Chapter wise 1 jee

1. 29.2 % (w/w) HCl stock solution has a density of 1.25 g mL^–1. The molecular weight of HCl is 36.5 g mol^–1. Find the volume of (mL) of stock solution required to
prepare a 200 mL solution of 0.4 M HCl 

2. A ball of mass 100 g is moving with 100 ms^–1. Its wavelength is x x 10^-25 A. Value of x to closest integer is

3. Statement 1: The principal quantum number, n, can have whole number values 1, 2, 3, … etc.
Statement 2: The angular momentum quantum number can never be equal to n.

4. Find the value of n in the molecular formula Be_nAl₂Si₆O₁₈

5. Which of the following statement is incorrect about the characteristics of cathode rays?

6. The maximum number of electrons that can have principal quantum number, n = 3 and spin quantum number, m_s =-1/2 is

7. Match the expressions/statements in Column I with expressions/Statements in Column II.

Match the columns according the Boh’s theory.
8. E_n = Total energy
K_n = Kinetic energy
V_n = Potential energy
n_r = Radius of n^th orbit

9. Match the following type of rays given in Column I with their characteristics given in Column II. Select an appropriate answer from the codes given below.

10. What is the maximum number of electrons that may be present in all the atomic orbitals with principal quantum number 3 and azimuthal quantum number 2?

11. On bombarding a beam of α-particles on the atom of the gold sheet, few particles get deflected, whereas most of them go straight and remains undeflected. This is due to

12. When zinc reacts with dilute nitric acid, nitrous oxide is produced. What mass of the gas is evolved by treating 325 g zinc with excess of nitric acid?

13. Chlorine exists in two isotopic forms, Cl-37 and Cl-35 but its atomic mass is 35.5. This indicates the ratio of Cl-37 and Cl-35 is approximately.

14. Statement 1: The Paschen series in the spectrum of hydrogen lies in the infra-red region.
Statement 2: The Paschen series is born of transition of electrons onto the second orbit from higher orbits.

15. What is the work function of the metal, n the light of wavelength 4000 Å generates photoelectron of velocity 6 x 10⁵ m s ^-1 from it? 
(Mass of electron = 9 x 10^-31 kg, Velocity of light = 3 x 10⁸ m s^-1, Planck’s constant = 6.626 x 10^-34 Js, Charge of electron = 1.6 x 10^-19 JeV^-1)

16. What is the concentration of sugar (C₁₂H₂₂O₁₁) mol L^-1 if its 20 g are dissolved in enough water to make a final volume up to 2 L in mol L^-1?

17. Statement I: The ground state configuration of Cr is 3d⁵ 4s¹.
Statement II: A set of exactly half-filled orbitals containing parallel spin arrangement provide extra stability.

18. CH_{4 (g)} + 2 O_{2 (g)} → CO_{2 (g)}+ 2H₂O_(g)
According to the above chemical reaction, following information have been given.
(i) One mole of CH_{4 (g)} reacts with two moles of O_{2 (g)}to give one mole of CO_{2 (g)} and two moles of H₂O_(g)
(ii) One molecule of CH_{4 (g)} reacts with 2 molecules of O_{2 (g)} to give one molecule of CO_{2 (g)} and 2 molecules of H₂O_(g)
(iii) 22.7 L of CH_{4 (g)} reacts with 45.4 L of O_{2 (g)} to give 22.7 L of CO_{2 (g)} and 45.4 L of H₂O_(g)
(iv) 16 g of CH_{4 (g)} reacts with 2 32 × g of O_{2 (g)} to give 44 g of CO_{2 (g)} and 2 18 × g of H₂O_(g)
From this information the correct interconversion should be

19. Statement I: p-orbital has dumb-bell shape. Because
Statement II: Electrons present in p-orbital can have one of three values for ‘m’, i.e., 0, +1, –1.

20. 25 g of an unknown hydrocarbon upon burning produces 88 g of CO₂ and 9 g of H₂O. This unknown hydrocarbon contains.

21. Match the entries in column I with the related entries in Column II

22. Among the following, what is the number of elements showing only one non-zero oxidation state? O, Cl, F, N, P, Sn, Tl, Na, Ti

23. Ethanol-water mixture has 46 g ethanol in 100 g mixture. By a suitable technique volatile component goes off. Thus

24. Arrange the following in the order of increasing mass (Atomic mass of O = 16, Cu = 63 and N = 14).
I. One atom of oxygen
II. One atom of nitrogen
III. 1 x 10^-10 mole of oxygen
IV. 1 x 10^-10 mole of copper

25. Statement I: Nodal plane of p_x atomic orbital in yz plane.
Statement II: In p_x, atomic orbital electron density is zero in the yz plane.

26. Consider the following laws of chemical combination with examples.
I. Law of multiple proportion: N₂O, NO, NO₂.
II. Law of reciprocal proportion: H₂O, SO₂, H₂S.
Which is correct with example?

27. Match the entries in column I with the related quantum number(s) in Column II

28. An element has mass number of 23 and its unipositive ion has electronic configuration 1s² 2s² 2p⁶. Select the correct statement(s).
(I) It is isotonic with Mg²⁴.
(II) The ratio of n to l for last electron in atom of above element is 2.
(III) Atom of the above element is isoelectronic with H₂O.
(IV) Atom of the above element is paramagnetic.

29. Mole fraction of the solute in a 1.00 molar aqueous solution is?

Select the correct statement(s).
(I) Maximum number of electrons having 30. 12 s = +1/2 in Sulphur is 9.
(II) If electron has zero magnetic quantum number, then it must be present in s-orbital.
(III) All isoelectronic ions have same value of Z_eff.
(IV) Number of subshell present in a nth shell is equal to ‘n’.