Question

1. g of Mg is burnt with 0.56g of oxygen in a closed vessel. which reactant is let and how much?
AND PLEASE ANSWER WISELY AND HONESTLY PLSSSSSSSSSSSSSSSSS!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!

Answer 1

No . of moles of 1g Mg = 1/ 24 =0.04 moles

No. of moles of O2 = 0.56/32= 0.0175 moles

Oxygen has less no. of moles

Answer 2

The equation is as follows:

2Mg + O2  ------>  2MgO

(s)      (g)                (s)

Therefore 2 moles of Mg require 1 mole of O2 to produce 2 moles of MgO.

Calculate actual moles.

moles= mass/ molar mass

Mg=    1/24  = 0.041667

O2=   0.56/32 = 0.0175

MgO=

Mole ratio of Mg: O2   = 2:1

find mass of Mg that reacts:

that means 2 mole of Mg reacts with 1 moles of O2

If 1 = 2 

Then 0.0175 = 0.0175 x 2

                     =0.035 moles of magnesium

mass of magnesium that reacts:

mass= moles x molar mass

        = 24 x 0.035

         

              0.84 g

That means that of the 1 gram of magnesium that reacts only 0.84 grams is used

Therefore magnesium is in excess and by 0.16

plz follow me and mark as brainliest