Which of The following has a maximum number of molecules?
1. 7g N2
2. 2g H2
3. 16g NO2
4. 16g O2
How much oxygen gas (O2) at standard temperature (0°C) and pressure (1 atm) is required to completely combust 1 liter of propane gas (C3H8) under the same conditions?
1. 7L
2. 6L
3. 5L
4. 10L
The product of atomic mass and specific heat of metal is approximately 6.4. This was given by:
1. Dalton's law
2. Avogadro's law
3. Newton's law
4. Dulong Petit's law
A gas is found to have the formula (CO)x. Its VD is 70. The value of x must be:
1. 7
2. 4
3. 5
4. 6
2 gm Iron pyrite (FeS2) is burnt with O2 to form Fe2O3 and SO2. The mass of SO2 produced is (Fe=56, S=32, O=16)
1. 2 gm
2. 2.13 gm
3. 4 gm
4. 4.26 gm
Oxygen contains 90% O16 and 10% O18. Its atomic mass is
(1) 17.4
(2) 16.2
(3) 16.5
(4) 17
KClO3 on heating decomposes to KCl and O2. The volume of O2 at STP liberated by 0.1 mole KClO3 is
1. 4.36 L
2. 3.36 L
3. 2.36 L
4. None of these
At S.T.P. the density of CCl4 vapour in g/L will be nearest to [CBSE PMT 1988]
(1) 6.84
(2) 3.42
(3) 10.26
(4) 4.57
4.4 g of an unknown gas occupies 2.24 litres of volume at NTP. The gas may be:
1. | Carbon dioxide | 2. | Carbon monoxide |
3. | Oxygen | 4. | Sulphur dioxide |
The mass of carbon present in 0.5 mole of K4[Fe(CN)6] is
(1) 1.8 g
(2) 18 g
(3) 3.6 g
(4) 36 g
The number of moles of oxygen in one litre of air containing 21% oxygen by volume under standard conditions is [CBSE PMT 1995]
(1) 0.186 mole
(2) 0.21 mole
(3) 0.0093 mole
(4) 2.10 mole
The empirical formula of an organic compound containing carbon and hydrogen is CH2. The mass of one litre of this organic gas at STP is exactly equal to that of one litre of N2 STP.Therefore, the molecular formula of the organic gas is
1. C2H4
2. C3H6
3. C6H12
4. C4H8
An organic compound containing C, H, and N gave the following on analysis: C = 40%, H = 13.3% and N = 46.67%. Its empirical formula would be:
1. CHN
2. C2H2N
3. CH4N
4. C2H7N
At standard temperature and pressure (STP), the volume of oxygen required to completely combust 30 ml of acetylene under similar conditions is:
1. 100 ml
2. 75 ml
3. 50 ml
4. 25 ml
If the Avogadro number NA, is changed from 6.022 x 1023 mol-1 to 6.022 x 1020 mol-1 this would change:
1. The definition of mass in units of grams.
2. The mass of one mole of carbon.
3. The ratio of chemical species to each other in a balanced equation.
4. The ratio of elements to each other in a compound.
6.02 x 1020 molecules of urea are present in 100 mL of its solution. The concentration of the solution is:
1. | 0.02 M | 2. | 0.01 M |
3. | 0.001 M | 4. | 0.1 M |
The maximum amount of BaSO4 precipitated on mixing 20mL of 0.5 M BaCl2 with 20 mL of 1 M H2SO4 is:
1. 0.25 mole
2. 0.5 mole
3. 1 mole
4. 0.01 mole
Insulin contains 3.4% sulphur: The minimum molar mass of insulin is:
1. 941 g
2. 1000 g
3. 841 g
4. 1041 g
1.60 g of a metal were dessolved in HNO3 to prepare its nitrate. The nitrate on strong heating gives 2 g oxide. The equvalent mass of metal is:
1. 16
2. 32
3. 48
4. 12
100 ml each of 0.5 N NaOH, N/5 HCl and N/10 H2SO4 are mixed together. The resulting solution will be
1. Acidic
2. Alkaline
3. Neutral
4. Can't be determine
An element A (at. wt. = 75) and B (at. wt. = 25) combine to form a compound that contains 75% A by weight. The formula of the compound will be:
1. A2B
2. A3B
3. AB3
4. AB
The ratio of number of atoms in 4.4 gm CO2 and 1.7 gm NH3 is
1. 1:1
2. 3:4
3. 4:3
4. 1:2
, 6.4 gm SO2 and 3.2 gm O2 to form SO3. How much maximum mass of SO3 is formed?
1. 32 gm
2. 16 gm
3. 8 gm
4. 4 gm
A metallic nitride(M3N2) contains 20% nitrogen. Equivalent weight of metal is
1. 37.33
2. 18.67
3. 112
4. 56
The weight of iron which will be converted into oxide (Fe3O4) by the action of 18 gm of steam of it will be (at. wt. of Fe = 56)
1. 168 gm
2. 84 gm
3. 42 gm
4. 21 gm
Calculate the molality of 20% CaCO3 solution is (by mass). The density of solution is 1.2 gm/ml
1. 1.25 m
2. 2.5 m
3. 2.08 m
4. 1.5 m
A mixture of methane and ethene in the molar ratio of x : y has a mean molar mass of 20. What would be the mean molar mass. if the gases are mixed in the molar ratio of y : x?
(1) 22
(2) 24
(3) 20.8
(4) 19
The volume of a drop of water is 0.0018 mL then the number of water molecules present in two drop of water at room temperature is:
1.
2.
3.
4.
Carbon and oxygen combine to form two oxides, carbon monoxide and carbon dioxide in which the ratio of the weights of carbon and oxygen is respectively 12 : 16 and 12 : 32. These figures illustrate the:
1. Law of multiple proportions
2. Law of reciprocal proportions
3. Law of conservation of mass
4. Law of constant proportions
The formula of an acid is The mass of 0.0242 moles of the acid is 1.657 g.
The atomic weight of X is:
1. | 35.5 | 2. | 28.1 |
3. | 128 | 4. | 19.0 |
A 6.85 g sample of the hydrates is dried in an oven to give 3.13 g of anhydrous . The value of x is -
(Atomic weights : Sr=87.60, O=16.0, H=1.0)
1. 8
2. 12
3. 10
4. 6
A sample of phosphorus that weights 12.4 g exerts a pressure 8 atm in a 0.821 litre closed vessel at 527C. The molecular formula of the phosphorus vapour is:
1.
2.
3.
4.
Phosphoric acid prepared in a two step process.
(1)
(2)
We allow 62g of phosphorus to react with react with excess oxygen which form in 85% yield. In the step (2) reaction 90% yield of is obtained. Produced mass of is:
1. 37.485 g
2. 149.949 g
3. 125.47 g
4. 564.48 g
What volume of HCl solution of density 1.2 g/cm3 and containing 36.5% by weight HCl, must be allowed to react with zinc(Zn) in order to liberate 4.0 g of hydrogen?
1. 333.33 mL
2. 500 mL
3. 614.66 mL
4. None of these
The molar mass of diacidic organic Lewis base (B), if 12 g of chloroplatinate salt on ignition produced 5 gm residue of Pt,will be -
1. 52
2. 58
3. 88
4. None of these
What volume of measured at 1 atm and 273 K will be formed by the action of 100 mL of 0.5 N KMnO4 on hydrogen peroxide in an acid solution?
The skeleton equation for the reaction is
1. 0.12 litre
2. 0.028 litre
3. 0.56 litre
4. 1.12 litre
Cisplatin, an anticancer drug, has the molecular formula . What is the mass (in gram) of one molecule? (Atomic weights : Pt=195, H=1.0, N=14, Cl=35.5)
1.
2.
3.
4.
The conversion of oxygen to ozone occurs to the extent of 15% only. The mass of ozone that can be prepared from 67.2 L oxygen at 1 atm and 273 K will be:
1. 14.4 gm
2. 96 gm
3. 640 gm
4. 64 gm
Average atomic mass of magnesium is 24.31 a.m.u. This magnesium is compound of 79 mole% of and remaining 21 mole % of and . Calculate mole% of .
1. 10
2. 11
3. 15
4. 16
Calculate the % of free in oleum (a solution of in ) that is labelled 109% .
1. 40
2. 30
3. 50
4. None
Suppose two elements X and Y combine to form two compounds and when 0.05 mole of weighs 5 g while 3.0111023 molecules of weighs 85 g. The atomic masses of x and y are respectively:
1. 20, 30
2. 30, 40
3. 40, 30
4. 80, 60
The impure 6 g of is dissolved in water and then treated with excess of silver nitrate solution. The weight of precipitate of silver chloride is found to be 14 g. The % purity of solution would be:
1. 95%
2. 85%
3. 75%
4. 65%
60 mL of a mixture of nitrous oxide and nitric oxide was exploded with excess of hydrogen. If 38 mL of was formed, calculate the volume of each gas in the mixture. All measurements are made at constant P and T.
1.20 ml +30 ml
2. 44 ml + 16 ml
3. 10 ml+40 ml
4 .25 ml +25 ml
The haemoglobin from the red blood corpuscles contains approximately 0.33% iron
by mass. The molar mass of haemoglobin is 67,200. The number of iron atoms in each molecule of haemoglobin is :
(atomic mass of iron=56):
1. | 2 | 2. | 3 |
3. | 4 | 4. | 5 |
Volume strength of 1 M solution of is:
1. 11.2 2. 22.4
3. 10.8 4. 21.6