Based on the following balanced equation- how many grams of zinc oxide could be generated from 1.75 miles of zinc sulfide assuming there was excess oxygen?
c = 12.01, o = 16.00, zn = 65.38 (g/mol)

mass of ZnO = 95.62 g  

Explanation:

Balanced chemical equation  

       2ZnS + 3O₂ → 2ZnO  + 2SO₂

Given data from eq.

     moles of zinc sulfide = 2 mol  

     moles of zinc oxide = 2 mol  

     mass of zinc oxide = ?

     Given moles of   zinc sulfide = 1.75 mol

Solution  

1st we will find out the mole ratio of zinc sulfide and zinc oxide from balanced chemical equation  

          ZnS : ZnO

               2 : 2

            2/2 : 2/2

                 1 : 1  

given number of moles of zinc sulfide = 1.75 mol

So we can find out moles (x) of ZnO  needed for 1.75 mol of zinc sulfide  

from the balanced chemical equation the mole ratios are:  

               1 : 1  

          1.75 : x  

Cross multiply these ratios  

        1 × 1.175 = 1x  

             1.175 = 1 x  

             x = 1.175 mol  

Now we will find out the mass of ZnO

    mass = moles × molar mass  

    mass of ZnO = 1.175 mol × 81.38 g/mol  

    mass of ZnO = 95.62 g  

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.