Acompound that contains both potassium and oxygen formed when potassium metal was burned in oxygen gas. the mass of the compound was 7.11 grams. the mass of the potassium metal was 3.91 grams. what mass of oxygen was involved in this reaction? justify your answer.

             3.2 g of O₂

Solution:
             This reaction is for the formation of Potassium Superoxide, The reaction is as follow,

                                           K  +  O₂     →     KO₂

First let us confirm that either the given amount of Potassium produces the given amount of Potassium oxide or not,
So,
As,
                39.098 g (1 mole) K produced  =  71.098 g of K₂O
So,
                          3.91 g of K will produce  =  X g of K₂O

Solving for X,
                      X  =  (3.91 g × 71.098 g) ÷ 39.098

                      X  =  7.11 g of K₂O

Hence, it is confirmed that we have selected the right equation,
So,
As,
                     39.098 g of K required  =  32 g of O₂
So,
                     3.91 g of K will require  =  X g of O₂

Solving for X,
                     X  =  (3.91 g × 32 g) ÷ 39.098 g

                     X  =  3.2 g of O₂

Atomicity occurs to prevent updates of the database occurring only partially, which can cause greater problems than rejecting the whole series outright.some are monatomic, diatomic, triatomic etc because it shows the number of atoms. for example, monatomic means it contains only one atom.

Yes, endothermic means it turns cold. and some chemical changes include change of tempature.