How do I determine what reactant is limiting?
Q. For Al + HCl --> AlCl^3 + H^2. If 15.0 g of the reactant is taken, how do I determine if the reactant is limiting and what mass of each product is expected? (If it is assumed the limiting reactant is completely conusmed? :S please help me!
Asked by Michael M - Sun Mar 2 17:07:06 2008 - - 1 Answers - 0 Comments
A. ALWAYS start with a balanced equation, and then figure the formula weights. Here, we have: 2Al + 6HCl -> 2AlCl3 + 3H2, and the formula weights are 54, 213, 261, and 6. (Verify these.) You don't specify what it is that we have 15 grams of, but suppose that it is the aluminum. To fully react 15 grams of aluminum by this reaction would require 15/54 x 213 grams of HCl. If you have that much or more HCl, the aluminum is limiting. If you have less, the acid is limiting.
Answered by rhsaunders - Sun Mar 2 17:17:58 2008
Q. For Al + HCl --> AlCl^3 + H^2. If 15.0 g of the reactant is taken, how do I determine if the reactant is limiting and what mass of each product is expected? (If it is assumed the limiting reactant is completely conusmed? :S please help me!
Asked by Michael M - Sun Mar 2 17:07:06 2008 - - 1 Answers - 0 Comments
A. ALWAYS start with a balanced equation, and then figure the formula weights. Here, we have: 2Al + 6HCl -> 2AlCl3 + 3H2, and the formula weights are 54, 213, 261, and 6. (Verify these.) You don't specify what it is that we have 15 grams of, but suppose that it is the aluminum. To fully react 15 grams of aluminum by this reaction would require 15/54 x 213 grams of HCl. If you have that much or more HCl, the aluminum is limiting. If you have less, the acid is limiting.
Answered by rhsaunders - Sun Mar 2 17:17:58 2008
What is the limiting reactant for a process?
Q. Why does a reaction stop when the limiting reactant is consumed, even though there may be plenty of the other reactants present?
Asked by DijoLola - Tue Oct 21 13:23:13 2008 - - 2 Answers - 0 Comments
A. The limiting reagent is found by taking the initial amounts of reactants (usually in grams) and using the chemical equation to find out if they are sufficient or too plentiful to react with the other reactants. You do this by using the coefficients of the balanced chemical equation to convert the mass of a given reactant to moles of that reactant to moles of another reactant to grams of that reactant. If it is found that the grams of the first(given) reactant yield more than the given amount of the other reactant (if there are only two) then the second reactant is the limiting reagent because not all of the first one will be consumed in the reaction. If the first one is found using the same stoichiometric calculations to yield less than… [cont.]
Answered by Burney - Tue Oct 21 13:50:11 2008
Q. Why does a reaction stop when the limiting reactant is consumed, even though there may be plenty of the other reactants present?
Asked by DijoLola - Tue Oct 21 13:23:13 2008 - - 2 Answers - 0 Comments
A. The limiting reagent is found by taking the initial amounts of reactants (usually in grams) and using the chemical equation to find out if they are sufficient or too plentiful to react with the other reactants. You do this by using the coefficients of the balanced chemical equation to convert the mass of a given reactant to moles of that reactant to moles of another reactant to grams of that reactant. If it is found that the grams of the first(given) reactant yield more than the given amount of the other reactant (if there are only two) then the second reactant is the limiting reagent because not all of the first one will be consumed in the reaction. If the first one is found using the same stoichiometric calculations to yield less than… [cont.]
Answered by Burney - Tue Oct 21 13:50:11 2008
How would you determine limiting reactant for the following?
Q. When 16.8g of NiS are allowed to react with 81.5gO2, 7.29g NiO are collected. Determine the limiting reactant, theoretical yield of NiO.
Asked by unknown - Tue Mar 24 16:03:54 2009 - - 1 Answers - 0 Comments
A. here's the steps...for all problems of this type. ie.. "memorize the following steps.." 1) write a balanced equation 2) convert everything to moles 3) determine limiting reagent 4) convert moles limiting reagent to moles other species 5) convert moles back to mass.. this is theoretical mass 6) calculate % yield = actual mass / theoretical mass x 100%... here we go... *** 1 *** 2 NiS + 3 O2 ---> 2 NiO + 2 SO2 *** 2 *** moles NiS = 16.8 g x (1 mole / 90.8g) = 0.185 moles moles O2 = 81.5 g x (1 mole / 32.0g) = 2.55 moles *** 3 *** from the balanced equation, 2 moles NiS react with 3 moles O2... 0.185 moles NiS x ( 3 moles O2 / 2 moles NiS) = 0.278 moles O2... so we need 0.278 moles O2 and we have 2.55 moles available. so we have XS O2… [cont.]
Answered by m w - Tue Mar 24 16:40:16 2009
Q. When 16.8g of NiS are allowed to react with 81.5gO2, 7.29g NiO are collected. Determine the limiting reactant, theoretical yield of NiO.
Asked by unknown - Tue Mar 24 16:03:54 2009 - - 1 Answers - 0 Comments
A. here's the steps...for all problems of this type. ie.. "memorize the following steps.." 1) write a balanced equation 2) convert everything to moles 3) determine limiting reagent 4) convert moles limiting reagent to moles other species 5) convert moles back to mass.. this is theoretical mass 6) calculate % yield = actual mass / theoretical mass x 100%... here we go... *** 1 *** 2 NiS + 3 O2 ---> 2 NiO + 2 SO2 *** 2 *** moles NiS = 16.8 g x (1 mole / 90.8g) = 0.185 moles moles O2 = 81.5 g x (1 mole / 32.0g) = 2.55 moles *** 3 *** from the balanced equation, 2 moles NiS react with 3 moles O2... 0.185 moles NiS x ( 3 moles O2 / 2 moles NiS) = 0.278 moles O2... so we need 0.278 moles O2 and we have 2.55 moles available. so we have XS O2… [cont.]
Answered by m w - Tue Mar 24 16:40:16 2009
If equal masses of methane and sulfur are reacted, which reactant is the limiting reactant?
Q. Please help! Heating methane gas, CH4, in the presence of elemental sulfur gives liquid carbon disulfide and hydrogen sulfide gas as the only two products. 1) write the balanced chemical equation 2) if equal masses of methane and sulfure are reacted, which reactant is the limiting reactant? 3) calculated the theoretical yeild, in grams, of carbon disulfide when 120.00g of methane is reacted w/ equal an equal mass of sulfur. please show all work and how to set up equations. Thanks!
Asked by krisg0303 - Sat May 3 14:14:59 2008 - - 1 Answers - 0 Comments
A. Sulfur is the limiting reactant
Answered by Petco Associate - Sat May 3 14:28:39 2008
Q. Please help! Heating methane gas, CH4, in the presence of elemental sulfur gives liquid carbon disulfide and hydrogen sulfide gas as the only two products. 1) write the balanced chemical equation 2) if equal masses of methane and sulfure are reacted, which reactant is the limiting reactant? 3) calculated the theoretical yeild, in grams, of carbon disulfide when 120.00g of methane is reacted w/ equal an equal mass of sulfur. please show all work and how to set up equations. Thanks!
Asked by krisg0303 - Sat May 3 14:14:59 2008 - - 1 Answers - 0 Comments
A. Sulfur is the limiting reactant
Answered by Petco Associate - Sat May 3 14:28:39 2008
What is the limiting reactant in this experiment?
Q. Why? Assume water is the other reactant. The density of methyl salicylate is 1.18 g/mL at 20 degrees Celcius.
Asked by Mz Stormie Lee - Mon Nov 17 17:11:07 2008 - - 2 Answers - 0 Comments
A. you can not find the limiting reactant with these information. you need the amount of each substance that you use in the experiment. then convert the milligram of reactants to mole by using the density that they gave you. after you get the moles, whichever has lower number is limiting reactant.
Answered by soheil z - Mon Nov 17 17:20:43 2008
Q. Why? Assume water is the other reactant. The density of methyl salicylate is 1.18 g/mL at 20 degrees Celcius.
Asked by Mz Stormie Lee - Mon Nov 17 17:11:07 2008 - - 2 Answers - 0 Comments
A. you can not find the limiting reactant with these information. you need the amount of each substance that you use in the experiment. then convert the milligram of reactants to mole by using the density that they gave you. after you get the moles, whichever has lower number is limiting reactant.
Answered by soheil z - Mon Nov 17 17:20:43 2008
How can i prove that phosphoric acid is a catalyst, rather than a reactant?
Q. I have synthesised aspirin from acetic anhydride and salycilic acid and used phosphoric acid as a catalyst for the reaction. I have been asked to prove that phosphoric acid is a catalyst not a reactant; how could i do this?
Asked by Matt - Mon May 18 08:24:31 2009 - - 1 Answers - 0 Comments
A. The simplest way would be to remove the aspirin product and then introduce new reactants without phosphoric acid. If the acid was a reactant, then it would have been used up in the first run. If you still get the normal level of product, it was a catalyst. Otherwise you're looking at doing analysis for P.
Answered by tinman97prn - Mon May 18 08:31:45 2009
Q. I have synthesised aspirin from acetic anhydride and salycilic acid and used phosphoric acid as a catalyst for the reaction. I have been asked to prove that phosphoric acid is a catalyst not a reactant; how could i do this?
Asked by Matt - Mon May 18 08:24:31 2009 - - 1 Answers - 0 Comments
A. The simplest way would be to remove the aspirin product and then introduce new reactants without phosphoric acid. If the acid was a reactant, then it would have been used up in the first run. If you still get the normal level of product, it was a catalyst. Otherwise you're looking at doing analysis for P.
Answered by tinman97prn - Mon May 18 08:31:45 2009
Does changing the volume of a reactant affect the rate of the reaction?
Q. This is assuming that when you lower the volume, this reactant is still in excess, and all other factors, such as concentration, surface area and temperature are kept constant. N.B. the reactant in question is a liquid
Asked by SB1 - Sun Feb 15 05:58:45 2009 - - 2 Answers - 0 Comments
Q. This is assuming that when you lower the volume, this reactant is still in excess, and all other factors, such as concentration, surface area and temperature are kept constant. N.B. the reactant in question is a liquid
Asked by SB1 - Sun Feb 15 05:58:45 2009 - - 2 Answers - 0 Comments
Which is the limiting reactant and how many grams of the product will be formed in the reaction?
Q. A 20 g sample of Sulfur is mixed with 160 g of oxygen. Which is the limiting reactant and how many grams of the product will be formed in the reaction? For the same reaction, which is the limiting reactant if now we use 20g of Sulfur mixed with 15.0 g of oxygen? How many grams of the product will be formed in the reaction? please help me! thank you!
Asked by jobajeterarod - Thu Jun 4 10:39:04 2009 - - 1 Answers - 0 Comments
A. S (s) + O2 (g) SO2 (g) Atomic mass of S is 32 g/mole, and molecular mass of O2 is 32 g/mole. The number of moles of S is: (20 g) / (32 g/mole) = 0.625 moles The number of moles of O2 is: (160 g) (32 g/mole) = 5 moles O2. Since the reagents react in a 1:1 mole ratio, all of the S and 0.625 moles of the O2 react; the rest of the O2 is unreacted and S is the limiting reagent. Therefore we can expect no more than 0.625 moles of SO2 product: (0.625 moles) (64 g/mole) = 40 g of SO2. If we use 15 g of O2, then (15 g) / (32 g/mole) = 0.469 moles of O2. This time, S is the limiting reagent, and we expect (0.469 moles) (64 g/mole) = 30 g of SO2 as product.
Answered by Blah D. - Fri Jun 5 14:37:42 2009
Q. A 20 g sample of Sulfur is mixed with 160 g of oxygen. Which is the limiting reactant and how many grams of the product will be formed in the reaction? For the same reaction, which is the limiting reactant if now we use 20g of Sulfur mixed with 15.0 g of oxygen? How many grams of the product will be formed in the reaction? please help me! thank you!
Asked by jobajeterarod - Thu Jun 4 10:39:04 2009 - - 1 Answers - 0 Comments
A. S (s) + O2 (g) SO2 (g) Atomic mass of S is 32 g/mole, and molecular mass of O2 is 32 g/mole. The number of moles of S is: (20 g) / (32 g/mole) = 0.625 moles The number of moles of O2 is: (160 g) (32 g/mole) = 5 moles O2. Since the reagents react in a 1:1 mole ratio, all of the S and 0.625 moles of the O2 react; the rest of the O2 is unreacted and S is the limiting reagent. Therefore we can expect no more than 0.625 moles of SO2 product: (0.625 moles) (64 g/mole) = 40 g of SO2. If we use 15 g of O2, then (15 g) / (32 g/mole) = 0.469 moles of O2. This time, S is the limiting reagent, and we expect (0.469 moles) (64 g/mole) = 30 g of SO2 as product.
Answered by Blah D. - Fri Jun 5 14:37:42 2009
How do you determine theoretically the limiting reactant?
Q. Im having trouble figuring out this answer It states consider the msses of the starting materials ( which are nails before the reaction 1.5413 grams and Solid copper (II) chloride 2.50 grams) to determine theoretically the limiting reactant. If someone would help me that would be great
Asked by Zeinab - Thu Jun 4 00:18:43 2009 - - 2 Answers - 0 Comments
A. Good ole' chemistry lol What you want to do is convert the amounts into moles and then look at the actual reaction and do mole ratios. Which ever one is less is going to be the limiting reagent Hopefully this helps sorry I couldn't be more specific I don't have the rxn
Answered by michaelmuoio@sbcglobal.net - Thu Jun 4 00:25:14 2009
Q. Im having trouble figuring out this answer It states consider the msses of the starting materials ( which are nails before the reaction 1.5413 grams and Solid copper (II) chloride 2.50 grams) to determine theoretically the limiting reactant. If someone would help me that would be great
Asked by Zeinab - Thu Jun 4 00:18:43 2009 - - 2 Answers - 0 Comments
A. Good ole' chemistry lol What you want to do is convert the amounts into moles and then look at the actual reaction and do mole ratios. Which ever one is less is going to be the limiting reagent Hopefully this helps sorry I couldn't be more specific I don't have the rxn
Answered by michaelmuoio@sbcglobal.net - Thu Jun 4 00:25:14 2009
What is the mass of each reactant and product for the equation as balanced?
Q. CH4+O2--->CO2+H2O Assume the following atomic masses: H=1amu C=12amu O=16amu What is the mass of each reactant and product for the equation as balanced: 1. CH4 2. O2 3. H2O 4.CO2 What is the total mass of All reactants All products
Asked by Independent and Strong - Wed Jul 29 01:33:53 2009 - - 1 Answers - 0 Comments
A. CH4 + O2 ---> CO2 + H2O CH4 + 2O2 ---> CO2 + 2H2O .. 1. CH4 = 12 + (4 * 1) = 16 2. 2O2 = 2 * (2 * 16) = 64 3. 2H2O = 2 * ((2 * 1) + 16) = 36 4. CO2 = 12 + (2 * 16) = 44 .. reactants = 16 + 64 = 80 products = 36 + 44 = 80 .. here, u can see that the mass of reactants and products is always the same.
Answered by FreaK - Wed Jul 29 01:48:12 2009
Q. CH4+O2--->CO2+H2O Assume the following atomic masses: H=1amu C=12amu O=16amu What is the mass of each reactant and product for the equation as balanced: 1. CH4 2. O2 3. H2O 4.CO2 What is the total mass of All reactants All products
Asked by Independent and Strong - Wed Jul 29 01:33:53 2009 - - 1 Answers - 0 Comments
A. CH4 + O2 ---> CO2 + H2O CH4 + 2O2 ---> CO2 + 2H2O .. 1. CH4 = 12 + (4 * 1) = 16 2. 2O2 = 2 * (2 * 16) = 64 3. 2H2O = 2 * ((2 * 1) + 16) = 36 4. CO2 = 12 + (2 * 16) = 44 .. reactants = 16 + 64 = 80 products = 36 + 44 = 80 .. here, u can see that the mass of reactants and products is always the same.
Answered by FreaK - Wed Jul 29 01:48:12 2009
Can energy count as a reactant or product in a chemical reaction?
Q. For example, if my chemical reaction is C2H6 + heat --> C2H4 + H2 is heat considered a reactant?
Asked by giligy - Tue Feb 10 21:29:40 2009 - - 1 Answers - 0 Comments
A. Yes, energy is needed for the reaction to take place. So it's taken from the surroundings and ends up stored in the products.
Answered by srvevh1 - Tue Feb 10 21:35:12 2009
Q. For example, if my chemical reaction is C2H6 + heat --> C2H4 + H2 is heat considered a reactant?
Asked by giligy - Tue Feb 10 21:29:40 2009 - - 1 Answers - 0 Comments
A. Yes, energy is needed for the reaction to take place. So it's taken from the surroundings and ends up stored in the products.
Answered by srvevh1 - Tue Feb 10 21:35:12 2009
how many moles of each reactant and product?
Q. I am horrible with chemistry please can someone help me. Using the information given by a chemical equation: How many moles of each reactant and product?
Asked by Laura - Sat Jun 13 00:23:52 2009 - - 1 Answers - 0 Comments
A. You look at the coefficient of each reactant or product in the balanced chemical equation to get the ratio of reactants or products to one another. Ba(OH)2 --> Ba(2+) + 2OH(-) The coefficients are 1, 1, and 2 respectively meaning that for every mol of Barium hydroxide (Ba(OH)2), there is one mole of Ba2+ ions formed and 2 moles of OH- ions formed. Hope this somewhat answers your question, it was somewhat vague.
Answered by tishermanr - Sat Jun 13 00:34:02 2009
Q. I am horrible with chemistry please can someone help me. Using the information given by a chemical equation: How many moles of each reactant and product?
Asked by Laura - Sat Jun 13 00:23:52 2009 - - 1 Answers - 0 Comments
A. You look at the coefficient of each reactant or product in the balanced chemical equation to get the ratio of reactants or products to one another. Ba(OH)2 --> Ba(2+) + 2OH(-) The coefficients are 1, 1, and 2 respectively meaning that for every mol of Barium hydroxide (Ba(OH)2), there is one mole of Ba2+ ions formed and 2 moles of OH- ions formed. Hope this somewhat answers your question, it was somewhat vague.
Answered by tishermanr - Sat Jun 13 00:34:02 2009
How do you find the limiting reactant when given moles?
Q. I know how to find this if it was given in grams, but im a bit confused on how to answer this problem when given moles. Zn + 2HCl ---> ZnCl2 + H2 If 4.50 moles of Zinc reacts with 6.00 moles of hydrochloric acid, what is the limiting reactant? how many grams of zinc chloride will be produced?
Asked by bluedolfinswimmer13 - Tue Nov 17 20:49:04 2009 - - 0 Answers - 0 Comments
Q. I know how to find this if it was given in grams, but im a bit confused on how to answer this problem when given moles. Zn + 2HCl ---> ZnCl2 + H2 If 4.50 moles of Zinc reacts with 6.00 moles of hydrochloric acid, what is the limiting reactant? how many grams of zinc chloride will be produced?
Asked by bluedolfinswimmer13 - Tue Nov 17 20:49:04 2009 - - 0 Answers - 0 Comments
What happens to a reaction at equilibrium when more reactant is added to the system?
Q. What happens to a reaction at equilibrium when more reactant is added to the system? a. the reaction makes more products b. the reaction makes more reactants c. the reaction is unchanged d. the answer cannot be determined
Asked by zerokun4 - Mon May 28 10:53:38 2007 - - 2 Answers - 0 Comments
A. When you change a system that is in equilibrium, the system will shift in order to regain equilibrium again. So if more reactant is added to the system, the other side of teh equation will react by making more products in order to achieve balance again.
Answered by Carolyn R - Mon May 28 11:02:19 2007
Q. What happens to a reaction at equilibrium when more reactant is added to the system? a. the reaction makes more products b. the reaction makes more reactants c. the reaction is unchanged d. the answer cannot be determined
Asked by zerokun4 - Mon May 28 10:53:38 2007 - - 2 Answers - 0 Comments
A. When you change a system that is in equilibrium, the system will shift in order to regain equilibrium again. So if more reactant is added to the system, the other side of teh equation will react by making more products in order to achieve balance again.
Answered by Carolyn R - Mon May 28 11:02:19 2007
Which reactant in the following equation is the reducing agent?
Q. 1. Which reactant in the following equation is the reducing agent? 2H+(aq) + Mg(s) --> Mg2+(aq) + H2(g) 2. Which reactant in the following equation is being oxidized? Cu(s) + 2Ag+(aq) --> 2Ag(s) + Cu2+(aq) 3. Which reactant in the following equation is being oxidized? CO(g) + 2H2(g) --> CH3OH(g)
Asked by spottedfrog99 - Sat Jul 5 22:33:49 2008 - - 5 Answers - 0 Comments
A. LEO-GER Lose electrons = oxidized, gain electrons = reduced 2H+ --> H2 (you LOSE electrons, so the Hydrogen is being reduced; thus, Mg is the oxidizing agent and H is the reducing agent) Try the others see if you can get them :)
Answered by THE nerd. - Sat Jul 5 22:39:06 2008
Q. 1. Which reactant in the following equation is the reducing agent? 2H+(aq) + Mg(s) --> Mg2+(aq) + H2(g) 2. Which reactant in the following equation is being oxidized? Cu(s) + 2Ag+(aq) --> 2Ag(s) + Cu2+(aq) 3. Which reactant in the following equation is being oxidized? CO(g) + 2H2(g) --> CH3OH(g)
Asked by spottedfrog99 - Sat Jul 5 22:33:49 2008 - - 5 Answers - 0 Comments
A. LEO-GER Lose electrons = oxidized, gain electrons = reduced 2H+ --> H2 (you LOSE electrons, so the Hydrogen is being reduced; thus, Mg is the oxidizing agent and H is the reducing agent) Try the others see if you can get them :)
Answered by THE nerd. - Sat Jul 5 22:39:06 2008
How do you figure out the Limiting Reactant and Moles consumed?
Q. For the equation: HCl+NaOH=NaCl+H2O If 9mL of 1.01M HCl are mixed with 10mL of 0.992M NaOH: a) What is the Limiting Reactant? b)How many moles of HCl will be consumed?
Asked by Daniel C - Sat Oct 17 18:09:08 2009 - - 2 Answers - 0 Comments
A. Work out the moles of each: HCl n=concentration*volume=1. 01*0.009 = 0.00909mol NaOH n=0.992*0.01 = 0.00992mol As you can see, HCl has the least moles in the reaction and so will be the limiting reactant. All 0.00909mol of HCl will be used up, as the reaction will only stop once it is depleted (by definition of being limiting reactant)
Answered by unknown - Sat Oct 17 18:39:57 2009
Q. For the equation: HCl+NaOH=NaCl+H2O If 9mL of 1.01M HCl are mixed with 10mL of 0.992M NaOH: a) What is the Limiting Reactant? b)How many moles of HCl will be consumed?
Asked by Daniel C - Sat Oct 17 18:09:08 2009 - - 2 Answers - 0 Comments
A. Work out the moles of each: HCl n=concentration*volume=1. 01*0.009 = 0.00909mol NaOH n=0.992*0.01 = 0.00992mol As you can see, HCl has the least moles in the reaction and so will be the limiting reactant. All 0.00909mol of HCl will be used up, as the reaction will only stop once it is depleted (by definition of being limiting reactant)
Answered by unknown - Sat Oct 17 18:39:57 2009
What is the half-life of the reactant in seconds?
Q. The reaction 2N2O5 ==> 4NO2+O2 is the first order type. The rate constant is k=3.38 x 10-5 1/s. What is the half-life of the reactant in seconds?
Asked by Success - Sun Aug 2 16:09:00 2009 - - 1 Answers - 0 Comments
A. half-life = ln 2 / (rate constant)
Answered by Filpi - Sun Aug 2 17:21:37 2009
Q. The reaction 2N2O5 ==> 4NO2+O2 is the first order type. The rate constant is k=3.38 x 10-5 1/s. What is the half-life of the reactant in seconds?
Asked by Success - Sun Aug 2 16:09:00 2009 - - 1 Answers - 0 Comments
A. half-life = ln 2 / (rate constant)
Answered by Filpi - Sun Aug 2 17:21:37 2009
Can physical observation during a chemical reaction support the fact that one reactant is limiting?
Q. I did this experiment with Iron 2 and Iron 3 and CuSO4. for each iron in the reaction, the limiting reactant is different. Can our observation of physical change during the experiment support the fact that one reactant is limiting?
Asked by Goli - Tue Oct 14 10:01:51 2008 - - 2 Answers - 0 Comments
A. Yes some times it is possible. The reaction is: Fe + CuSO4 (blue) ---> Cu + FeSO4 (light green) When Fe is added to a solution of CuSO4 (blue). 1. After some time it is observed that all the iron has disappeared but solution is still blue. it means that Fe is a limiting reagent and CuSO4 is still available. 2. After some time some iron is still available and blue colour has disappeared (some very light green colour of FeSO4 may be visible). It indicates that CuSO4 is the limiting reagent and Fe is still available.
Answered by trikha - Tue Oct 14 10:26:43 2008
Q. I did this experiment with Iron 2 and Iron 3 and CuSO4. for each iron in the reaction, the limiting reactant is different. Can our observation of physical change during the experiment support the fact that one reactant is limiting?
Asked by Goli - Tue Oct 14 10:01:51 2008 - - 2 Answers - 0 Comments
A. Yes some times it is possible. The reaction is: Fe + CuSO4 (blue) ---> Cu + FeSO4 (light green) When Fe is added to a solution of CuSO4 (blue). 1. After some time it is observed that all the iron has disappeared but solution is still blue. it means that Fe is a limiting reagent and CuSO4 is still available. 2. After some time some iron is still available and blue colour has disappeared (some very light green colour of FeSO4 may be visible). It indicates that CuSO4 is the limiting reagent and Fe is still available.
Answered by trikha - Tue Oct 14 10:26:43 2008
How many grams of the excess reactant is left?
Q. 4NH3 + 5O2 ===>4NO + 6H2O 1.85 g of NH3 reacts with 3.39 g of O2. O2 is the limiting reactant. how many grams of NO and H2O form? How many grams of the excess reactant remain after the limiting reactant is completely consumed? Please help ! I don't know what I'm doing wrong...! please tell me how you got your answer-- thanks!
Asked by J-Walker - Wed Sep 16 17:20:28 2009 - - 4 Answers - 0 Comments
A. moles of NH3 = 1.85/17 = 0.1088 moles of O2 = 3.39/32 = 0.1059 (limiting reactant) 4NH3 + 5O2 ===>4NO + 6H2O NO formed = 4/5*moles of O2 = 4/5*0.1059 = 0.0847 moles grams of NO = 0.0847*30 = 2.54 grams H2O formed = 6/5*moles of O2 = 0.127 moles grams of H2O = 0.127*18 = 2.287 grams NH3 reacted = 4/5*moles of O2 = 0.087 moles excess of NH3 = 0.1088 - 0.087 = 0.0218 moles = 0.0218*17 = 0.37 grams.
Answered by abdee1 - Wed Sep 16 17:37:21 2009
Q. 4NH3 + 5O2 ===>4NO + 6H2O 1.85 g of NH3 reacts with 3.39 g of O2. O2 is the limiting reactant. how many grams of NO and H2O form? How many grams of the excess reactant remain after the limiting reactant is completely consumed? Please help ! I don't know what I'm doing wrong...! please tell me how you got your answer-- thanks!
Asked by J-Walker - Wed Sep 16 17:20:28 2009 - - 4 Answers - 0 Comments
A. moles of NH3 = 1.85/17 = 0.1088 moles of O2 = 3.39/32 = 0.1059 (limiting reactant) 4NH3 + 5O2 ===>4NO + 6H2O NO formed = 4/5*moles of O2 = 4/5*0.1059 = 0.0847 moles grams of NO = 0.0847*30 = 2.54 grams H2O formed = 6/5*moles of O2 = 0.127 moles grams of H2O = 0.127*18 = 2.287 grams NH3 reacted = 4/5*moles of O2 = 0.087 moles excess of NH3 = 0.1088 - 0.087 = 0.0218 moles = 0.0218*17 = 0.37 grams.
Answered by abdee1 - Wed Sep 16 17:37:21 2009
Explain how one determines which reactant in a process is the limiting reactant.?
Q. Explain how one determines which reactant in a process is the limiting reactant. Does this depend only on the masses of the reactant present?
Asked by DijoLola - Sun Oct 19 02:20:15 2008 - - 4 Answers - 0 Comments
A. the one that runs out first, it depends on the number of moles present
Answered by jonno - Sun Oct 19 02:43:37 2008
Q. Explain how one determines which reactant in a process is the limiting reactant. Does this depend only on the masses of the reactant present?
Asked by DijoLola - Sun Oct 19 02:20:15 2008 - - 4 Answers - 0 Comments
A. the one that runs out first, it depends on the number of moles present
Answered by jonno - Sun Oct 19 02:43:37 2008
From Yahoo Answer Search: 'reactant'
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Trading Markets (press release)
On Wednesday, the company put out news announcing that it signed a worldwide exclusive licensing agreement for a Mixed Reactant Fuel Cell (MRFC) technology ...
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cdsanalytical.com
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Model 5200 Reactant Gas Pyrolysis System Contact Gary Deger CDS Analytical Inc Date February 2005
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freepatentsonline.com: Nanotechnology
ue, 15 Sep 2009 12:00:00 GM
a method includes producing an isolation atmosphere in a phase changing area above a . reactant. liquid and then injecting a feed material into the . reactant. liquid. the feed material preferably comprises a quantity of a hydrocarbon ...
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