What are some possible sources of error in burning Mg in O2 to find the empirical formula for magnesium oxide?
Q. Purpose: determine empirical formula of magnesium oxide by percentage composition. Results: 68.75% Mg---> 3Mg 31.25% O---> 2O Therefore, empirical formula is Mg3O2 (**The above is wrong, the actual formula is MgO**) Discuss possible sources of error and their effects on your results. Purpose: determine empirical formula of magnesium oxide by percentage composition. Results: 68.75% Mg---> 3Mg 31.25% O---> 2O Therefore, empirical formula is Mg3O2 (**The above is wrong, the actual formula is MgO**) Discuss possible sources of error and their effects on your results. Please explain any answer you give. Thanks!
Asked by Sarah B - Mon Mar 31 23:07:21 2008 - - 1 Answers - 0 Comments
A. You also produce Mg3N2, which is why you add some water before completing the experiment. This produces NH3 and MgO. Then you reheat the crucible. Chemical Demonstration Videos
Answered by kentchemistry.com - Mon Mar 31 23:13:39 2008
Q. Purpose: determine empirical formula of magnesium oxide by percentage composition. Results: 68.75% Mg---> 3Mg 31.25% O---> 2O Therefore, empirical formula is Mg3O2 (**The above is wrong, the actual formula is MgO**) Discuss possible sources of error and their effects on your results. Purpose: determine empirical formula of magnesium oxide by percentage composition. Results: 68.75% Mg---> 3Mg 31.25% O---> 2O Therefore, empirical formula is Mg3O2 (**The above is wrong, the actual formula is MgO**) Discuss possible sources of error and their effects on your results. Please explain any answer you give. Thanks!
Asked by Sarah B - Mon Mar 31 23:07:21 2008 - - 1 Answers - 0 Comments
A. You also produce Mg3N2, which is why you add some water before completing the experiment. This produces NH3 and MgO. Then you reheat the crucible. Chemical Demonstration Videos
Answered by kentchemistry.com - Mon Mar 31 23:13:39 2008
Determining the Empirical Formula of Magnesium Oxide?
Q. mass of crucible and cover, g...24.05g mass of crucible, cover and MG, g...24.41g mass of crucible, cover, and magnesium oxide, g...24.58 What would the the mass of Mg reacted be? What would be the mass of magnesium oxide formed? What would be the mass of O that combined with the Mg? Calculate the average number of moles of Mg that reacted. The molar mass of Mg is 24.31 g/mol. What is the average number of moles of Mg? Calculate the average number of moles of O that combined with the Mg. The molar mass of O is 16.00 g/mol. What is the average number of moles of O? Find the simplest ratio of the average number of moles of Mg to the average number of moles of O. Divide the average number of moles of Mg by the smaller of the average… [cont.]
Asked by Lora - Tue Mar 9 21:02:34 2010 - - 0 Answers - 0 Comments
Q. mass of crucible and cover, g...24.05g mass of crucible, cover and MG, g...24.41g mass of crucible, cover, and magnesium oxide, g...24.58 What would the the mass of Mg reacted be? What would be the mass of magnesium oxide formed? What would be the mass of O that combined with the Mg? Calculate the average number of moles of Mg that reacted. The molar mass of Mg is 24.31 g/mol. What is the average number of moles of Mg? Calculate the average number of moles of O that combined with the Mg. The molar mass of O is 16.00 g/mol. What is the average number of moles of O? Find the simplest ratio of the average number of moles of Mg to the average number of moles of O. Divide the average number of moles of Mg by the smaller of the average… [cont.]
Asked by Lora - Tue Mar 9 21:02:34 2010 - - 0 Answers - 0 Comments
I need help with my chemistry homework! Please!?
Q. What is the empirical formula of a compound that contains 10.52 g Ni, 4.38 g C, and 5.10 g N? (Type your answer using the format CO2 for CO2.) Monosodium glutamate (MSG) is sometimes added to food to enhance flavor. Analysis determined this compound to be 35.5% C, 4.77% H, 8.29% N, 13.6% Na, and 37.9% O.What is the empirical formula for MSG? (Type your answer using the format CO2 for CO2.) Determine the number of chloride ions in 11.17 g of magnesium chloride Calculate the moles of aluminum ions present in 299.8 g aluminum oxide (Al2O3). How many moles of oxygen atoms are contained in the following? (a) 2.64 mol KMnO4 mol (b) 49.6 mol CO2 mol (c) 2.05 10-2 mol CuSO4 5H2O mol Calculate the number of atoms in each of the… [cont.]
Asked by girleee1443 - Tue Dec 16 20:44:27 2008 - - 1 Answers - 0 Comments
A. How will you learn if you just get the answers from someone else? I'll do one for you: (a) 1.64 mol CS2 x 6.02 x 10^23 molecules (Avogradro's #)/1 mol CS2 = 9.8728 molecules CS2 = 9.87 x 10^23 molecules (significant digits) You use Avogadro's number in order to change from moles to molecules. You put it divided by 1 mol CS2 in order to cancel the mol units. Do the same for b, c, and d of that question and the one about calculating atoms.
Answered by killerkim - Tue Dec 16 20:59:50 2008
Q. What is the empirical formula of a compound that contains 10.52 g Ni, 4.38 g C, and 5.10 g N? (Type your answer using the format CO2 for CO2.) Monosodium glutamate (MSG) is sometimes added to food to enhance flavor. Analysis determined this compound to be 35.5% C, 4.77% H, 8.29% N, 13.6% Na, and 37.9% O.What is the empirical formula for MSG? (Type your answer using the format CO2 for CO2.) Determine the number of chloride ions in 11.17 g of magnesium chloride Calculate the moles of aluminum ions present in 299.8 g aluminum oxide (Al2O3). How many moles of oxygen atoms are contained in the following? (a) 2.64 mol KMnO4 mol (b) 49.6 mol CO2 mol (c) 2.05 10-2 mol CuSO4 5H2O mol Calculate the number of atoms in each of the… [cont.]
Asked by girleee1443 - Tue Dec 16 20:44:27 2008 - - 1 Answers - 0 Comments
A. How will you learn if you just get the answers from someone else? I'll do one for you: (a) 1.64 mol CS2 x 6.02 x 10^23 molecules (Avogradro's #)/1 mol CS2 = 9.8728 molecules CS2 = 9.87 x 10^23 molecules (significant digits) You use Avogadro's number in order to change from moles to molecules. You put it divided by 1 mol CS2 in order to cancel the mol units. Do the same for b, c, and d of that question and the one about calculating atoms.
Answered by killerkim - Tue Dec 16 20:59:50 2008
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