Question

Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 4.25 g of magnesium ribbon burns with 8.15 g of oxygen, a bright, white light and a white, powdery product are formed Enter the balanced chemical equation for this reaction. Be sure to include all physical states. equation: 2Mg(s) +02(g) 2MgO(s) What is the limiting reactant? охуgen magnesium If the percent yield for the reaction is 82.2%, how many grams of product were recovered? mass of product recovered:5.8 g How many grams of the excess reactant remain? mass of excess reactant: g со

Answer 1

Ans weight of Mg = 1.25gm weight of Oz = 8.159m Mole o Ma: 4.25 - 24 0.177 mole Mac: given weight Morce Mass Mole of O2 = 8.15 - = 0.254 Mele 32 - 2MgO (3) 2 Mges + 0.177 O2 (s) 0.254 Mole mg is a limiting Reagent, because it will consume first in the given Chemical Reaction. 2 i Mole Mgo is used mole Mge is used to form 2 to form more of Mgo I more of Mo 0.177 mole of mg is used to form 0.177 more of myo it yield percentage is 82.2% then mole of Product is mere of Mgo Produced = de? * 0.177= 0.145 moie Mass of Product = 0.145 * 40 = S ym 1 Mgo have molar) mass = 40 Mole of excess Reagent (oz) left = 0.254 – (0.17) = 0.254-0.0885 = 0.165 molie mass of Oz left = 0.165x 32= 5.29 gm.