5. Express the followings as the power of 10:
7. Round off the following number into (a) Four significant figures (b) three significant figures (c)Acetic acid contains002021010 two significant figures
8. acidic acid contains carbon, hydrogen and oxygen. 4.24 g sample of acetic on complete combustion gave 6.21 g of CO2 and 2.54 g of H2O. the molecular mass of acetic acid is 60. find(i) empirical formula of acetic acid and (ii) molecular formula of acetic acid
9. Ethylene glycol is used as an anti freeze. combustion of 6.38 mg of ethylene glycol gives 9.06 mg of CO2 and 5.58 mg of H2O. Ethylene glycol contains carbon, hydrogen and oxygen and its molecular mass is 62. Find empirical formula and molecular formula.
10. When dinitrogen pentoxide ( N2O5), a white solid is heated,. it decomposes to nitrogen dioxide and oxygen.
2N2O5 ------ 4NO2(g) + O2(g)
Find the volume of NO2 and O2 gases produced at S.T.P when a sample
of 54g of N2O5 is heated.
11. Hydrogen cyanide is prepared from ammonia, air and natural gas ( CH4) by the following process
If a reaction vessel contains 51 g of NH3 • What is the maximum mass of
HCN that could be made, assuming the reaction goes to completion? Find also the volumes of O2 and CH4 gases required for the reaction at S.T.P.
12.Ammonia gas can be produced by heating together the solid NH4Cl and Ca(OH)2, If a mixture containing 100 gm of each of this solid s is heated.How many grams of NH3 are produced? also find the volume of
NH3 gas at S.T.P.
2NH4Cl + Ca( OH)2 ➔ 2NH3 + CaCl2+ 2H2O
7. 1.40 dm3 volume of a gas measured at a temperature of 27°C and a pressure of 900 torr was found to have mass 2.273 g. Calculate the molecular mass of the gas [Hint: Calculate "n" by the formula PV=nRT and then molecular mass]
8. A 12.5 dm3 vessel contains 4.0 g CH3 1.8 g N2 and 10.0g Xe. What is the pressure in the vessel at 0°C?(Hint: Find out the total moles of the gases and then apply PV = nRT).
9(a) State and explain the Graham's law of Diffusion.
(b) Compare the rates of diffusion of the following pairs of gases: (i) H2 and D2 (ii) CH3 and He (iii) SF6 and SO2
12. Four containers of equal volume are filled as follows:
(i) 2.0g H2 at O°C (ii) 1.0g H2 at 273°C (iii) 24 g O2 at O°C (iv) 16 g CH3 at 273°C.
Which container (a) is at the greatest pressure (b) is at the lowest pressure.
22. 40 dm3 of hydrogen gas was collected over water at 831 torr Hg pressure at 23°C. What would be the volume of dry hydrogen gas at standard conditions ? The vapour pressure of water at 23°C is 21 torr of Hg.
23. What is the density of methane gas (CH3) at 127°C and 3.50 atmosphere.
CHAPTER NO.3 : THE ATOMIC STRUCTURE
CHAPTER NO.4 : CHEMICAL BONDING
4 (a)State and explain Hess's law of constant heat summation Give its applications.
(b) Calculate the heat of formation of acetic acid from the following data.
i) 2C. + 2H, +O2 == CH3COOH H= ?
ii) C + O2 == CO2 H = -394 KJ/mole
iii) H2 + 1/2O2 == H2O= -286 KJ/mole
iv) CH3COOH + 20,2 == 2CO2 + 2H2O H = -870.8 KJ/mole
5. (a) Define and explain the terms (i) Exothermic process (ii) Endothermic process (iii) Heat of formation.
(b) Calculate the heat of formation of Ethane at 25°C from the following data
(i) 2C + 3H2 == CH3 H =?
(ii) C+ 02 == CO2 H = -394.00 KJ/mole
(iii) H2 + 1/2 O2 == H2O H = -286.0 KJ/mole
(iv) C2H6 + 7/2 O2 == 2C02 +3H2O H= -1560.632 KJ/mole
6.(a) Show that the product of pressure and volume, PV has the dimension of energy.
(b) In a certain process 848J of heat is absorbed by a system, while 394 J of work is done on the system. What is the change in the internal energy for the process ?
7.(a) If 1800 cals, of heat is added to a system while system does work equivalent to 2800 cals by expanding against the surrounding. What is the value of E for the system?
(b) In a certain process, 500J of work is done on a system which gives of 200J of heat. What is the value of E for the process ?
6. A quantity of PCl, was heated in a 12 dm3 vessel at
250°C. PCI, == PCI, + Cl, At equilibrium, the vessel contains 0.21 mole
PCl,0.32 mole PCl, and 0.32 mole Cl2. Compute the equilibrium constant Kc.
8.
One mole of HI is introduced into a vessel held at constant temperature. When
equilibrium is reached, it is found that 0.1 mole of I, have been formed.
Calculate the equilibrium constant Kc
12. When 1 mole of pure ethyl alcohol
(C2H5OH) is mixed with 1 mole of acetic acid (CH3 COOH) at room temperature,
the equilibrium mixture contains 3/2, mole each of ester (CH3 COOC2H5) and
water. (a), What is the equilibrium constant Kc (b) how many moles of ester are
formed at equilibrium when 3 moles of alcohol are mixed with 1 mole of acid?
All substances are liquids at room temperature.
13. PCI5 = PCI3 + Cl,.
Calculate the number of moles of Cl, produced at equilibrium when one mole of
PCI5 is heated at 250°C in a vessel having a capacity of 10 dm3. At 250°C, Kc =
0.041 for the dissociation.
14 (b) To determine the value of Kc for the
reaction CH3COOH, + C2H5 OH = CH3COOC2H5 + H2O, 1 mole of CH3 COCH and 1 mole
of C2H5OH in 1 dm3 of solution in an inert solvent containing a small amount of
acid catalyst were warmed until no further change occurred. At equilibrium,
0.667 mole of water was present. Calculate the value of Kc.
16 (b) What is the
solubility of lead chromate in moles per dm3 at 25°C. K,, for PbCrO4=2.8x10-13
mole/dm3.
17.(a) Will Cadmium hydroxide precipitate from 0.01M solution of
CdCl, at pH 9. Kc of Cd(OH),=2.5x10-14 mole/dm3.
(b) The solubility of Mg (OH)2
at 25°C is 0.00764 g/dm3. What is the solubility product of Mg (OH)2?
(Kc=9.0x10-12 mole2/dm3)
CHAPTER NO.7 : SOLUTIONS AND ELECTROLYTES
CHAPTER NO.8 : INTRODUCTION TO CHEMICAL KINETICS
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