Question

Magnesium Oxide can be made by heating magnesium metal in the presence of the oxygen. The...

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 10.2 g of Mg is allowed to react with 10.6 g O2, 11.9 g MgO is collected. Determine the theoretical yield for the reaction. Express your answer in grams. Determine the percent yield for the reaction. Express your answer as a percent.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Magnesium oxide can be made by heating magnesium metal in the presence of the oxygen. The...
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 10.0 g Mg is allowed to react with 10.5 g O2, 11.8 g MgO is collected. Determine the theoretical yield for the reaction. Determine the percent yield for the reaction.
Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced...
Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is: 2Mg(s)+O2(g)-->2MgO(s) When 10.1g of Mg are allowed to react with 10.5g of O2 11.0g of MgO are collected. A. determine the limiting reactant for the reaction. B. determine the theoretical yeild for the reaction C. determine the percent yeild for the reaction. B.
Magnesium oxide can be made by heating magnesium metal in the presence of gaseous oxygen. When...
Magnesium oxide can be made by heating magnesium metal in the presence of gaseous oxygen. When 10.1 grams of magnesium is allowed to react with 10.5 grams of molecular oxygen, 11.9 grams of magnesium oxide is collected. What is the percent yield of this reaction?
Magnesium metal can combust to yield magnesia or magnesium oxide according to the balanced equation for...
Magnesium metal can combust to yield magnesia or magnesium oxide according to the balanced equation for the reaction: 2Mg + O2 ----> 2 MgO.    Determine the mass of magnesia product (i.e. the theoretical yield) when 1.8 grams of magnesium combusts in the presence of an excess of oxygen. Please show process so I understand solving future stoich problems. THanks
ICE TABLE PLEASEEEEE The oxidation of 100 g of magnesium, Mg, by 50 g of oxygen,...
ICE TABLE PLEASEEEEE The oxidation of 100 g of magnesium, Mg, by 50 g of oxygen, O2, produces 80g of magnesium oxide, MgO. Draw a chemical spreadsheet to show what happens during the reaction and calculate how many grams of Mg, if any, are left after the reaction. Calculate the percent yeild to MgO. 2Mg + O2 ----> 2MgO ICE TABLE PLEASEEEEE
2Mg(s)+O2(g) ---> 2MgO(s) what is the theoretical yield of MgO(s) in moles when 6.50g Mg(s) reacts...
2Mg(s)+O2(g) ---> 2MgO(s) what is the theoretical yield of MgO(s) in moles when 6.50g Mg(s) reacts with 3.45g of O2(g)​
2Mg(s)+ O2(g) ----> 2MgO(s) a) What is the theoretical yield of MgO(s), in moles, when 6.50g...
2Mg(s)+ O2(g) ----> 2MgO(s) a) What is the theoretical yield of MgO(s), in moles, when 6.50g Mg(s) reacts with 3.45g of O2(g) b) What was the limiting reactant(LR) and the mass (in g) of MgO formed?
PART B When exposed to air, aluminum metal, Al, reacts with oxygen, O2, to produce a...
PART B When exposed to air, aluminum metal, Al, reacts with oxygen, O2, to produce a protective coating of aluminum oxide, Al2O3, which prevents the aluminum from rusting underneath. The balanced reaction is shown here: 4Al+3O2→2Al2O3 Part A: What is the theoretical yield of aluminum oxide if 2.80 mol of aluminum metal is exposed to 2.40 mol of oxygen? ANSWER: 1.40 mol Part B: In Part A, we saw that the theoretical yield of aluminum oxide is 1.40 mol ....
7.0 of Nitrogen gas is combined with 3.0g of oxygen gas. 4.5g of nitrous oxide is...
7.0 of Nitrogen gas is combined with 3.0g of oxygen gas. 4.5g of nitrous oxide is formed during the experiment. The balanced reaction is : N2(g) + O2(g) = 2NO(g). A. What is the limiting reagent? justify your answer. B. How many grams of NO is it possible to form (theoretical yield)? C. what is the percent yield?
1. In the following reaction, 451.4 g of lead reacts with excess oxygen forming 365.8 g...
1. In the following reaction, 451.4 g of lead reacts with excess oxygen forming 365.8 g of lead(II) oxide. Calculate the percent yield of the reaction. 2Pb(s)+O2(g) = 2PbO(s) 2. Assuming an efficiency of 32.60%, calculate the actual yield of magnesium nitrate formed from 119.8 g of magnesium and excess copper(II) nitrate. Mg + Cu(NO3)2 = Mg(NO3)2 + Cu 3. Combining 0.282 mol of Fe2O3 with excess carbon produced 18.8 g of Fe. Fe2O3 + 3C = 2Fe + 3CO...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT