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

answer is: c. the experiment shows that the red substance experienced a chemical change.

this is chemical change (chemical reaction), because two new substances are formed (metalig liquid and gas), the atoms are rearranged and the reaction is followed by an energy change.

this is example of chemical decomposition.

chemical decomposition (analysis) is the separation of a single chemical compound into its two or more elemental parts or to simpler compounds.  

chemical decomposition is opposite of chemical synthesis.