Gasoline is produced from crude oil, a nonrenewable resource. ethanol is mixed with gasoline to produce a fuel called gasahol. calculate the mass of water produced when 100.0 g of ethanol, c2h5oh, is burned in 82.82 g of oxygen.

              46.58 g of H₂O

The Balance Chemical Equation is as follow,

                            C₂H₅OH  +  3 O₂     →      2 CO₂  +  3 H₂O

Step 1: Calculate the Limiting Reagent,

According to Balance equation,

               46.07 g (1 mol) C₂H₅OH reacts with  =  96 g (3 mol) of O₂

So,

                   100 g of C₂H₅OH will react with  =  X g of O₂

Solving for X,

                       X  =  (100 g × 96 g) ÷ 46.07 g

                       X  =  208.3 g of O₂

It means 100 g of C₂H₅OH requires 208.3 g of O₂, while we are provided with 82.82 g of O₂ which is less than required. Therefore, O₂ is the limiting reagent and will control the yield of products.

Step 2: Calculate amount of Water produced,

According to equation,

                96 g (3 mol) of O₂ produces  =  54 g (3 mol) of H₂O

So,

                        82.82 g of O₂ will produce  =  X moles of H₂O

Solving for X,

                      X  =  (82.82 g × 54 mol) ÷ 96 g

                     X  =  46.58 g of H₂O

the atomic number will stay the same no matter how many electrons it has, so it doesn’t decrease nor increase. it’ll only change with a different number of protons