Some basic concepts of chemistry practice · Mixed difficulty

Law of constant composition is same as the law of

Which one of the following is not a redox reaction

The Largest number of molecules is in

Any quantitative observation or measurement is represented by $A$ followed by $B$ in which it is measured. $A$ and $B$ respectively are

The number of significant figures in 10.3106 g is

One mole of mixture of $\mathrm{N}_2, \mathrm{NO}_2$ and $\mathrm{N}_2 \mathrm{O}_4$ has a mean molar mass of $55.4 \mathrm{~g}.$ On heating to a temperature, at which all the $\mathrm{N}_2 \mathrm{O}_4$ is dissociated into $\mathrm{NO}_2,$ the mean molar mass tends to a lower value of $39.6 \mathrm{~g}.$ What is the mole ratio of $\mathrm{N}_2, \mathrm{NO}_2$ and $\mathrm{N}_2 \mathrm{O}_4$ in the original mixture?

The oxidation number and covalency of sulphur in the sulphur molecule $\left( {{S_8}} \right)$ are respectively :

Assertion: Components of a homogeneous mixture cannot be separated by using physical methods.

Reason: Composition of homogeneous mixture is uniform throughout as the components react to form a single compound.

Choose correct option based on following statements. Here T stands for true statement and F for false statement.
(i) Homogeneous mixture has uniform composition throughout.
(ii) All components of a heterogeneous mixture are observable to naked eyes.
(iii) All solutions are homogeneous in nature.
(iv) Air is an example of heterogeneous mixture.

Statement-I: 12 parts by mass of carbon in $\mathrm{CO}$ and $\mathrm{CO}_2$ molecules combine with 16 and 32 parts by mass of oxygen.

Statement-II: A given compound always contains exactly the same proportion of elements by weight.

Which is not a redox reaction?

One mole electron means:

The number of Na atoms in 46 g ‘Na”

If Avogadro number ${\mathrm{N}_\mathrm{A}}$ , is changed from $6.022 \times {10^{23}}\,mo{l^{ - 1}}\,to\,6.022 \times {10^{20}}\,mo{l^{ - 1}}$ , this would change:

To neutralise 20 mL of M/ 10 NaOH, the volume of M/20 HCl needed is:

74.5 g of a metallic chloride contains 35.5 g of chlorine, the equivalent weight of the metal is

Assertion: Sulphate is estimated as $\mathrm{BaSO}_4$ and not as $\mathrm{MgSO}_4$.
Reason: Ionic radius of $\mathrm{Mg}^{2+}$ is smaller than $\mathrm{Ba}^{2+}$.

0.1 mole of a carbohydrate with empirical formula $\mathrm{C}{\mathrm{H}_2}\mathrm{O}$ contains 1 g of hydrogen. What is its molecular formula?

Irrespective of the source, pure sample, of water always yields 88.89% mass of oxygen and 11.11% mass of hydrogen. This is explained by the law of

Oxygen and the oxide ion have the

The equivalent weight of a metal is 9 and vapour density of its chloride is 59.25. The atomic weight of metal is

The value of gram molar volume of gas is:

The least count of an instrument is 0.01 cm. Taking all precautions, the most possible error in the measurement can be

One gram mole of a gas at NTP occupies 22.4 L. This fact was derived from

Equivalent weight of oxygen is:

Iron forms two oxides. If for the same mass of iron, the mass of oxygen combined in the first oxide is two-third of the mass of oxygen combined in the second oxide, then the ratio of valency of iron in first and second oxide is

Ratio in hydrogen and oxygen in water molecule by volume is

$M$ is the molecular weight of $\mathrm{KMn}{\mathrm{O}_4}.$ The equivalent weight of $\mathrm{KMn}{\mathrm{O}_4}$ when it is converted into ${\mathrm{K}_2}\mathrm{Mn}{\mathrm{O}_4}$ is :

Camphor is often used in molecular mass determination because

5 molar solution of ${H_2}S{O_4}$ is diluted from 1 litre to a volume of 10 litre, the normality of the solution will be