of iodine is liberated from a solution of potassium iodide when 1 litre of $C{{l}_{2}}$ gas at 10°C and 750 mm pressure is passed through it?
|
|
0
|
4036
|
August 9, 2016
|
|
What is limiting reactant?
|
|
1
|
1748
|
August 9, 2016
|
|
Two oxides of the metal contain 27.6 % and 30.0 % of oxygen respectively, If the formula of the first oxide is $M_{3}O_{4}$, find that of the second
|
|
0
|
5646
|
August 9, 2016
|
|
Calculate the volume of 0.05 KMn${{O}_{4}}$ solution re-quired to oxidise completely 2.70 g of oxalic acid in acidic solution
|
|
0
|
940
|
August 9, 2016
|
|
The mass of precious stones is expressed in term of 'carat'
|
|
1
|
2955
|
August 9, 2016
|
|
The reactant which is entirely consumed in reaction is known as limiting reagent. In the reaction
|
|
1
|
5308
|
August 9, 2016
|