How many grams of Magnesium nitride can be made by mixing 35g of magnesium with 15 g of nitrogen?
Q. Magnesium nitride is made by combining magnesium and nitrogen. How many grams of Magnesium nitride can be made by mixing 35 g of magnesium with 15 g of nitrogen? What is the percent yield if actually 35g of Magnesium nitride is isolated? How many grams of the excess reactant remain after the reaction? Please show your work. Thanks.
Asked by Danilo - Mon Nov 23 16:48:00 2009 - - 1 Answers - 0 Comments
A. moles Mg = 35 / 24.305 g/mol=1.44 moles N2 = 15 g / 28.0134 g/mol=0.535 3 Mg + N2 = Mg3N2 Mg is the limiting reactant ( 0.535 x 3 =1.61 moles are needed) moles Mg3N2 = 1.44 /3 = 0.484 mass Mg3N2 = 0.48 x 100.8 g/mol=48.4 g % yield = 35 x 100 /48=73 moles N2 required = 1.44 /3 = 0.48 moles N2 in excess = 0.535 - 0.48 =0.055 mass N2 in excess = 0.055 x 28.0134 =1.5 g
Answered by Dr.A - Sat Nov 28 07:55:56 2009
Q. Magnesium nitride is made by combining magnesium and nitrogen. How many grams of Magnesium nitride can be made by mixing 35 g of magnesium with 15 g of nitrogen? What is the percent yield if actually 35g of Magnesium nitride is isolated? How many grams of the excess reactant remain after the reaction? Please show your work. Thanks.
Asked by Danilo - Mon Nov 23 16:48:00 2009 - - 1 Answers - 0 Comments
A. moles Mg = 35 / 24.305 g/mol=1.44 moles N2 = 15 g / 28.0134 g/mol=0.535 3 Mg + N2 = Mg3N2 Mg is the limiting reactant ( 0.535 x 3 =1.61 moles are needed) moles Mg3N2 = 1.44 /3 = 0.484 mass Mg3N2 = 0.48 x 100.8 g/mol=48.4 g % yield = 35 x 100 /48=73 moles N2 required = 1.44 /3 = 0.48 moles N2 in excess = 0.535 - 0.48 =0.055 mass N2 in excess = 0.055 x 28.0134 =1.5 g
Answered by Dr.A - Sat Nov 28 07:55:56 2009
What is the concentration of the magnesium nitrate after the reaction?
Q. 1.93 mL of 0.15 M magnesium hydroxide is added to 57 mL of 0.4 M nitric acid. (Magnesium nitrate and water are formed.) What is the concentration of the magnesium nitrate after the reaction?
Asked by undercover - Thu Mar 5 19:14:11 2009 - - 1 Answers - 0 Comments
A. Mg(OH)2 + 2H(NO3) --> Mg(NO3)2 + 2H2O first find the moles of each reagent Mg(OH)2: moles = (0.00193)*(0.15) = 0.0002895 moles H(NO3) moles = (0.057)*(0.4) = 0.228 moles Second, find the limiting reagent Mg(OH)2 : 2H(NO3) 1 2 2H(NO3) : Mg(OH)2 1 1/2 2 x 0.0002895mol Mg(OH)2 = 0.000573mol 2H(NO3) therefore limiting reagent is Mg(OH)2 Next find the number moles of Mg(NO3)2 0.0002895*(1mol Mg(NO3)2 /2mol Mg(OH)2) = 0.00014475 mol next find the molarity of Mg(NO3)2 0.00014475mol / 0.05893 L = 0.00246 M
Answered by Mike E - Sun Mar 8 17:11:38 2009
Q. 1.93 mL of 0.15 M magnesium hydroxide is added to 57 mL of 0.4 M nitric acid. (Magnesium nitrate and water are formed.) What is the concentration of the magnesium nitrate after the reaction?
Asked by undercover - Thu Mar 5 19:14:11 2009 - - 1 Answers - 0 Comments
A. Mg(OH)2 + 2H(NO3) --> Mg(NO3)2 + 2H2O first find the moles of each reagent Mg(OH)2: moles = (0.00193)*(0.15) = 0.0002895 moles H(NO3) moles = (0.057)*(0.4) = 0.228 moles Second, find the limiting reagent Mg(OH)2 : 2H(NO3) 1 2 2H(NO3) : Mg(OH)2 1 1/2 2 x 0.0002895mol Mg(OH)2 = 0.000573mol 2H(NO3) therefore limiting reagent is Mg(OH)2 Next find the number moles of Mg(NO3)2 0.0002895*(1mol Mg(NO3)2 /2mol Mg(OH)2) = 0.00014475 mol next find the molarity of Mg(NO3)2 0.00014475mol / 0.05893 L = 0.00246 M
Answered by Mike E - Sun Mar 8 17:11:38 2009
What ratio of magnesium and oxidizer is needed for flash powder?
Q. I need to know what ratio is needed for flash powder eg. 3 parts magnesium 1 part oxidizer.
Asked by Martin - Thu May 21 03:16:16 2009 - - 1 Answers - 0 Comments
A. Why? Flash powder is considered a high explosive by the BATFE, which makes it illegal to make without a Type 20 High Explosives Manufacturing License from the BATFE. I know people who have been caught with flash making materials, they get thrown in jail and labeled as a potential terrorist, it's not worth it.
Answered by crackerjacker13 - Thu May 21 08:07:22 2009
Q. I need to know what ratio is needed for flash powder eg. 3 parts magnesium 1 part oxidizer.
Asked by Martin - Thu May 21 03:16:16 2009 - - 1 Answers - 0 Comments
A. Why? Flash powder is considered a high explosive by the BATFE, which makes it illegal to make without a Type 20 High Explosives Manufacturing License from the BATFE. I know people who have been caught with flash making materials, they get thrown in jail and labeled as a potential terrorist, it's not worth it.
Answered by crackerjacker13 - Thu May 21 08:07:22 2009
How much magnesium is in this sample of seawater?
Q. 1 kg of 40 ppt seawater has 1.6 g magnesium ions. How many grams of magnesium ions are in 1 kg of 30 ppt seawater? I have the answer already, but the first person to get it right receives 10 pts!
Asked by Dynamic Fetch - Mon Mar 16 23:48:20 2009 - - 1 Answers - 0 Comments
A. 1.2 g
Answered by physicq210 - Tue Mar 17 00:31:53 2009
Q. 1 kg of 40 ppt seawater has 1.6 g magnesium ions. How many grams of magnesium ions are in 1 kg of 30 ppt seawater? I have the answer already, but the first person to get it right receives 10 pts!
Asked by Dynamic Fetch - Mon Mar 16 23:48:20 2009 - - 1 Answers - 0 Comments
A. 1.2 g
Answered by physicq210 - Tue Mar 17 00:31:53 2009
How do you find the mole ratio of magnesium oxide to magnesium?
Q. And then from there on, use that and the molar mass of magnesium oxide to calculate the theoretical yield of the product.
Asked by doomikazi - Fri Apr 4 04:47:44 2008 - - 2 Answers - 0 Comments
A. first, you need a balanced chemical equation. Look up the mole ratios you need for the coefficients. from that, you have to calculate first the limiting reactant. it's usually the one with the smaller amount. after that, use the limiting reactant to find the theoretical yield. BTW, that limiting reactant that you solved might be in moles. Use first the mole ratio between the reactant and the product and then convert to mass of magnesium oxide (product) using its molar mass. that's your theoretical yield. :)
Answered by rubidium.chloride - Fri Apr 4 04:58:01 2008
Q. And then from there on, use that and the molar mass of magnesium oxide to calculate the theoretical yield of the product.
Asked by doomikazi - Fri Apr 4 04:47:44 2008 - - 2 Answers - 0 Comments
A. first, you need a balanced chemical equation. Look up the mole ratios you need for the coefficients. from that, you have to calculate first the limiting reactant. it's usually the one with the smaller amount. after that, use the limiting reactant to find the theoretical yield. BTW, that limiting reactant that you solved might be in moles. Use first the mole ratio between the reactant and the product and then convert to mass of magnesium oxide (product) using its molar mass. that's your theoretical yield. :)
Answered by rubidium.chloride - Fri Apr 4 04:58:01 2008
Why add water to magnesium metal to convert it to magnesium oxide?
Q. What I'd like to know is WHY must we add water to magnesium metal to convert it to magnesium oxide? Mg(s) + air -> Mg3N2 Magnesium Nitride Mg3N2 + water -> MgO Magnesium Oxide Where does the Hydrogen go in the equation?
Asked by matthewrs_rahl - Sat Oct 3 17:14:41 2009 - - 1 Answers - 0 Comments
A. Okay, write it out. Mg3N2 + H2O --> MgO + N2 + H2 Balance: Mg3N2 + 3H2O --> 3MgO + N2 + 3H2 But this is probably double replacement, so you'll end up with ammonia: Mg3N2 + 3H2O---> 3MgO + 2NH3
Answered by Great Wolf - Mon Oct 5 14:24:17 2009
Q. What I'd like to know is WHY must we add water to magnesium metal to convert it to magnesium oxide? Mg(s) + air -> Mg3N2 Magnesium Nitride Mg3N2 + water -> MgO Magnesium Oxide Where does the Hydrogen go in the equation?
Asked by matthewrs_rahl - Sat Oct 3 17:14:41 2009 - - 1 Answers - 0 Comments
A. Okay, write it out. Mg3N2 + H2O --> MgO + N2 + H2 Balance: Mg3N2 + 3H2O --> 3MgO + N2 + 3H2 But this is probably double replacement, so you'll end up with ammonia: Mg3N2 + 3H2O---> 3MgO + 2NH3
Answered by Great Wolf - Mon Oct 5 14:24:17 2009
What is the theoretical yield of magnesium oxide?
Q. I use to know how to do these but I'm stumped. Can anyone walk me through this? Here's the given information: Mass of the empty crucible:15.3g Mass of crucible+magnesium: 15.83g Mass of crucible + product: 16.04g Mass of magnesium used: 0.3g Mass of magnesium oxide: 0.19g I don't know where to even begin. If you could help me I would be very appreciative!
Asked by Akumi B - Fri Dec 18 22:07:07 2009 - - 1 Answers - 0 Comments
A. Theoretically reactions go to completion so if you use.3g of Mg then you would have used .0123431393 moles and then you would produce .0123431393 moles of MgO which would weigh .497g
Answered by Erik - Fri Dec 18 23:46:40 2009
Q. I use to know how to do these but I'm stumped. Can anyone walk me through this? Here's the given information: Mass of the empty crucible:15.3g Mass of crucible+magnesium: 15.83g Mass of crucible + product: 16.04g Mass of magnesium used: 0.3g Mass of magnesium oxide: 0.19g I don't know where to even begin. If you could help me I would be very appreciative!
Asked by Akumi B - Fri Dec 18 22:07:07 2009 - - 1 Answers - 0 Comments
A. Theoretically reactions go to completion so if you use.3g of Mg then you would have used .0123431393 moles and then you would produce .0123431393 moles of MgO which would weigh .497g
Answered by Erik - Fri Dec 18 23:46:40 2009
What is the decomposition reaction when magnesium and HCl are mixed and heated to get Mg2Cl?
Q. can you tell me the balanced equation when magnesium mixes with HCL (and is heated) to form the salt? Please tell me all the products.
Asked by Eienstien's Ghost - Fri Sep 21 09:31:33 2007 - - 2 Answers - 0 Comments
A. I think you will find the salt is MgCl2. (Magnesium bonds two Chlorine atoms) and Hydrogen gas bubbles are produced. Mg + 2HCl = MgCl2 + H2 Caution: Magnesium is moderately reactive so you probably will not need to heat the solution. Definitely avoid naked flame.
Answered by leadbelly - Fri Sep 21 09:39:08 2007
Q. can you tell me the balanced equation when magnesium mixes with HCL (and is heated) to form the salt? Please tell me all the products.
Asked by Eienstien's Ghost - Fri Sep 21 09:31:33 2007 - - 2 Answers - 0 Comments
A. I think you will find the salt is MgCl2. (Magnesium bonds two Chlorine atoms) and Hydrogen gas bubbles are produced. Mg + 2HCl = MgCl2 + H2 Caution: Magnesium is moderately reactive so you probably will not need to heat the solution. Definitely avoid naked flame.
Answered by leadbelly - Fri Sep 21 09:39:08 2007
How can you test if theres magnesium in a sparkler?
Q. I want to know if a coloured sparkler contains magnesium. Are there any tests i can conduct to see if they do?
Asked by kfc_muncha - Tue Aug 19 06:30:35 2008 - - 1 Answers - 0 Comments
A. Try some flame tests on different compounds and see what looks right. Magnesium metal burns with a bright white light and does not give the characteristic sparks; that's iron. There's a list of flame colours here if you're not sure what to try:
Answered by cstspeedy - Tue Aug 19 06:47:11 2008
Q. I want to know if a coloured sparkler contains magnesium. Are there any tests i can conduct to see if they do?
Asked by kfc_muncha - Tue Aug 19 06:30:35 2008 - - 1 Answers - 0 Comments
A. Try some flame tests on different compounds and see what looks right. Magnesium metal burns with a bright white light and does not give the characteristic sparks; that's iron. There's a list of flame colours here if you're not sure what to try:
Answered by cstspeedy - Tue Aug 19 06:47:11 2008
What are some statements of comparison for magnesium and sulfur?
Q. in other words, what are the differences between sulfur and magnesium?
Asked by azncutie45 - Wed Oct 17 00:17:17 2007 - - 1 Answers - 0 Comments
A. Sulfur is A pale yellow nonmetallic element occurring widely in nature in several free and combined allotropic forms. It is used in black gunpowder, rubber vulcanization, the manufacture of insecticides and pharmaceuticals, and in the preparation of sulfur compounds such as hydrogen sulfide and sulfuric acid. Atomic number 16; atomic weight 32.066; melting point (rhombic) 112.8C, (monoclinic) 119.0C; boiling point 444.6C; specific gravity (rhombic) 2.07, (monoclinic) 1.957; valence 2, 4, 6. Magnesium is A light, silvery-white, moderately hard metallic element that in ribbon or powder form burns with a brilliant white flame. It is used in structural alloys, pyrotechnics, flash photography, and incendiary bombs. Atomic number 12; atomic… [cont.]
Answered by Pennsylvania - Wed Oct 17 01:05:53 2007
Q. in other words, what are the differences between sulfur and magnesium?
Asked by azncutie45 - Wed Oct 17 00:17:17 2007 - - 1 Answers - 0 Comments
A. Sulfur is A pale yellow nonmetallic element occurring widely in nature in several free and combined allotropic forms. It is used in black gunpowder, rubber vulcanization, the manufacture of insecticides and pharmaceuticals, and in the preparation of sulfur compounds such as hydrogen sulfide and sulfuric acid. Atomic number 16; atomic weight 32.066; melting point (rhombic) 112.8C, (monoclinic) 119.0C; boiling point 444.6C; specific gravity (rhombic) 2.07, (monoclinic) 1.957; valence 2, 4, 6. Magnesium is A light, silvery-white, moderately hard metallic element that in ribbon or powder form burns with a brilliant white flame. It is used in structural alloys, pyrotechnics, flash photography, and incendiary bombs. Atomic number 12; atomic… [cont.]
Answered by Pennsylvania - Wed Oct 17 01:05:53 2007
What are the formulas for zinc bicarbonate and magnesium bisulfate?
Q. What are the formulas for zinc bicarbonate and magnesium bisulfate? I think they're Zn(HCO3)2 and Mg(NaHSO4). If I'm wrong - explain the correct answer, please. Haha. The sodium was a weird typo.
Asked by Aneth - Sat Aug 9 18:18:45 2008 - - 3 Answers - 0 Comments
A. Both Zn and Mg have a valence of 2. Bicarbonate and Bisulphate have valences of 1. You're first formula is correct... Zn(2+) ion + 2 x HCO3(1-) ions... = Zn(HCO3)2. (Neutral Compound). The second will be Mg(HSO4)2... Mg(2+) ion + (2 x HSO4(1-) ions... = Mg(HSO4)2. (Neutral Compound).
Answered by __A_YAHOO_USER__ - Sat Aug 9 19:21:41 2008
Q. What are the formulas for zinc bicarbonate and magnesium bisulfate? I think they're Zn(HCO3)2 and Mg(NaHSO4). If I'm wrong - explain the correct answer, please. Haha. The sodium was a weird typo.
Asked by Aneth - Sat Aug 9 18:18:45 2008 - - 3 Answers - 0 Comments
A. Both Zn and Mg have a valence of 2. Bicarbonate and Bisulphate have valences of 1. You're first formula is correct... Zn(2+) ion + 2 x HCO3(1-) ions... = Zn(HCO3)2. (Neutral Compound). The second will be Mg(HSO4)2... Mg(2+) ion + (2 x HSO4(1-) ions... = Mg(HSO4)2. (Neutral Compound).
Answered by __A_YAHOO_USER__ - Sat Aug 9 19:21:41 2008
Is there a test to tell the difference between magnesium and aluminum?
Q. Is there an easy way to tell the difference? Will aluminum stick to magnesium by tig?
Asked by elmechino - Fri Oct 19 08:04:18 2007 - - 5 Answers - 0 Comments
A. Well their is always density, mass spectrometry, or magnesium shaving ignite at a relatively low temperature. Density is probably the easiest, figure out the mass per unit of volume and look it up on the periodic table.
Answered by Brian K - Fri Oct 19 08:08:10 2007
Q. Is there an easy way to tell the difference? Will aluminum stick to magnesium by tig?
Asked by elmechino - Fri Oct 19 08:04:18 2007 - - 5 Answers - 0 Comments
A. Well their is always density, mass spectrometry, or magnesium shaving ignite at a relatively low temperature. Density is probably the easiest, figure out the mass per unit of volume and look it up on the periodic table.
Answered by Brian K - Fri Oct 19 08:08:10 2007
What happens when you mix burnt magnesium and hydrochloric acid?
Q. I need to know what can be observed when these two mix, i.e. color, temperature change or foaming. I know unburnt magnesium and hydrochloric acid yield a gas (it foams) but what happens with burnt magnesium? Please help.
Asked by Cici - Sat Sep 5 18:48:58 2009 - - 1 Answers - 0 Comments
A. Magnesium burns in air to form magnesium oxide, MgO, which is a white solid. When the oxide is mixed with hydrochloric acid (HCl), the products are magnesium chloride and water according to the reaction equation: MgO + 2HCl MgCl2 + H2O Hope this answers your question.
Answered by Reginald - Sat Sep 5 19:13:54 2009
Q. I need to know what can be observed when these two mix, i.e. color, temperature change or foaming. I know unburnt magnesium and hydrochloric acid yield a gas (it foams) but what happens with burnt magnesium? Please help.
Asked by Cici - Sat Sep 5 18:48:58 2009 - - 1 Answers - 0 Comments
A. Magnesium burns in air to form magnesium oxide, MgO, which is a white solid. When the oxide is mixed with hydrochloric acid (HCl), the products are magnesium chloride and water according to the reaction equation: MgO + 2HCl MgCl2 + H2O Hope this answers your question.
Answered by Reginald - Sat Sep 5 19:13:54 2009
How many moles of magnesium are present in 47.9 grams of magnesium phosphate?
Q. How many moles of magnesium are present in 47.9 grams of magnesium phosphate? I want to know all the steps you take to solve this. Thanks!
Asked by Angela - Fri Nov 7 00:54:07 2008 - - 1 Answers - 0 Comments
A. First figure out what the formula of Magnesium Phosphate is. A rough estimate will say that Magnesium is +2 and Phosphate is -3, so the formula is Mg3(PO4)2. Now we know that there are three moles of magnesium in every one mole of Magnesium Phosphate. What remains is to find how many grams a mole of magnesium Phosphate is, which can be calculated from most periodic tables. Magnesium has an atomic weight of 24.31 grams/mole. Phosphorous has an atomic weight of 30.97 grams/mole. Oxygen has an atomic weight of 15.99 grams/mole. Adding all the atoms together gives us the formula, so. Mg3(PO)4 = 3Mg+2P+8O = 3(24.31)+2(30.97)+8(15.99 ) = 262.79 g/mol Now we have everything to calculate the moles of Magnesium. 47.9 grams / 262.79 grams/mole =… [cont.]
Answered by AKchem - Fri Nov 7 01:15:18 2008
Q. How many moles of magnesium are present in 47.9 grams of magnesium phosphate? I want to know all the steps you take to solve this. Thanks!
Asked by Angela - Fri Nov 7 00:54:07 2008 - - 1 Answers - 0 Comments
A. First figure out what the formula of Magnesium Phosphate is. A rough estimate will say that Magnesium is +2 and Phosphate is -3, so the formula is Mg3(PO4)2. Now we know that there are three moles of magnesium in every one mole of Magnesium Phosphate. What remains is to find how many grams a mole of magnesium Phosphate is, which can be calculated from most periodic tables. Magnesium has an atomic weight of 24.31 grams/mole. Phosphorous has an atomic weight of 30.97 grams/mole. Oxygen has an atomic weight of 15.99 grams/mole. Adding all the atoms together gives us the formula, so. Mg3(PO)4 = 3Mg+2P+8O = 3(24.31)+2(30.97)+8(15.99 ) = 262.79 g/mol Now we have everything to calculate the moles of Magnesium. 47.9 grams / 262.79 grams/mole =… [cont.]
Answered by AKchem - Fri Nov 7 01:15:18 2008
What are the vegetables that are rich in zinc and magnesium?
Q. Hello nutrition geeks can anyone tell me which fruits and vegetables are rich in magnesium and zinc. Please let me know only the vegetables, I know about oysters.
Asked by Router ID - Tue Oct 6 08:35:45 2009 - - 2 Answers - 0 Comments
A. Spinach, watercress, Swiss chard, romaine, kale, Beets and mustard greens and all kinds of beans contain both magnesium and zinc. Potato (with skin), Bananas,Kiwi, Papaya and Natural peanut butter contain magnesium but not zinc. Soya foods and grains such as Barley, Brown rice, Oatmeal and Wheat have both zinc and magnesium.
Answered by jarantar - Tue Oct 6 09:28:46 2009
Q. Hello nutrition geeks can anyone tell me which fruits and vegetables are rich in magnesium and zinc. Please let me know only the vegetables, I know about oysters.
Asked by Router ID - Tue Oct 6 08:35:45 2009 - - 2 Answers - 0 Comments
A. Spinach, watercress, Swiss chard, romaine, kale, Beets and mustard greens and all kinds of beans contain both magnesium and zinc. Potato (with skin), Bananas,Kiwi, Papaya and Natural peanut butter contain magnesium but not zinc. Soya foods and grains such as Barley, Brown rice, Oatmeal and Wheat have both zinc and magnesium.
Answered by jarantar - Tue Oct 6 09:28:46 2009
What is the chemical equation to fire ; Burning magnesium?
Q. Basically i need to know the word and skeleton equation of burning magnesium its a pain in the ass hopefully you can help. thanks not a big fan of chem so holla at me. and we used a bunsen burner to burn the magnesium . ... propane.. so that should help a little bit!
Asked by camoflage m - Thu Mar 27 00:29:53 2008 - - 1 Answers - 0 Comments
A. Doesn't matter what is used to ignite the Magnesium, it's the combustion reaction of Magnesium with Oxygen of the Air that is in question. Because Mg is a single atom (Mg(2+) ion) and, O2 is a di-atomic molecule (2 x O(2-) ions) , we need 2 atoms of Magnesium to 1 molecule of Oxygen... 2Mg + O2 = 2MgO
Answered by __A_YAHOO_USER__ - Thu Mar 27 00:59:53 2008
Q. Basically i need to know the word and skeleton equation of burning magnesium its a pain in the ass hopefully you can help. thanks not a big fan of chem so holla at me. and we used a bunsen burner to burn the magnesium . ... propane.. so that should help a little bit!
Asked by camoflage m - Thu Mar 27 00:29:53 2008 - - 1 Answers - 0 Comments
A. Doesn't matter what is used to ignite the Magnesium, it's the combustion reaction of Magnesium with Oxygen of the Air that is in question. Because Mg is a single atom (Mg(2+) ion) and, O2 is a di-atomic molecule (2 x O(2-) ions) , we need 2 atoms of Magnesium to 1 molecule of Oxygen... 2Mg + O2 = 2MgO
Answered by __A_YAHOO_USER__ - Thu Mar 27 00:59:53 2008
What kind of energy is released from burning magnesium?
Q. what about the product, is it just magnesium oxide and magnesium nitride.
Asked by perez_anaheim - Thu Dec 4 19:01:07 2008 - - 1 Answers - 0 Comments
A. hydrogen energy
Answered by D D - Thu Dec 4 19:17:35 2008
Q. what about the product, is it just magnesium oxide and magnesium nitride.
Asked by perez_anaheim - Thu Dec 4 19:01:07 2008 - - 1 Answers - 0 Comments
A. hydrogen energy
Answered by D D - Thu Dec 4 19:17:35 2008
Does anyone know how to raise magnesium in a salt water aquarium without affecting salinity?
Q. My magnesium is low and is affecting my calcium, is there any way to raise it without havign to use Tech M?
Asked by Ben H - Thu Oct 12 23:28:29 2006 - - 4 Answers - 0 Comments
A. A mix of magnesium chloride and magnesium sulfate is considered the best way to go. (see link) Calcium can be increased with limestone.
Answered by Sabersquirrel - Fri Oct 13 13:26:40 2006
Q. My magnesium is low and is affecting my calcium, is there any way to raise it without havign to use Tech M?
Asked by Ben H - Thu Oct 12 23:28:29 2006 - - 4 Answers - 0 Comments
A. A mix of magnesium chloride and magnesium sulfate is considered the best way to go. (see link) Calcium can be increased with limestone.
Answered by Sabersquirrel - Fri Oct 13 13:26:40 2006
Can Magnesium Citrate be mixed with soft drinks such as Pepsi?
Q. I am enlisting in the United States Navy. My recruiter informed me to take Magnesium Citrate to help 'flush' my system so that I can meet my maximum allowable weight. I can barely stand the bitter taste, and have found out that chilling it takes away the bitterness somewhat, but am wondering if it can be mixed with drinks like Pepsi or milk.
Asked by Topher - Tue Feb 26 18:50:01 2008 - - 3 Answers - 0 Comments
A. NO! You have to drink the entire bottle, didn't you get the flavored one? Just down it, and deal with it and make sure you are by a toilet.
Answered by April R - Tue Feb 26 18:55:24 2008
Q. I am enlisting in the United States Navy. My recruiter informed me to take Magnesium Citrate to help 'flush' my system so that I can meet my maximum allowable weight. I can barely stand the bitter taste, and have found out that chilling it takes away the bitterness somewhat, but am wondering if it can be mixed with drinks like Pepsi or milk.
Asked by Topher - Tue Feb 26 18:50:01 2008 - - 3 Answers - 0 Comments
A. NO! You have to drink the entire bottle, didn't you get the flavored one? Just down it, and deal with it and make sure you are by a toilet.
Answered by April R - Tue Feb 26 18:55:24 2008
How do you calculate how much magnesium oxide is formed?
Q. If i have 42 grams of Mg and 45 grams of O then how do find out how much magnesium oxide is formed?
Asked by Alli Bee - Tue Dec 15 19:45:14 2009 - - 1 Answers - 0 Comments
A. 1] Write balanced equation. 2] Write molar masses under each substance 3] You see that 48g Mg reacts with 32g O2 so you have more than enough oxygen 4] so amount of Mg controls it all 5] write statement from your equation ...g Mg forms ... g MgO 6] change to quantity you were given [43g Mg] by simple proportion 7] gives answer
Answered by Colin - Wed Dec 16 09:55:26 2009
Q. If i have 42 grams of Mg and 45 grams of O then how do find out how much magnesium oxide is formed?
Asked by Alli Bee - Tue Dec 15 19:45:14 2009 - - 1 Answers - 0 Comments
A. 1] Write balanced equation. 2] Write molar masses under each substance 3] You see that 48g Mg reacts with 32g O2 so you have more than enough oxygen 4] so amount of Mg controls it all 5] write statement from your equation ...g Mg forms ... g MgO 6] change to quantity you were given [43g Mg] by simple proportion 7] gives answer
Answered by Colin - Wed Dec 16 09:55:26 2009
From Yahoo Answer Search: 'Magnesium'
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It provides a balanced source of nutrition, rich in essential elements and magnesium . Algoflash consists of 100% mineral base and a range of very pure trace ...
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Discontinued The mineral magnesium performs hundreds of jobs within the body One vital function is to package food into an energy form the body can burn In addition magnesium is required for glucose
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Magnesium. metal smelters raised their quotations this week, on the back of increased production costs. But market demand remains slow and the future market is not expected to pick up much further. Tungsten miners continued to hold ...
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