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Chemistry Test - 1
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Chemistry Test - 1

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  • Question 1/10
    1 / -0

    How many moles of magnesium phosphate Mg3(PO4)2 will contain 0.25 moles of oxygen atoms?

    Solutions

  • Question 2/10
    1 / -0

    How many moles of Na2S2O3 can be produced from 32 g of sulphur?

    Solutions

    Number of moles of sulphur = 32/32 = 1 mole

    One mole of Na2S2O3 will be obtained from 2 moles of sulphur.

    Mole of Na2S2O3 obtained from 1 mole of sulphur = ½ = .50 mole

  • Question 3/10
    1 / -0

    What is the approximate number of molecules in 4.25 g of NH3?

    Solutions

    Number of moles of ammonia = 4.25/17 = 0.25 mol

    Number of molecules in 0.25 mol of ammonia = 0.25 x 6.022 x 1023

     = 1.5 x 1023

  • Question 4/10
    1 / -0

    What volume of 0.1 M ethanol is required for the preparation of 5.6 g of C2H4 using concentrated H2SO4?

    Solutions

    46 g 28 g

    It is clear from the above equation that number of moles of ethene formed = Number of moles of ethanol used

    Number of moles of ethene formed = 5.6/28 = 0.2

    M = n/V

    V = n/M = 0.2/0.1 = 2 L

  • Question 5/10
    1 / -0

    What is the number of atoms in 100 amu of He? (Atomic weight of He is 4 u)

    Solutions

    Mass of 1 atom of helium = 4 amu

    So, in 100 amu, the number of helium atoms = 100/4 = 25 

  • Question 6/10
    1 / -0

    Which gas has the highest partial pressure in atmosphere?

    Solutions

    Nitrogen is present in largest amount in the atmosphere. So it has the highest partial pressure in the atmosphere.

  • Question 7/10
    1 / -0

    Ratio between r.m.s. velocity of hydrogen at 50 K and that of oxygen at 800 K is 

    Solutions

  • Question 8/10
    1 / -0

    Which of the following does not crystallise in the rock-salt structure?

    Solutions
    CsCL has body-centred cubical packing.
  • Question 9/10
    1 / -0

    The partial pressure of hydrogen in a flask containing 2 g of H2 and 32 g of SO2 is

    Solutions

    The partial pressure of A in a mixture of A and other gases is the total pressure multiplied by the mole fraction of A.

    In the present case,

    Mole fraction of hydrogen =1/(1+(1/2)) = 2/3

    The partial pressure of Hydrogen = 2/3 of total pressure

  • Question 10/10
    1 / -0

    The density of a gaseous substance at 1 atm pressure and 773 K is 0.4 g/l. If the molecular weight of the substance is 30 g, the forces existing among gas molecules are

    Solutions

    PV = ZnRT

    Here, n (number of moles)=mass(W) / molar mass(M)

    Then, PM=( W/V )ZRT

    PM = ZdRT (where, M is molecular mass and d is density) [W/V=d (density)]

    Substituting the values,

    (1)(30) = Z(0.4)(0.082)(773) 

    Z = 1.183 > 1

    Thus, forces are repulsive.

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