Chemistry Intermediate Part I
(Ch. # 8+9+10+11)
1. The cryoscopic constant of water is 1.86oC.
The elevation of B.P. for a 0.1 m solution of a solute in water is:
a.
18.6 oC b. 1.86oC c. 0.186oC d-
sufficient data not given
2. Freezing point of equimolal aqueous solutions will be
minimum for:
a. Fructose b.
Urea C. Glycose d- NH4Cl
3. 3.42 g of sucrose and 1.8 g of glucose
in 100 g of H2O separately have the elevation of boiling point as 0.052oC.How
much quantity of urea in 100 g of H2O is required to have the same
effect:
a. 1.2 g b. 0.6 g c.1.8
g d. 10.1 g
4. If more solvent is added to solution, the value of heat of
solution:
a. increases b- decreases c.
is not affected
d. is affected
only when the solution is infinitely diluted.
5. Which one of the following substance when dissolved in water
give acidic solution:
a. NaCl b. Na2SO4 C. NH4Cl d- CH3COONH4
6. 2NO+O2 ® 2NO2
is
a. 1st order b. 2nd
order c. 3rd order d. zero order
7. In zero order reaction, the rate is
independent of
a. temp of reaction b- concentration of reaction
c. concentration of product d. Non of these
8. The unit of rate const. is same as that
of the rate of reaction
a. first order reaction b. 2nd order reaction
c. zero order reaction d. 3rd order reaction
9. Rate of endothermic reaction ___________
with increase in temp.
a. increases b. decreases C.
Never change d- Non of these
10. Arrhenius eq. can be used to find out
________ of reaction.
a. energy of
activation b. order of reaction
c- possibility
of reaction d- Non of them
11. Fe3+ ® Fe2+
is a
(a) oxidation
reaction b. reduction reaction
c. oxidation reduction d. reverse reaction
12. Stronger the oxidizing agent, greater is
the
(a) oxidation potential b. reduction potential
c. redox potential d. E.M.F. of cell
13. Which of the following statement is
correct about galvanic cell?
a. Anod
negatively charged b-
reduction occur at anode
c. cathode is +vely charged d.
reduction occur at cathode
14. What is SHE
(a) standar
Hydrogen Electrod b. standard helium
electrode
c. standard high energy electrod d. None of them
15. Reduction is
a. gain of electron b. loss of electron
c. gain and loss of electron d. All of them
Total
Marks:70 Subjective Time:2:30
minutes
Section
– I
Q.2. Attempt All Short Questions: 20 x 2 = 40
1. How do you justify that boiling
points of solvents increase in the presence of solutes.
2. Give cathodic anodic reactions for the
electrolysis of aqueous NaCl.
3.
Beckmann thermometer is used to note the depression in freezing point.
4. How electrochemical series is helpful
in calculating the emf of cells.
5. Give rodox reactions of alkaline
battery.
6. Give
redox reactions of silver oxide battery.
7. Na
& K can displace hydrogen from acids but PtPd & Cu cannot! Why?
8. Impure Cu can be purified by
electrolytic process.
9. Give redox reactions of Nickel cadmium
cell.
10. How is Al anodized in n electrolytic
cell.
11. The radioactive decay is always a first
order reaction.
12. Calculate the molarity of glucose when 9g
of it are dissolved in 250cm3 of solution.
13. Relative lowering of vapour pressure is
independent of temperature.
14. A very small amount of a catalyst may
prove sufficient to carry out a reaction.
15. What are second order reactions.
16. The concentration in terms of molality
is independent of temperature but molarity depends upon temperature.
17. What is instantaneous rate of a
reaction.
18. What is the effect of temperature on the
activity of a catalyst.
19. What are pseudo first order
reaction.
20. Non-ideal solutions don’t obey
Raoult’s law
Section – II
Attempt any three
Questions 10 x 3 = 30
Q.No.3 (a) The equilibrium constant for the
reaction between acetic acid & ethyl alcohol is 4.0 A mixture of 3 moles of
acetic acid & 1 mole of ethyl alcohol is allowed to come to equilibrium.
Calculate the amount of ethyl acetate at equilibrium stage. Also calculate the
masses of reactants left behind.
(b) The solubility
product of Ag2CrO4 is 2.6 x 10-2 at 25oC.
Calculate the solubility of the compound.
Q.No.4. (a)
What are azeotropic mixtures? Explain them with the help of graphs.
(b)
Balance the following equation by oxidation number method
Q.No.5. (a)
Explain collision theory & energy of activation.
(b) Give four industrial
applications of electrolysis.
Q.No.6. (a)
What are conjugate solutions. Explain the effect of temperature on phenol-water
system.
(b) What is the function
of a catalyst. Differentiate between homogeneous & heterogeneous catalysis.
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