The chemical equation below shows the decomposition of ammonium nitrate (nh4no3).

nh4no3 -> n2o + 2h2o

a chemist who is performing this reaction starts with 160.1 g of nh4no3. the molar mass of nh4no3 is 80.03 g/mol; the molar mass of water (h2o) is 18.01 g/mol. what mass, in grams, of h2o is produced?

a)9.01
b)18.01
c)36.03
d)72.06

 The mass  in grams  of H₂O  is 72.04  grams  which  is  around (answer D)

Calculation

Step 1 :  calculate the moles of NH₄NO₃

moles  =  mass/molar  mass

 =160.1 g / 80.03  g /mol =  2 moles

Step  2: use the mole  ratio to calculate the  moles of H₂O

NH₄NO₃:H₂O  is 1:2  therefore the moles of H₂O  is  

= 2 moles x 2 = 4 moles

Step 3: calculate the mass of  H₂O

mass = moles  x molar mass

= 4  moles  x 18.01 g/mo= 72.04 grams  approximate   (answer D)

the mass of the cathode increases because ions from the solution get reduced to atoms and become part of the cathode.

explanation:

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