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Engineering
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40% of a mixture of 0.2 mole of N_{2} and 0.6 mole of H_{2} react to give NH_{3} according to the equation, N_{2} (g)+3H_{2}(g)\leftrightarrow 2NH_{3}(g) at constant temperature and pressure. Then the ratio of the final volume to the initial volume of gases is

  • Option 1)

    4:5

  • Option 2)

    5:4

  • Option 3)

    7:10

  • Option 4)

    8:5

 
As learnt in Law of Chemical equilibrium - At a given temperature, the product of concentration of the reaction products raised to the respective stoichiometric coefficient in the balanced chemical equation divided by the product of concentration of the reactants raised to their individual stoichiometric coefficients has a constant value. - wherein are equilibrium concentration    The...
Engineering
185 Views   |  

36g of glucose, C6H12O6 ,is dissolved in 1kg of water in a saucepan. temperature at which water will boil at 1.013 bar? Kb for water is 0.52 kg/mole

  • Option 1)

    373.008K

  • Option 2)

    373.202 K

     

     

  • Option 3)

    373.254K

  • Option 4)

    below 373K

 
As we learned in concept Mathematical Expression - Unis of   - wherein       Water boils at 373.15 K at 1.013 bar pressure T = 373.15 + 0.104 = 373.254 K Option 1) 373.008K This option is incorrect. Option 2) 373.202 K     This option is incorrect. Option 3) 373.254K This option is correct. Option 4) below 373K This option is incorrect.
Engineering
2286 Views   |  

3.2 mole of iodide were heated in a sealed bulb at 444 degree C till the equilibrium was reached. The degree of dissociation of HI at this temperature was found to be 22% . The number of moles of hydrogen iodide present at equilibrium are :

  • Option 1)

    2.496

  • Option 2)

    1.87

  • Option 3)

    2.00

  • Option 4)

    4.00

 
As we learned in concept Law of Chemical equilibrium - At a given temperature, the product of concentration of the reaction products raised to the respective stoichiometric coefficient in the balanced chemical equation divided by the product of concentration of the reactants raised to their individual stoichiometric coefficients has a constant value. - wherein are equilibrium...
Engineering
85 Views   |  

28 g N2 and 6 g H2 were mixed. At equilibrium 17 g NH3 was formed. The mass of N2 and H2 of equilibrium are 

  • Option 1)

    11 g , zero

  • Option 2)

    1 g , 3 g

  • Option 3)

    14 g , 3 g

  • Option 4)

    11 g , 3 g

 
As we learned in concept Law of Chemical equilibrium - At a given temperature, the product of concentration of the reaction products raised to the respective stoichiometric coefficient in the balanced chemical equation divided by the product of concentration of the reactants raised to their individual stoichiometric coefficients has a constant value. - wherein are equilibrium...
Engineering
82 Views   |  

1gm of non-electrolyte solute disolved in 50gm of benzene lowered the freezing point of benzene by 0.4 K. Freezing point depression constant of benzene is 5.12 K Kg/mol. Molar mass of solute is  

  • Option 1)

    252 g/mol

  • Option 2)

    256g/mol

  • Option 3)

    262 g/mol

  • Option 4)

    356 g/mol

 
As we discussed in concept Mathematical Expression of Depression in Freezing point -   - wherein m = molarity of solvent  = cryoscopic  constant     molal depress const Units =    We know that 0.4 = 5.12 x m where m = molality of solute  = Molecular weight = Option 1) 252 g/mol This option is incorrect. Option 2) 256g/mol This option is correct. Option 3) 262 g/mol This option is...
Engineering
381 Views   |  

100ml of 1N NH4OH (Kb=5x10-5) is neutralized to equivalence point by 1N HCl. The PH of solution at equivalence point is

  • Option 1)

    2

  • Option 2)

    2.5

  • Option 3)

    3

  • Option 4)

    5

 
As we discussed in concept Buffer Solutions - The solutions which resist change in pH on dilution or with addition of small amounts of acid or alkali are called buffer solution.   - wherein Many body fluids  e.g.  blood    pH in case of strong acid and a weak base at equivalence point is given by        =       = Option 1) 2 This option is incorrect. Option 2) 2.5 This option is...
Engineering
473 Views   |  

10 ml of a solution contains 0.1M NH4Cl + 0.01M  NH4OH. Which addition would not change the PH of the solution? 

  • Option 1)

    Adding 1ml water 

  • Option 2)

    Adding 5ml of 0.1M NH4Cl

  • Option 3)

    Adding 5ml of 0.1M NH4OH

  • Option 4)

    Adding 10ml of 0.1NH4Cl

 
As we discussed in concept Buffer Solutions - The solutions which resist change in pH on dilution or with addition of small amounts of acid or alkali are called buffer solution.   - wherein Many body fluids  e.g.  blood    pOH of a buffer solution = pH = 14 - pOH Adding 1ml of water would not affecr the concentration of salt or base as much as to make a change in pH of the solution. That is...
Engineering
1121 Views   |  

0.2 moler solution of formic acid is 3.2% ionized. Its ionization constant is 

  • Option 1)

    9.6x10-3

  • Option 2)

    2.1x10-4

  • Option 3)

    1.25x10-6

  • Option 4)

    4.8x10-5

 
As we discussed in concept Ionization constant of weak acids - Consider    - wherein         Ionization constant                                                          =                                 Option 1) 9.6x10-3 This option is incorrect. Option 2) 2.1x10-4 This option is correct. Option 3) 1.25x10-6 This option is incorrect. Option 4) 4.8x10-5 This option is incorrect.
Engineering
99 Views   |  


What molar concentration of NHprovides a[OH-] of 1.5x10-3? (Kb=1.8x10-5)

  • Option 1)

    0.125m

  • Option 2)

    (0.125+1.5x10-3)

  • Option 3)

    (0.124-1.5x10-3)m

  • Option 4)

    (1.5x10-3)m

 
As we discussed in concept Value of Kb - - wherein    The reaction goes as follows   We know that Option 1) 0.125m This option is correct. Option 2) (0.125+1.5x10-3) This option is incorrect. Option 3) (0.124-1.5x10-3)m This option is incorrect. Option 4) (1.5x10-3)m This option is incorrect.
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