Determine the theoretical yield for the reaction. Express your answer in grams C

Question

Determine the theoretical yield for the reaction. Express your answer in grams Constants I Periodic Table You may want to reference (Pages 131 -137) section 4.3 while completing this problem. Magnesium oxide can be made by heating magnesium metal in the presence of the oxygen. The balanced equation for the reaction is 2Mg(s) + O2()2Mgo(s) Submit When 10.0 g Mg is allowed to react with 10.4 g O2. 12.1 g MgO is collected Part C Determine the percent yield for the reaction Express your answer as a percent 2

Explanation / Answer

Molar mass of Mg = 24.3 g/mol

10 g / 24.3 g/mol => 0.4115 mol of Mg

Molar mass of O2 = 32 g/mol

10.4 g / 32 g/mol => 0.325 mol of O2

2 mol of Mg reacts with 1 mol O2

So 0.4115 mol of Mg would require 0.4115 /2 => 0.2057 mol of O2

Theoretical yield of MgO = 2*0.2057 => 0.4115 mol

Molar mass of MgO => 40.3 g/mol

0.4115 mol * 40.3 g/mol => 16.58 g of MgO

Part B) answer m = 16.58 g

Part C)

% yield = ( actual yield / theoretical yield) * 100

= ( 12.1 g / 16.58 ) * 100

= 72.9 or 80 %

Answer = 72.9 %

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