Answer to Question #249703 in General Chemistry for Ian

Question #249703
a 0.910 g sample of magnesium was reacted with oxygen to form 1.510 g of magnesium oxide.how much magnesium is needed to produce 0.850 g of magnesium oxide? how much magnesium and oxygen are needed to produce exactly 2.55 of magnesium oxide
1
Expert's answer
2021-10-11T06:12:29-0400

In the first case we can calculate the Mass of oxygen used =1.510g-0.910g


For the second question;

2Mg+O22MgO2Mg+O_2\to 2MgO

now moles of magnesium oxide =0.8502(24+16)=0.0106=\frac{0.850}{2(24+16)}=0.0106

mole ratio; 2Mg:2MgO=2:2=1:12Mg:2MgO=2:2=1:1

moles of Mg=0.0106

mass of magnesium=48×0.0106=0.5088g=48\times 0.0106=0.5088g


For the next question;

2Mg+O22MgO2Mg+O_2\to 2MgO

mass of magnesium oxide =2.552(24+16)=0.031875=\frac{2.55}{2(24+16)}=0.031875

mole ratio 2MgO:2Mg=2:2=1:12MgO:2Mg=2:2=1:1

mass of Mg =2×24×0.031875=1.53g=2\times 24\times 0.031875=1.53g

mass of oxygen=2.55g-1.53g=1.02g


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