How many grams of NO2 are needed to form 88.0 g of HNO3?

64.4g

Explanation:

The chemical reaction that will produce HNO₃ from NO₂ is given below:

        3NO₂  +  H₂O →  2HNO₃  + NO

Given;

Mass of HNO₃  = 88g

  Now;

To solve this problem, find the number of moles of HNO₃;

  Number of moles  =  

      Molar mass of HNO₃ = 1 + 14 + 3(16) = 63g/mol

 Number of moles  =   = 1.40mol

From the balanced reaction;

    2 mole of HNO₃ is produced from 3 mole of NO₂

   1.4 mole of HNO₃ will be produced from   = 2.1mole of NO₂  

Mass of NO₂ = number of moles x molar mass

  Molar mass of NO₂ = 14 + 2(16) = 46g/mol

  Mass of NO₂ = 1.4 x 46  = 64.4g

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the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be