Balance the chemical equation given below, and determine the number of grams of MgO that are needed to produce 20.0 g of Fe2O3. MgO(s) Fe(s) Fe2O3(s) Mg(s)

1.) The balanced equation is    3MgO(s) +  2Fe(s) ===> Fe2O3(s) + 3Mg(s)

2.) 20g of Fe2O3 will be produced by 20 ×120/160 = 15g of MgO

Explanation:

THE CORRECT EQUATION IS: MgO(s) + ___ Fe(s)  ===> Fe2O3(s) + ___ Mg(s)

The balanced equation is: 3MgO(s) +  2Fe(s) ===> Fe2O3(s) + 3Mg(s)

molar mass of 3MgO = 3(24 + 16) = 120

Molar mass of Fe2O3 = 2 X 56 + 3 X 16

                                    =112 +48 =160

From the equation, 120g of MgO Produced 160g of Fe2O3

Therefore 20g of Fe2O3 will be produced by 20 ×120/160 = 15g of MgO.

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.