HSC Science (Electronics) १२ वीं कक्षा - Maharashtra State Board Important Questions for Chemistry

If the total volume of a simple cubic unit cell is 6.817 × 10^-23 cm³, what is the volume occupied by particles in the unit cell?

Calculate the number of unit cells in 0.3 g of a species having density of 8.5 g/cm³ and unit cell edge length 3.25 × 10^-8 cm.

Calculate the packing efficiency for bcc lattice.

The unit cell of Na is bcc and its density is 0.97 g/cm³. What is the radius of a sodium atom if the molar mass of Na is 23 g/mol?

Derive the relationship between density of substance, its molar mass, and the unit cell edge length. Explain how you will calculate the number of particles, and a number of unit cells in x g of metal.

The coordination number of atoms in body-centred cubic structure (bcc) is ______.

Write the consequences of Schottky defect with reasons.

Explain metal deficiency defect with examples.

Aluminium crystallises in a cubic close-packed structure with a unit cell edge length of 353.6 pm. What is the radius of Al atom? How many unit cells are there in 1.00 cm³ of Al?

An element has a bee structure with unit cell edge length of 288 pm. How many unit cells and number of atoms are present in 200 g of the element?

Name a compound where Frenkel defect is found.

The relation between the radius of the sphere and the edge length in the body-centred cubic lattice is given by the formula ______.

Explain the following term:

Substitutional impurity defect

Explain the following term:

Interstitial impurity defect

Silver crystallizes in the fcc structure. If the edge length of the unit cell is 400 pm, calculate the density of silver (Atomic mass of Ag = 108).

The number of particles present in Face Centred Cubic Unit cell is/are ______.

Predict the type of cubic lattice of a solid element having edge length of 400 pm and density is 6.25 g/ml.
(Atomic mass of element = 60)

Write the formula to determine the molar mass of a solute using freezing point depresssion method.

Why is molality of a solution independent of temperature?

1.0 x10^-3Kg of urea when dissolved in 0.0985 Kg of a solvent, decreases freezing point of the solvent by 0.211 k. 1.6x10 Kg of another non-electrolyte solute when dissolved in 0.086 Kg of the same solvent depresses the freezing point by 0.34 K. Calculate the molar mass of the another solute. (Given molar mass of urea = 60)