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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(g)?2MgO(s)
When 10.1g Mg is allowed to react with10.5g O2, 12.1g MgO is collected.
PART A
Determine the theoretical yield for the reaction.
PART B
Determine the percent yield for the reaction.
I need proficient help to solve the above problem
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There is a one to one relationship between the number of moles of hydrogen gas evolved and the moles of Magnesium metal consumed in the reaction, therefore moles of H2 evolved = moles Mg consumed and the atomic weight of Mg = weight of Mg consumed..
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