calculate the enthalpy change in kJ when 27.2 of hydrogen sulfide is burned?
Q. 2H2S(g) + 3O2(g) ---> 2SO2(g) + 2H2O(g) delta H: -1036 kJ/mol what steps do i use to find the answer? THNK YOU!
Asked by doahgolfer - Sun Nov 8 20:24:22 2009 - - 1 Answers - 0 Comments

A. Enthalpy change of a reaction is equal to delta H of all the products minus that of the reactants. You can probably find the delta H values for the products and reactants in a chemistry textbook or on the internet somewhere.
Answered by timmeh37 - Sun Nov 8 20:36:58 2009

what color does hydrogen sulphide burn, if it does?
Q. what color does hydrogen sulphide burn, if it does?
Asked by Grapies07 - Tue Jul 3 19:51:07 2007 - - 3 Answers - 0 Comments

A. It will burn in an oxygen rich atmosphere with a blue flame, and produces heat, water, and sulfur dioxide gas.
Answered by nyninchdick - Tue Jul 3 19:57:21 2007

I need help with a chemical equation?
Q. Hydrogen sulfide burns in oxygen to produce water and sulfur dioxide, 2H2S(g) + 3O2(g) = 2H2O(g) + 2SO2(g) ho do i work out how much oxygen is required to produce 6.4g of sulfur dioxide?
Asked by Siobhan K - Fri Apr 25 22:01:57 2008 - - 2 Answers - 0 Comments

What is the answer to this question?
Q. Hydrogen Sulfide, H2S, is a foul-smelling gas which burns to form sulfer dioxide. Calculate the enthalpy change in kJ when 12.2g of hydrogen sulfide is burned.
Asked by ifeanyiboy23 - Tue Dec 8 05:15:34 2009 - - 1 Answers - 0 Comments

A. Nice question. But the data is not sufficient to solve this question. Please check it out from your end so that needful can be done at the earliest. delta H = [delta H of products - delta H of reactants.] Delta H values must be given in your text books. These values are given for one mole. you need to calculate the moles of H2S for the given mass that is 12.2 g and then multiply the delta H value with it's number of moles. At the same time you need to know how many moles of each of the product will be there. H2S ---> H2 + S It is clear from the balanced reaction that 1 mole of H2S gives 1 mole H2 and 1 mole of S. that means there is 1:1:1 mole ratio. and hence the moles of H2 and S will be same as the moles of H2S in it's 12.2 g. … [cont.]
Answered by amit m - Tue Dec 8 05:38:14 2009

questions for balancing chemical reaction.?
Q. convert the ff description of reactions into balanced equations: 1. in a gaseous reaction, hydrogen sulfide burns in oxygen to form sulfur dioxide and water vapor. 2. when crystalline potassium chlorate is heated to just above its melting point, it reacts to form two different crystalline compounds, potassium chloride and potassium perchlorate. 3. when hydrogen gas is passed over powdered iron (III) oxide, iron metal and water vapor form. 4. the combustion of gaseous ethane in air forms carbon dioxide and water vapor. 5. Iron (III) chloride is converted to iron (III) flouride by treatment with chlorine triflouride gas. Chlorine gas is also formed.
Asked by semi_sonic3 - Wed Oct 3 10:11:07 2007 - - 1 Answers - 1 Comments

A. 1) Balanced equation: 2H2S + 3O2 + heat ---> 2SO2 + 2H2O(g) 2) Balanced equation: 4KClO3 + heat ---> KCl + 3KClO4 3) Balanced equation: 3H2(g) + Fe2O3 ---> 2Fe + 3H2O 4) Balanced equation: 2C2H6 + 7O2 ---> 4CO2 + 6H2O 5) Balanced equation: 2FeCl3 + 2ClF3 ---> 2FeF3 + 4Cl2(g) That's it!
Answered by CHESSLARUS - Wed Oct 3 10:43:59 2007

Help me with my chemistry (grade 9) homework?
Q. How would I write these as a balanced equation. I know how to balance equations, but not when they are in paragraph form. I get really confused. Can anyone help me? 1. Magnesium hydroxide has been used for many years as an antacid ("milk of magnesia") because it reacts with the hydrochloric acid in the stomach, producing magnesium chloride and water. Write the balance chemical equation for this process. 2. Nitrous oxide gas (systemic name: dinitrogen monoxide) is used by some dentists as an anesthetic. Nitrous oxide (and water vapor) can be produced in small amounts in the laboratory by careful heating of ammonium nitrate. Write the balanced chemical equation for this reaction. 3. Hydrogen sulfide gas is responsible for the odor of… [cont.]
Asked by :) - Sun Jan 17 16:25:17 2010 - - 3 Answers - 0 Comments

Can you check my answers for some chemistry questions? Can you correct the ones I get wrong?
Q. 6. Silver will dissolve in concentrated nitric acid, producing NO gas and leaving a solution of silver nitrate in water. Write the unbalanced chemical equation for this process. A. Ag (s) + HNO3 (aq) ---> NO (g) + AgNO3 (aq) 7. Calcium carbonate reacts by combining with hydrochloric acid, producing a solution of calcium chloride, converting the acid into water, and releasing carbon dioxide gas. Write the unbalanced chemical equation for this process. A. CaCO3 (g) + HCl (aq) ---> CaCl2 (aq) + CO2 8. Hydrogen sulfide burns in air, producing sulfur dioxide gas and water vapor. Write the unbalanced chemical equation for this process. A. H2S (g) ---> SO2 (g) + H2O (g) 9. The group 2 metals (Ba, C, Sr) can be produced in elemental state… [cont.]
Asked by sgtleo1995 - Fri Dec 28 13:38:11 2007 - - 2 Answers - 0 Comments

A. 6. Ag (s) + HNO3 (aq) ---> NO (g) + AgNO3 (aq) + H2O 7. CaCO3 (s) + HCl (aq) ---> CaCl2 (aq) + CO2 + H2O Calcium carbonate is usually a solid. 9. Oxides are basically compounds with oxygen in it (e.g.: BaO, NO) BaO + Al --> Ba + Al2O3 CaO + Al --> Ca + Al2O3 SrO + Al --> Sr + Al2O3
Answered by /\/ ? - Fri Dec 28 13:47:51 2007

How do I form this equation and predict the volume?
Q. Some sulfur compounds are undesirable components of much of Alberta's fossil fuels. For example Sour natural gas contains Hydrogen Sulfide in varying proportions. One technology for removing hydrogen sulfide from sour natural gas involves converting part of the hydrogen sulfide to sulfur dioxide by burning it in air. Predict the volume of oxygen required to burn 124 kL of hydrogen sulfide measured at the same temperature and pressure?
Asked by Legato T - Sat Jul 12 18:12:13 2008 - - 1 Answers - 0 Comments

A. Equation for the reaction is: 2H2S + 3O2 2H2O + 2SO2 Every 2 moles of H2S require 3 moles of molecular oxygen (O2) for complete combustion. At the same temperature & pressure all gases contain the same number of molecules, so 124 kiloliters of hydrogen sulfide will require 1 times that volume of oxygen, or 186 kiloliters, to burn completely. Hope this answers your question.
Answered by Reginald - Sat Jul 12 19:01:26 2008

Enthalpy Change?
Q. Hydrogren Sulfide, H2S, is a foul-smelling gas, which burns to form sulfur dioxide. 2H2S(g) + 3O2(g) --> 2SO2(g) + 2H2O(g) delta H= -1036 kJ/mol Calculate the enthalpy change in kJ when 11.3 g of hydrogen sulfide is burned.
Asked by Pink_gixxie_chick - Sun Oct 7 12:22:43 2007 - - 1 Answers - 0 Comments

A. Determine how many moles are in 11.3 g of H2S. Multiple this by H to get the amount of energy released.
Answered by Lance - Wed Oct 10 22:43:48 2007

Help with homework please!!!!!!!!?
Q. give the reactions for these and balance: Hydrogen gas and iodine solid are reacted Aluminum iodide and chlorine gas are reacted hydrogen sulfide gas burns with oxygen gas propane gass is burned in air cesium phosphate is added to barium chloride platinum is added to a solution of lead(II) nitrate
Asked by ren - Tue Mar 17 23:28:30 2009 - - 1 Answers - 0 Comments

A. Try to post this in the Chemistry section.
Answered by iceman - Tue Mar 17 23:35:49 2009

chemistry help?
Q. Write a balanced equation for the reaction of hydrogen sulfide, H2S, with oxygen, O2, forming sulfur dioxide, SO2, and water. List the bonds broken and the bonds formed in the reaction. Then, based upon the bond energies listed below (not all may be needed), calculate the energy released when 47.8 grams of hydrogen sulfide is burned in oxygen. Enter the energy released, in kJ, as a positive number without units. S-S 226kJ/mol O-O 498kJ/mol S-O 398kJ/mol S-H 339kJ/mol O-H 463kJ/mol
Asked by bloooper28 - Sat Oct 6 00:45:56 2007 - - 1 Answers - 0 Comments

A. Since S-H bonds are broken, it takes energy to break the bonds. Also O-O bonds are broken. The products create S-O bonds and O-H bonds, which release energy. After you find out how many moles of H2S are in 47.8 g, you would determine how many bonds of each type need to be broken and how many are formed. From this you can determine the energy released (or needed) for the reaction.
Answered by Lance - Tue Oct 9 22:45:49 2007

How would anyone figure this question out?
Q. An industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas. In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g) + 3O2(g) ==> 2H2O(l) + 2SO2(g); DeltaHo = -1125 kJ The density of sulfur dioxide at 25oC and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/(mol x oC). A.) How much heat (in kJ) would be evolved in producing 1.00 L of SO2 at 25oC and 1.00 atm? B.) Suppose heat from this reaction is used to heat 1.00 L of SO2 from 25oC and 1.00 atm to 483oC for its use in the next step of the process. What percentage of the heat evolved is required for this?
Asked by Joe C. - Thu Oct 18 01:21:24 2007 - - 2 Answers - 0 Comments

A. Part A: you know from the density of SO2 that 1 l at 25C and 1 atm is 2.62 g of SO2. So convert this to mol of SO2: 2.62 g x (1 mol/64 g) = 0.041 mol of SO2 The delta H is -1125 kJ/mol so the heat eveloved would be: 0.041 mol * 1125 kJ/mol = 46.1 kJ Part B: To figure this out you need to determine the amount of heat required to raise the temp from 25 C to 483 C. To do this use the heat capacity and the delta T: delta T = (483-25) = 458 C 458 C * 0.0302 kJ/(mol*C) = 13.8 kJ/mol and since you are heating 0.041 mol: 13.8 kJ/mol * 0.041 mol = 0.57 kJ are required to heat this amount of SO2 from 25 c to 483 C. To get the percentage: (0.57/46.1)*100 = 1.23%
Answered by lateda1000 - Thu Oct 18 02:05:13 2007

What are the answers to these stoichiometry problems (AS Level Chemistry)?
Q. 1) 100 cm3 was reacted with 500 cm3 of oxygen. What is the total volume of the gases at the end? (Please indicate how much there is of each gas) CH4 (g) + 2 O2 (g) --> CO2 (g) + 2 H2O (l) 2) If 4dm3 of hydrogen sulphide is burned in 10dm3 of oxygen, what is the final volume of the mixture? (Provide the volume of each gas at the end) 2 H2S (g) + 3 O2 (g) --> 2 H2O (g) + 2 SO2 (g)
Asked by mizzromi - Sun Sep 28 17:22:14 2008 - - 1 Answers - 0 Comments

A. First determine the limiting reagent: 100 cm^3 CH4 x 1 m^3/(1000 cm^3) x 1000 L/1m^3 = 0.1 L CH4 0.1 L CH4 x (1 mole/22.4 L) = 0.00446 mole CH4 Same process for O2 ---> 0.02232 mole O2 Thus, CH4 is the limiting reagent. 0.00446 mole CH4 x 1 mole CO2/1 mole CH4 x 22.4 L/1 mole = 0.099904 liter CO2 same process for amount of H20, ... 0.199808 Liter H20 add together to get total volume of gases created. convert back to cm^3 if you have to
Answered by Dr. Fell - Sun Sep 28 17:49:55 2008

Is it safe to leave candles burning in the bedroom,?
Q. When your husband lets f@1$ that blow you out of bed? I hear hydrogen sulfide is flammable.
Asked by little big mama - Thu Nov 19 15:12:26 2009 - - 4 Answers - 0 Comments

A. Oh My God! Never leave burning candles unattended in any room of the house...least of all the bedroom where most things are easily flammable and hard to extinguish like mattresses, pillows etc. Not to mention your husbands back-door bombs!!!.
Answered by Brainz - Thu Nov 19 16:10:21 2009

I am still having a hard times figuring these chemical mathmatics out please help?
Q. I am also having a hard figuring out the moles for the formulas please help. Question 11: How many grams of zinc chloride are produced when 3255 grams of zinc react with hydrochloric acid? Question 12: How many grams of hydrogen are produced by the action of hydrochloric acid on 50 grams of zinc? Question 13: How many grams of copper oxide may be reduced by 10 grams of hydrogen? Question 14: How many grams of sodium chloride are required to react with 196 grams of H2SO4? Question 15: How many grams of mercuric oxide are needed to produce 100 liters of O2? Question 16: How many grams of zinc are needed to produce 100 liters of hydrogen by acid replacement? Question 17: How many liters of hydrogen are needed to reduce 120… [cont.]
Asked by Shinoda - Sat Dec 2 22:13:56 2006 - - 1 Answers - 0 Comments

A. I don't think too many folks on here are going to flat-out do your homework for you. (Darn...) Have you checked out the Stoichiometry section of your text? That should shed some light on most of these.
Answered by unknown - Sat Dec 2 22:25:19 2006

Chemhelp?- energy change ?
Q. a waste heat exchanger is used to absorb the energy form the complete combustion of hydrogen sulfide gas. What volume of water undergoing a temperature change of 64 degrees is required to absorb all the energy form the burning of 15kg of hydrogen sulfide? i dont need to have the answer i just dont know how to formulate what is being asked?
Asked by Steph - Mon Dec 1 12:24:20 2008 - - 1 Answers - 0 Comments

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

write chemical equations for these reactions.?
Q. a. when solid naphthalene (C10H8) burns in air, the products are gaseous carbon dioxide and liqid water. b. bubbling hydrogen sulfide gas through manganese(II) chloride dissolved in water results in the formation of the precipitate manganese (II) sulfide and hydrochloric acid. c. Solid mangnesium reacts with nitrogen gas to produce solid magnesium nitride. d. Heating oxygen difluoride gas yields oxygen gas and fluorine gas.
Asked by esperanza_lea - Tue Feb 12 01:55:11 2008 - - 1 Answers - 0 Comments

A. a) C10H8(s) + 12O2(g) ===> 10CO2(g) + 4H2O(g) b) H2S(g) + MnCl2(aq) ===> MnS(s) + 2HCl(aq) c) 3Mg(s) + N2(g) ===> Mg3N2(s) ( i think this is correct) d) 2OF2(g) ===> O2(g) + 2F2(g)
Answered by Michael E - Tue Feb 12 02:09:31 2008

Write chemical equations for these reactions?
Q. A and B have 7 empty spaces. C and D have 5 empty spaces. (a) When solid naphthalene (C10H8) burns in air, the products are gaseous carbon dioxide and liquid water. C10H8(s) + (g) (g) + (l) (b) Bubbling hydrogen sulfide gas through manganese(II) chloride dissolved in water results in the formation of the precipitate manganese(II) sulfide and hydrochloric acid. (g) + (aq) (s) + HCl(aq) (c) Solid magnesium reacts with nitrogen gas to produce solid magnesium nitride. (s) + N2(g) (s) (d) Heating oxygen difluoride gas yields oxygen gas and fluorine gas. (g) (g) + F2(g)
Asked by Shorty - Wed Mar 5 16:46:47 2008 - - 1 Answers - 0 Comments

A. (a) C10H8 + 12 O2 = 10 CO2 + 4 H2O
Answered by wise owl - Wed Mar 5 16:56:19 2008

Standard enthalpies chemistry question?
Q. 1)Hydrogen sulfide gas is a poisonous gas with the odor of rotten eggs. It occurs in natural gas and is produced during the decay of organic matter, which contains sulfur. The gas burns in oxygen as follow: 2H2S(g)+3O2(g)->2H2O(l)+2 SO2(g) Calculate the standard enthalpy change for this reaction using standard enthalpies of formation. Okay so here is my work after using the standard enthalpy chart to determine the Hf 2H2S(g)=-20.5 kJ/mol 3O2(g)=0 kJ/mol 2H2O(l)=285.8 kJ/mol 2SO2(g)-296.8 kJ/mol I put them into the reaction H = ( Hf products) - ( Hf reactants) which looked like this: H =(2molH2O 285.8/1)+(2molSO2 (-296.8)/1)- (2molH2S -20.5/1)+(3molO2 0/1) =19kJ/mol But the answer is supposed to be -1124.2kJ, can anyone tell me… [cont.]
Asked by Gweedo8 - Thu Jun 25 14:16:14 2009 - - 1 Answers - 0 Comments