11.2 L of gas at STP Weight 14g. The gas would be from Chemistry

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 Multiple Choice QuestionsMultiple Choice Questions

271.

The number of atoms in 0.1 moles of a triatomic gas is (NA = 6.02 x 1023 mol-1)

  • 6.026 x 1022

  • 1.806 x 1023

  • 3.600 x 1023

  • 3.600 x 1023

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272.

10 g of hydrogen and 64 of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be


  • 2 mol

  • 3 mol

  • 4 mol

  • 4 mol

422 Views

273.

Number of moles of MnO4- required to oxidies one mole of ferrous oxalate completely in acidic medium will be 

  • 0.6 mole

  • 0.4 mole

  • 7.5 mole

  • 7.5 mole

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274.

An Organic compound contains carbon, hydrogen and oxygen. Its elemental analysis gave C, 38.71% and H, 9.67%. The empirical formula of the compound would be

  • CH3O

  • CH2O

  • CHO

  • CHO

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275.

How many moles of lead (II) chloride will be formed from a reaction between 6.5 g of PbO and 3.2 g of HCl?

  • 0.044

  • 0.333

  • 0.011

  • 0.011

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276.

An element, X has the following isotopic composition;


200X: 90%

199X : 8.0%

202X ; 2.0 %

The weighted average atomic mass of the naturally -occurring element X is closet to:

  • 200 amu

  • 201 amu

  • 202 amu

  • 202 amu


277.

Work is being performed, when a weight lifter lifts a base ball off a weight rack. This is due to

  • magnetic attraction

  • gravity

  • electrostatic repulsion

  • mechanical force


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278.

11.2 L of gas at STP Weight 14g. The gas would be

  • H2

  • CO

  • B2H6

  • All of these


D.

All of these

Molecular weigth of gas = 14 × 22.411.2 = 28

The above formula denotes the formula of mole concept. The gas would be CO, N2, B2H6.


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279.

For preparing 3.00 L of 1M NaOH by mixing portions of two stock solutions (A and B) of 2.50 M NaOH and 0.40 M NaOH respectively. Find out the amount of B stock solution (in L) added.

  • 8.57 L

  • 2.14 L

  • 1.28 L

  • 7.51 L


280.

What would be the heat released when an aqueous solution containing 0.5 mole of HNOis mixed with 0.3 mole of OH-?  (enthalpy of neutralisation is- 57.1 kJ)

  • 28.5 kJ

  • 17.1 kJ

  • 45.7 kJ

  • 1.7 kJ


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