Aluminum metal reacts with solid copper(II) oxide to form copper metal and solid aluminum oxide...............
Q. write the equation (balanced with whole numbers) representing this reaction and show any necessary calculations to find the enthalpy change for two moles of aluminum reacting. Is this endothermic or exothermic
Asked by amy s - Mon Feb 4 18:56:10 2008 - - 1 Answers - 0 Comments
A. reaction equation: 2 Al(s) + 3 CuO(s) Al O (s) + 3 Cu(s) According to Hess's law the enthalpy of reaction is the difference of the heat of formation of the products minus the heat of formation of the reactants: rH = ( _i fH_i)_products - ( _i fH_i)_reactants where _i is stoihiometric coefficient of component i The enthalpy of formation of elements in their standard state equals zero. From NIST webbook fH(CuO) = -156.06kJ/mol fH(Al O ) = -1675.7kJ/mol Hence the the enthalpy of the reaction above is rH = fH(Al O ) - 3 fH(CuO) = -1675.7kJ/mol - 3 (-156.06kJ/mol) = -1207.52kJ/mol rH<0, the reaction is exothermic.
Answered by schmiso - Tue Feb 5 05:10:13 2008
Q. write the equation (balanced with whole numbers) representing this reaction and show any necessary calculations to find the enthalpy change for two moles of aluminum reacting. Is this endothermic or exothermic
Asked by amy s - Mon Feb 4 18:56:10 2008 - - 1 Answers - 0 Comments
A. reaction equation: 2 Al(s) + 3 CuO(s) Al O (s) + 3 Cu(s) According to Hess's law the enthalpy of reaction is the difference of the heat of formation of the products minus the heat of formation of the reactants: rH = ( _i fH_i)_products - ( _i fH_i)_reactants where _i is stoihiometric coefficient of component i The enthalpy of formation of elements in their standard state equals zero. From NIST webbook fH(CuO) = -156.06kJ/mol fH(Al O ) = -1675.7kJ/mol Hence the the enthalpy of the reaction above is rH = fH(Al O ) - 3 fH(CuO) = -1675.7kJ/mol - 3 (-156.06kJ/mol) = -1207.52kJ/mol rH<0, the reaction is exothermic.
Answered by schmiso - Tue Feb 5 05:10:13 2008
formula for: fluorine gas reacts with solid aluminum oxide to form solid aluminum fluoride and oxygen?
Q. formula for: fluorine gas reacts with solid aluminum oxide to form solid aluminum fluoride and oxygen?
Asked by daisy ;) - Tue Mar 4 01:02:53 2008 - - 1 Answers - 0 Comments
A. 3F2+ 2Al2O3---> 2AlF3+302 Or three fluorines react with two aluminum oxides to form two aluminum fluorides and three oxygen
Answered by Teancum2010 - Tue Mar 4 01:07:54 2008
Q. formula for: fluorine gas reacts with solid aluminum oxide to form solid aluminum fluoride and oxygen?
Asked by daisy ;) - Tue Mar 4 01:02:53 2008 - - 1 Answers - 0 Comments
A. 3F2+ 2Al2O3---> 2AlF3+302 Or three fluorines react with two aluminum oxides to form two aluminum fluorides and three oxygen
Answered by Teancum2010 - Tue Mar 4 01:07:54 2008
aluminum metal+oxygen gas=aluminum oxide solid ---how to write chemical equation!?
Q. aluminum metal+oxygen gas=aluminum oxide solid ---how to write chemical equation!?
Asked by cleanlady12 - Wed Jul 15 14:25:35 2009 - - 3 Answers - 0 Comments
A. 4 Al (s) + 3 O2 (g) -> 2 Al2O3 (s) Chem Man, it's not balanced ;)
Answered by feanor - Wed Jul 15 15:21:18 2009
Q. aluminum metal+oxygen gas=aluminum oxide solid ---how to write chemical equation!?
Asked by cleanlady12 - Wed Jul 15 14:25:35 2009 - - 3 Answers - 0 Comments
A. 4 Al (s) + 3 O2 (g) -> 2 Al2O3 (s) Chem Man, it's not balanced ;)
Answered by feanor - Wed Jul 15 15:21:18 2009
is there any solid material which can break down the Aluminum oxide from the Alumonum surface?
Q. Someone told me that mg can react with the aluminum oxide Al2O3 and break it down...is that true?
Asked by Calgarian_man - Mon May 1 12:14:19 2006 - - 1 Answers - 0 Comments
A. Yes. Mg is more reactive than the Al, so the Mg will reduce the Al, and form an oxide or hydroxide. Much depends on the conditions. This would be helped along by a little water, acid would help even more, and a catalyst may also help.
Answered by Favoured - Mon May 1 12:20:26 2006
Q. Someone told me that mg can react with the aluminum oxide Al2O3 and break it down...is that true?
Asked by Calgarian_man - Mon May 1 12:14:19 2006 - - 1 Answers - 0 Comments
A. Yes. Mg is more reactive than the Al, so the Mg will reduce the Al, and form an oxide or hydroxide. Much depends on the conditions. This would be helped along by a little water, acid would help even more, and a catalyst may also help.
Answered by Favoured - Mon May 1 12:20:26 2006
Stoichiometry, iron (III) oxide and aluminum?
Q. Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel rocket motors. The reaction is given below. Fe2O3(s) + 2 Al(s) 2 Fe(l) + Al2O3(s) What masses of iron(III) oxide and aluminum must be used to produce 26.0 g iron? iron (III) oxide What is the maximum mass of aluminum oxide that could be produced?
Asked by DooBop. - Mon Aug 31 22:51:03 2009 - - 1 Answers - 0 Comments
A. Your Given is 26.0 g Fe and ? = Fe2O3 So start with your given 26.0g Fe, then what you need to do is find the atomic mass of 1 mole of Iron which is 55.9 g Fe. Next look at your eqn to compare moles there are 2 moles of Iron produced for every 1 mole of Iron (III) oxide. The last thing you need is the molar mass of Fe2O3 which is 159.8 g With all this info you just use stoich and it should look something like this (26.0g Fe) * (1 mol Fe/ 55.9 g Fe) * (1 mol Fe2O3/ 2 Mol Fe) * (159.8 g Fe2O3/ 1 Mol Fe2O3) You should be able to take it from there
Answered by Trigger - Mon Aug 31 23:07:31 2009
Q. Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel rocket motors. The reaction is given below. Fe2O3(s) + 2 Al(s) 2 Fe(l) + Al2O3(s) What masses of iron(III) oxide and aluminum must be used to produce 26.0 g iron? iron (III) oxide What is the maximum mass of aluminum oxide that could be produced?
Asked by DooBop. - Mon Aug 31 22:51:03 2009 - - 1 Answers - 0 Comments
A. Your Given is 26.0 g Fe and ? = Fe2O3 So start with your given 26.0g Fe, then what you need to do is find the atomic mass of 1 mole of Iron which is 55.9 g Fe. Next look at your eqn to compare moles there are 2 moles of Iron produced for every 1 mole of Iron (III) oxide. The last thing you need is the molar mass of Fe2O3 which is 159.8 g With all this info you just use stoich and it should look something like this (26.0g Fe) * (1 mol Fe/ 55.9 g Fe) * (1 mol Fe2O3/ 2 Mol Fe) * (159.8 g Fe2O3/ 1 Mol Fe2O3) You should be able to take it from there
Answered by Trigger - Mon Aug 31 23:07:31 2009
write and balance equations for the following reactions.?
Q. a. Iron metal and chlorine gas react to form solid iron(III) chloride. b. Solid aluminum carbonate decomposes to form solid aluminum oxide and carbon dioxide gas. c. Solid mangnesium reacts with aqueous silver nitrate to form solid silver and aqueous magnesium nitrate.
Asked by checojoel - Tue Apr 1 18:55:07 2008 - - 2 Answers - 0 Comments
A. 2Fe + 3Cl2 -> 2FeCl3 Al2(CO3)3 -> Al2O3 + 3CO2 Mg + 2AgNO3 -> 2Ag + Mg(NO3)2 hope this helps
Answered by Mr. Ridley - Tue Apr 1 19:06:02 2008
Q. a. Iron metal and chlorine gas react to form solid iron(III) chloride. b. Solid aluminum carbonate decomposes to form solid aluminum oxide and carbon dioxide gas. c. Solid mangnesium reacts with aqueous silver nitrate to form solid silver and aqueous magnesium nitrate.
Asked by checojoel - Tue Apr 1 18:55:07 2008 - - 2 Answers - 0 Comments
A. 2Fe + 3Cl2 -> 2FeCl3 Al2(CO3)3 -> Al2O3 + 3CO2 Mg + 2AgNO3 -> 2Ag + Mg(NO3)2 hope this helps
Answered by Mr. Ridley - Tue Apr 1 19:06:02 2008
Does anyone know how to balance these chemical equations...?
Q. 1.) iron metal and chlorine gas react to form solid iron(III) chloride. 2.) solid aluminum carbonate decomposes to form solid aluminum oxide and carbon dioxide gas. 3.) Solid magnesium reacts with aqueous sliver nitrate to form solid silver and aquarius magnesium nitrate
Asked by jonasbrothersjew - Wed Jan 7 16:38:33 2009 - - 4 Answers - 0 Comments
A. 1) 2Fe + 3Cl2 --> 2FeCl3 2) Al2(CO3)3 --> Al2O3 + 3CO2 Edit: 3) 2AgNO3 + Mg --> Mg(NO3)2 + 2Ag
Answered by Shivan S - Wed Jan 7 16:44:02 2009
Q. 1.) iron metal and chlorine gas react to form solid iron(III) chloride. 2.) solid aluminum carbonate decomposes to form solid aluminum oxide and carbon dioxide gas. 3.) Solid magnesium reacts with aqueous sliver nitrate to form solid silver and aquarius magnesium nitrate
Asked by jonasbrothersjew - Wed Jan 7 16:38:33 2009 - - 4 Answers - 0 Comments
A. 1) 2Fe + 3Cl2 --> 2FeCl3 2) Al2(CO3)3 --> Al2O3 + 3CO2 Edit: 3) 2AgNO3 + Mg --> Mg(NO3)2 + 2Ag
Answered by Shivan S - Wed Jan 7 16:44:02 2009
Easy ten points! Chem help! Balanced equation to represent this reaction?
Q. silicon dioxide gas reacts with solid aluminum to produce solid silicon and solid aluminum oxide
Asked by ASHA Y - Wed Nov 5 21:14:50 2008 - - 1 Answers - 0 Comments
A. 3SiO2 + 4Al >>2 Al2O3 + 3 Si
Answered by Dr.A - Thu Nov 6 07:58:18 2008
Q. silicon dioxide gas reacts with solid aluminum to produce solid silicon and solid aluminum oxide
Asked by ASHA Y - Wed Nov 5 21:14:50 2008 - - 1 Answers - 0 Comments
A. 3SiO2 + 4Al >>2 Al2O3 + 3 Si
Answered by Dr.A - Thu Nov 6 07:58:18 2008
need help with 2 more chemistry questions! contain 1 very very hard question!?
Q. 69. write the balanced chemical equation for this word equation: solid ferric oxide reacts with solid aluminum metal to yield solid aluminum oxide and solid iron metal (i dont know what the formula for ferric oxide :'( ) 112. Balance the equation: NH3 + NO2 --> N2O + H2O (even my teacher cound'nt balance it!!! anyone plz help )': )
Asked by Timberland F - Thu Dec 3 06:25:07 2009 - - 2 Answers - 0 Comments
A. 69.3 Al + (FeO2)3 = 3 AlO2 + 3 Fe 112.In this case, you must also account for the oxidation-reduction of the N's. 2NO2 + 6H+ + 6e- --> N2O + 3H2O 2NH3 + 8OH- --> N2O + 7H2O + 8e- Multiply the first equation by 8 and the second equation by 6 (to balance the electrons) 16NO2 + 12NH3 +48H2O --> 14N2O + 66H2O Subtract 48 waters 16NO2 + 12NH3 --> 14N2O + 18H2O Divide by 2 8NO2 + 6NH3 --> 7N2O + 9H2O
Answered by Will H - Thu Dec 3 06:56:16 2009
Q. 69. write the balanced chemical equation for this word equation: solid ferric oxide reacts with solid aluminum metal to yield solid aluminum oxide and solid iron metal (i dont know what the formula for ferric oxide :'( ) 112. Balance the equation: NH3 + NO2 --> N2O + H2O (even my teacher cound'nt balance it!!! anyone plz help )': )
Asked by Timberland F - Thu Dec 3 06:25:07 2009 - - 2 Answers - 0 Comments
A. 69.3 Al + (FeO2)3 = 3 AlO2 + 3 Fe 112.In this case, you must also account for the oxidation-reduction of the N's. 2NO2 + 6H+ + 6e- --> N2O + 3H2O 2NH3 + 8OH- --> N2O + 7H2O + 8e- Multiply the first equation by 8 and the second equation by 6 (to balance the electrons) 16NO2 + 12NH3 +48H2O --> 14N2O + 66H2O Subtract 48 waters 16NO2 + 12NH3 --> 14N2O + 18H2O Divide by 2 8NO2 + 6NH3 --> 7N2O + 9H2O
Answered by Will H - Thu Dec 3 06:56:16 2009
Chemistry Help With Unbalanced Chemical Equation!?
Q. The group 2 metals (Ba, Ca, Br) can be produced in the elemental state by the reaction of their oxides with aluminum metal at high temperatures, also producing solid Aluminum Oxide. Write the unbalanced chemical equation for reactions of barium oxide, calcium oxide, and strontium oxide with aluminum. Ty. :)
Asked by lelouchvibritannia17th - Thu Dec 17 02:06:17 2009 - - 2 Answers - 0 Comments
A. I'll assume that the reaction is conducted at high temperature in an inert atmosphere. Therefore, the unbalanced equation is: BaO + Al = Ba + AlO barium oxide + aluminum yields barium + aluminum oxide For the other two compounds just replace Ba with Ca or Sr. In reality, aluminum oxide is Al2O3. Therefore, you need 2 moles of Al and 3 moles of O. To get 3 moles of O you need 3 moles of BaO so you will produce 3 moles of Ba. The balanced equation is: 3BaO + 2 Al = 3 Ba + Al2O3
Answered by Typcynic - Thu Dec 17 02:20:54 2009
Q. The group 2 metals (Ba, Ca, Br) can be produced in the elemental state by the reaction of their oxides with aluminum metal at high temperatures, also producing solid Aluminum Oxide. Write the unbalanced chemical equation for reactions of barium oxide, calcium oxide, and strontium oxide with aluminum. Ty. :)
Asked by lelouchvibritannia17th - Thu Dec 17 02:06:17 2009 - - 2 Answers - 0 Comments
A. I'll assume that the reaction is conducted at high temperature in an inert atmosphere. Therefore, the unbalanced equation is: BaO + Al = Ba + AlO barium oxide + aluminum yields barium + aluminum oxide For the other two compounds just replace Ba with Ca or Sr. In reality, aluminum oxide is Al2O3. Therefore, you need 2 moles of Al and 3 moles of O. To get 3 moles of O you need 3 moles of BaO so you will produce 3 moles of Ba. The balanced equation is: 3BaO + 2 Al = 3 Ba + Al2O3
Answered by Typcynic - Thu Dec 17 02:20:54 2009
Balance equation? BEST ANSWER will be given!?
Q. solid aluminum oxide is decomposed into aluminum and oxygen. Write the balanced equation.
Asked by Kristi K - Thu Dec 18 20:10:01 2008 - - 2 Answers - 0 Comments
A. 2Al2O3(s) => 4Al(s) + 3O2(g)
Answered by jake_inman3 - Thu Dec 18 20:13:27 2008
Q. solid aluminum oxide is decomposed into aluminum and oxygen. Write the balanced equation.
Asked by Kristi K - Thu Dec 18 20:10:01 2008 - - 2 Answers - 0 Comments
A. 2Al2O3(s) => 4Al(s) + 3O2(g)
Answered by jake_inman3 - Thu Dec 18 20:13:27 2008
Chemistry Help Please?
Q. (11)Write and balance equations for the following reactions. a.) Iron metal and chlorine gas react to form solid iron(III) chloride. b.) Solid aluminum carbonate decomposes to form solid aluminum oxide and carbon dioxide gas. c.) Solid magnesium reacts with aqueous silver nitrate to form solid silver and aqueous magnesium nitrate.
Asked by Angie B - Sat Feb 21 12:29:56 2009 - - 2 Answers - 0 Comments
A. a) 2Fe + 3Cl2 = 2FeCL3 b) Al2(CO3)3 = Al2O3 + 3CO2 c) Mg + 2AgNO3 = Mg(NO3)2 + 2Ag
Answered by Dr^valentine - Sat Feb 21 12:41:34 2009
Q. (11)Write and balance equations for the following reactions. a.) Iron metal and chlorine gas react to form solid iron(III) chloride. b.) Solid aluminum carbonate decomposes to form solid aluminum oxide and carbon dioxide gas. c.) Solid magnesium reacts with aqueous silver nitrate to form solid silver and aqueous magnesium nitrate.
Asked by Angie B - Sat Feb 21 12:29:56 2009 - - 2 Answers - 0 Comments
A. a) 2Fe + 3Cl2 = 2FeCL3 b) Al2(CO3)3 = Al2O3 + 3CO2 c) Mg + 2AgNO3 = Mg(NO3)2 + 2Ag
Answered by Dr^valentine - Sat Feb 21 12:41:34 2009
Can you balance these equations? thank you!?
Q. a) Iron metal and chlorine gas react to form solid iron (III) chloride. b) Solid aluminum carbonate decomposes to form solid aluminum oxide and carbone dioxide gas. I don't understand these. =/ Thank you if you respond!
Asked by ^^PaperHeart^^ - Wed Apr 2 19:13:13 2008 - - 2 Answers - 0 Comments
A. a) 2Fe (s) + 3Cl2 (g) --> 2FeCl3 (s) b) Al2(CO3)3 (s) --> Al2O3 (s) + 3CO2 (g)
Answered by yayaya - Wed Apr 2 19:16:48 2008
Q. a) Iron metal and chlorine gas react to form solid iron (III) chloride. b) Solid aluminum carbonate decomposes to form solid aluminum oxide and carbone dioxide gas. I don't understand these. =/ Thank you if you respond!
Asked by ^^PaperHeart^^ - Wed Apr 2 19:13:13 2008 - - 2 Answers - 0 Comments
A. a) 2Fe (s) + 3Cl2 (g) --> 2FeCl3 (s) b) Al2(CO3)3 (s) --> Al2O3 (s) + 3CO2 (g)
Answered by yayaya - Wed Apr 2 19:16:48 2008
wats the equations?
Q. when solid aluminum oxide and hydrogen gas are heated, molten aluminum and water vapor form? magnesium metal and water react to form magnesium hydroxide and hydrogen gas? when C2H6 burns it combines with oxygen to form carbon dioxide and water? iron metal and aluminum oxide form when aluminum metal reacts with iron(III)?
Asked by cookiesworld85 - Wed May 21 01:27:59 2008 - - 2 Answers - 0 Comments
Q. when solid aluminum oxide and hydrogen gas are heated, molten aluminum and water vapor form? magnesium metal and water react to form magnesium hydroxide and hydrogen gas? when C2H6 burns it combines with oxygen to form carbon dioxide and water? iron metal and aluminum oxide form when aluminum metal reacts with iron(III)?
Asked by cookiesworld85 - Wed May 21 01:27:59 2008 - - 2 Answers - 0 Comments
science help plz?
Q. Thermite is a mixture of iron(III) oxide and aluminum powders that was once used to weld railroad tracks. It undergoes a spectacular reaction to yield solid aluminum oxide and molten iron. (a) How many grams of iron form when 147 g of aluminum reacts? (b) How many atoms of aluminum react for every 3.90 g of aluminum oxide formed?
Asked by Krn Pwner - Thu Dec 13 22:17:50 2007 - - 2 Answers - 0 Comments
A. Fe2O3 + 2 Al ---> Al2O3 + 2 Fe a) There is a 2:2 (or 1:1) mole ratio between aluminum and iron. Therefore: 147 g / 27 g = X / 56 g X = 305 grams b) Mol mass Al2O3 = 2(27) + 3(16) = 102 g/mol 2(6.02 X 10^23 Al atoms) / 102 g Al2O3 = X / 3.90 g Al2O3 X = 4.60 X10^22 Aluminum atoms
Answered by Dennis M - Thu Dec 13 22:33:50 2007
Q. Thermite is a mixture of iron(III) oxide and aluminum powders that was once used to weld railroad tracks. It undergoes a spectacular reaction to yield solid aluminum oxide and molten iron. (a) How many grams of iron form when 147 g of aluminum reacts? (b) How many atoms of aluminum react for every 3.90 g of aluminum oxide formed?
Asked by Krn Pwner - Thu Dec 13 22:17:50 2007 - - 2 Answers - 0 Comments
A. Fe2O3 + 2 Al ---> Al2O3 + 2 Fe a) There is a 2:2 (or 1:1) mole ratio between aluminum and iron. Therefore: 147 g / 27 g = X / 56 g X = 305 grams b) Mol mass Al2O3 = 2(27) + 3(16) = 102 g/mol 2(6.02 X 10^23 Al atoms) / 102 g Al2O3 = X / 3.90 g Al2O3 X = 4.60 X10^22 Aluminum atoms
Answered by Dennis M - Thu Dec 13 22:33:50 2007
easy ten points! balancing equations. chemistry help!?
Q. balanced equations to represent each reaction below?: a) silicon dioxide gas reacts with solid aluminum to produce solid silicon and solid aluminum oxide b) silver nitrate reacts with hydrogen chloride to produce silver chloride and hydrogen nitrate c) magnesium and copper(II) sulphate undergo a single displacement reaction d) to produce a single displacement reaction, chlorine gas is bubbled into a potassium bromide solution e) lead(IV) nitrate and sodium iodide undergo a double displacement reaction
Asked by bob - Wed Nov 5 19:41:38 2008 - - 1 Answers - 0 Comments
A. 3SiO2 +4 Al >>2 Al2O3 +3 Si AgNO3 + HCl >> AgCl + HNO3 Mg + CuSO4 >> MgSO4 + Cu Cl2 + 2 KBr >> 2 KCl + Br2 Pb(NO3)4 + 4 NaI >> PbI4 + 4 NaNO3
Answered by Dr.A - Thu Nov 6 08:50:50 2008
Q. balanced equations to represent each reaction below?: a) silicon dioxide gas reacts with solid aluminum to produce solid silicon and solid aluminum oxide b) silver nitrate reacts with hydrogen chloride to produce silver chloride and hydrogen nitrate c) magnesium and copper(II) sulphate undergo a single displacement reaction d) to produce a single displacement reaction, chlorine gas is bubbled into a potassium bromide solution e) lead(IV) nitrate and sodium iodide undergo a double displacement reaction
Asked by bob - Wed Nov 5 19:41:38 2008 - - 1 Answers - 0 Comments
A. 3SiO2 +4 Al >>2 Al2O3 +3 Si AgNO3 + HCl >> AgCl + HNO3 Mg + CuSO4 >> MgSO4 + Cu Cl2 + 2 KBr >> 2 KCl + Br2 Pb(NO3)4 + 4 NaI >> PbI4 + 4 NaNO3
Answered by Dr.A - Thu Nov 6 08:50:50 2008
net ionic equation help.. please?
Q. i'm having trouble with these: 1. solid lithium is added to a solution of sodium hydroxide 2. solid aluminum oxide is added to water. im having trouble dissociating them and writing them out. any help would be appreciated. i will pick a best answer.
Asked by Rachel A - Sun Nov 25 07:23:07 2007 - - 1 Answers - 0 Comments
A. 1. The lithium will displace the sodium from solution as it is more reactive. Li(s) + Na^+(aq) ---> Li^+(aq) + Na(s) 2. As far as i am aware the aluminium oxide is insoluable in water so no ionic equation is needed
Answered by snowboardtherapy - Sun Nov 25 07:44:03 2007
Q. i'm having trouble with these: 1. solid lithium is added to a solution of sodium hydroxide 2. solid aluminum oxide is added to water. im having trouble dissociating them and writing them out. any help would be appreciated. i will pick a best answer.
Asked by Rachel A - Sun Nov 25 07:23:07 2007 - - 1 Answers - 0 Comments
A. 1. The lithium will displace the sodium from solution as it is more reactive. Li(s) + Na^+(aq) ---> Li^+(aq) + Na(s) 2. As far as i am aware the aluminium oxide is insoluable in water so no ionic equation is needed
Answered by snowboardtherapy - Sun Nov 25 07:44:03 2007
Whoever loves reactions, help!?
Q. 1) solid aluminum oxide (Al2O3) is added to hydrochloric acid (HCl) 2) solid diphosphorus trioxide (P2O3) is added to water (in case you don't know, H2O)
Asked by ananymous - Sun Apr 29 09:25:25 2007 - - 2 Answers - 0 Comments
A. You should get something like - 1) Aluminium Chloride + Water 2) Diphosphorus Oxide + Hydrogen
Answered by ManicStreetPreacher - Sun Apr 29 09:34:04 2007
Q. 1) solid aluminum oxide (Al2O3) is added to hydrochloric acid (HCl) 2) solid diphosphorus trioxide (P2O3) is added to water (in case you don't know, H2O)
Asked by ananymous - Sun Apr 29 09:25:25 2007 - - 2 Answers - 0 Comments
A. You should get something like - 1) Aluminium Chloride + Water 2) Diphosphorus Oxide + Hydrogen
Answered by ManicStreetPreacher - Sun Apr 29 09:34:04 2007
Can you write out chemical equations or know of a site that can?
Q. How do you write theses and balance them: Chlorine gas is added to a container in which lithium metal was placed. It is heated to produce a solid compound. What does this mean. Is it.. Cl + Li --> ClLi If so how doy balance that, and if not what is the correct way to do it?? Others I need help on are... Solid aluminum carbonate is heated strongly. Solid aluminum oxide is produced along with a a gas which will extingush fires, I think its AlCO2 + O2 --> AlO2 + H2O Liquid hydrogeb peroxide is heated with the catalyst magneses (IV) oxide. A liquid os produced as well as a gas which allows things to burn. I have NO idea how to do this one. (???) Copper (II) chlorate is heated. Oxygen is prodeuced and a solied product is left behind. … [cont.]
Asked by Via - Sun Feb 15 23:20:49 2009 - - 2 Answers - 0 Comments
A. Lithium will react with chlorine gas at room temp. 2Li(s) + Cl2(g) --> 2LiCl(s) Aluminum carbonate is Al2(CO3)3 Al2(CO3)3 --> Al2O3(s) + CO2(g) MnO2 is a catalyst and doesn't show up as either a reactant or product, even though it is actually a reactant in the first step of a two step mechanism and a product in the second step. The catalyst is usually written over the arrow. H2O2(l) --MnO2--> H2O(l) + O2(g) Copper (II) chlorate is probably what you want. It decomposes when heated to make oxygen. Cu(ClO3)2(g) --> CuCl2(s) + 3O2(g) CuO(s) + H2O(l) --> Ca(OH)2(aq) You are really clueless, aren't you? All these answers you've gotten are worthless unless you can actually figure these out for yourself. This is not something that you… [cont.]
Answered by pisgahchemist - Sun Feb 15 23:42:46 2009
Q. How do you write theses and balance them: Chlorine gas is added to a container in which lithium metal was placed. It is heated to produce a solid compound. What does this mean. Is it.. Cl + Li --> ClLi If so how doy balance that, and if not what is the correct way to do it?? Others I need help on are... Solid aluminum carbonate is heated strongly. Solid aluminum oxide is produced along with a a gas which will extingush fires, I think its AlCO2 + O2 --> AlO2 + H2O Liquid hydrogeb peroxide is heated with the catalyst magneses (IV) oxide. A liquid os produced as well as a gas which allows things to burn. I have NO idea how to do this one. (???) Copper (II) chlorate is heated. Oxygen is prodeuced and a solied product is left behind. … [cont.]
Asked by Via - Sun Feb 15 23:20:49 2009 - - 2 Answers - 0 Comments
A. Lithium will react with chlorine gas at room temp. 2Li(s) + Cl2(g) --> 2LiCl(s) Aluminum carbonate is Al2(CO3)3 Al2(CO3)3 --> Al2O3(s) + CO2(g) MnO2 is a catalyst and doesn't show up as either a reactant or product, even though it is actually a reactant in the first step of a two step mechanism and a product in the second step. The catalyst is usually written over the arrow. H2O2(l) --MnO2--> H2O(l) + O2(g) Copper (II) chlorate is probably what you want. It decomposes when heated to make oxygen. Cu(ClO3)2(g) --> CuCl2(s) + 3O2(g) CuO(s) + H2O(l) --> Ca(OH)2(aq) You are really clueless, aren't you? All these answers you've gotten are worthless unless you can actually figure these out for yourself. This is not something that you… [cont.]
Answered by pisgahchemist - Sun Feb 15 23:42:46 2009
Please help me answer these!!!?
Q. For each of the following reactions: A. Write names and correct formulas for all reactants. B. Write names and correct formulas for all products. C. Write a balanced chemical equation, including (s), (g), (aq), and (l). *That's an "l" as in "little."* 1. Magnesium metal reacts with hydrochloric acid to form magnesium chloride solution and hydrogen gas. 2. Solid magnesium sulfide and aqueous hydrochloric acid react to form hydrogen sulfide gas and magnesium chloride solution. 3.Aluminum metal burns in pure oxygen to produce solid aluminum oxide. 4. Hydrogen sulfide gas is bubbled through a sodium hydroxide solution to produce sodium sulfide in solution and liquid water. 5. Hydrogen gas and aluminum chloride solution are produced when… [cont.]
Asked by AmazingSpidey - Tue Apr 29 22:48:53 2008 - - 2 Answers - 0 Comments
Q. For each of the following reactions: A. Write names and correct formulas for all reactants. B. Write names and correct formulas for all products. C. Write a balanced chemical equation, including (s), (g), (aq), and (l). *That's an "l" as in "little."* 1. Magnesium metal reacts with hydrochloric acid to form magnesium chloride solution and hydrogen gas. 2. Solid magnesium sulfide and aqueous hydrochloric acid react to form hydrogen sulfide gas and magnesium chloride solution. 3.Aluminum metal burns in pure oxygen to produce solid aluminum oxide. 4. Hydrogen sulfide gas is bubbled through a sodium hydroxide solution to produce sodium sulfide in solution and liquid water. 5. Hydrogen gas and aluminum chloride solution are produced when… [cont.]
Asked by AmazingSpidey - Tue Apr 29 22:48:53 2008 - - 2 Answers - 0 Comments
From Yahoo Answer Search: 'solid aluminum oxide'
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