Question 33Read the information below about the Orica ammonia plant in Newcastle.The city of Newcastle is the second most populated area in the Australian state of NewSouth Wales. Located at the mouth of the Hunter River, it is one of the largest coalexporting harbours in the world.The company Orica is one of the world's largest providers of commercial explosives andinnovative blasting systems to the mining, quarrying, oil and gas, and constructionmarkets. The map below shows the location of Orica's Newcastle Site.LenaghanWetlandsNational ParkStockringtonKooragangIslandFern BaD WorimiPort Waratah CoalServices (PWCS).FletcherMIShamptonShortland WarabrookMinmiMIPacific HeyOrica LimitedCallaghanWallsendA15WallsendJesmondTighes HillCameron ParkMánvileilleElermore ValeLambtonAISEngenium Pty LtdBlackbutt Nature ReserveB89O CompleteMining SolutionsO Palaris43Mindoro Resources LtdKotaraMerewetherCoal ServicesGlenrockTeralbaCharlestownGo gleWhitebridgeDS7An ammonia-manufacturing plantoperates on Kooragang Island.ORICA"Ammonia is used to make ammoniumnitrate, a hazardous chemical used inthe production of fertilisers andexplosives. Large stockpiles ofammonium nitrate exist within theTHIS IS A NON SMOKING SITENO MATCHES OR LIGHTERS PERMITTEDBEYOND THIS POINTOrica site.Last year, a major explosion in anoverseas major city was due to thedecomposition of large masses ofammonium nitrate.A photograph of the container used tostore ammonium nitrate at the plant.Question 33 continuesQuestion 33 (continued)(a) At temperatures above 260°C, if confined, and when contaminated,ammonium nitrate pellets can decompose, forming dinitrogen oxide gas andwater vapour.Write a balanced chemical equation for the reaction described above.(b)Given that the enthalpy of decomposition of ammonium nitrate is-454kJ/mol, calculate the energy released from the decomposition of 2.0kgof the solid.(c) Discuss the location of Orica's ammonium nitrate storage facility,applying principles studied in the Year 12 Chemistry Course.

An ammonia manufacturing plant operates on Kooragang Island. Ammonia is used to make ammonium…

Question 33 (continued) (a) At temperatures above 260°C, if confined, and when contaminated, ammonium nitrate pellets can decompose, forming dinitrogen oxide gas and water vapour. Write a balanced chemical equation for the reaction described above. (b) Given that the enthalpy of decomposition of ammonium nitrate is -454KJ/mol, calculate the energy released from the decomposition of 2.0kg of the solid. (c) Discuss the location of Orica's ammonium nitrate storage facility, applying principles studied in the Year 12 Chemistry Course.

Question 33 (continued) (a) At temperatures above 260°C, if confined, and when contaminated, ammonium nitrate pellets can decompose, forming dinitrogen oxide gas and water vapour. Write a balanced chemical equation for the reaction described above. (b) Given that the enthalpy of decomposition of ammonium nitrate is -454KJ/mol, calculate the energy released from the decomposition of 2.0kg of the solid. (c) Discuss the location of Orica's ammonium nitrate storage facility, applying principles studied in the Year 12 Chemistry Course.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Ozone, O31g2, is a form of elemental oxygen that plays an importantrole in the absorption of ultraviolet radiation in thestratosphere. It decomposes to O21g2 at room temperatureand pressure according to the following reaction:2 O31g2 ¡ 3 O21g2 ΔH = -284.6 kJ(a) What is the enthalpy change for this reaction per moleof O31g2?(b) Which has the higher enthalpy under these conditions,2 O31g2 or 3 O21g2?
(B) Balance this reaction. Then use the bond enthapies given in the table below to calculate the enthalpy of reaction for the balanced reaction. See 2 attachment
Question: The reaction between hydrogen gas (H2) and oxygen gas (O2) to form water (H2O) is a well-known exothermic reaction. However, if a mixture of hydrogen gas and oxygen gas is ignited in a closed container with limited volume, the reaction can result in a violent explosion. Explain the reasons behind this contrasting behavior and the factors that contribute to the explosiveness of the reaction.
Which statement about the reaction illustrated in the diagram is true? (B). (A] (C) (D) (E) O The energy required to break the bonds is more than the energy released upon forming new bonds. The energy required to break the bonds is less than the energy released upon forming new bonds. O No heat is required to start the reaction. The reaction is endothermic.
Consider the reaction of a mixture of NaHCO3 and Ca(HCO3)2 with excess HCl. The net ionic reaction observed is H+(aq) + HCO3-(aq) → H2O(l) + CO2(g) The data for this problem is for 25 oC 7.701 g of a sample containing a mixture of NaHCO3 and Ca(HCO3)2 is mixed with an excess of HCl to produce CO2 gas. When all of the (dried) gas is collected in a 1.00 L vessel, the total pressure is 1.452 atm. How many g of NaHCO3 were present in the initial sample?
Please don't provide handwritten solution ....
The reaction that produces the water gas mixture, described in Question 6.99, is C(s) + H₂O(g) → CO(g) + H₂(g) This reaction requires an input of 131 kJ of heat for every mole of carbon that reacts. (a) Is this reaction endothermic or exothermic? (b) What is the energy change for this reaction in units of kJ/mol of carbon?
Part A) The standard molar heat of formation of water vapor (steam) is -242 kJ/mol. What amount of energy, in kilojoules, is produced when 1.50*108 liters of hydrogen gas at STP are combusted with excess of oxygen. (a) 1.50x108 (b) 1.62x10-9 (c) 1.62x109 (d) 8.10x108 (e) None of those. If so, what is your answer? Part B) In a reaction between nickel (II) nitrate and sodium sulfide in aqueous solution, spectator ions are: (a) sodium & sulfide (b) nickel & nitrate (c) sodium & nitrate (d) nitrate & sulfide (e) There are no spectator ions Part C) Carbon dioxide diffuses through a porous barrier at a rate of 0.200 mL/min. If the unknown gas diffuses through the same barrier and at the same conditions at a rate of 0.331 mL/min, what gas out of the following it may be? (a) Ar (b) H2 (c) NO (d) CH4…
When 3.8 g A are reacted with 8.5 g D, according to the balanced chemical equation below, 33 kJ of energy are released. Please calculate the enthalpy for this reaction when 3 moles of G are produced. 2A + 3D = 2Z + 3G given molar masses: A = 141.8 g/mole D = 63.996 g/ mole Z = 4.032 g/ mole G = 56.028 g/ mole
Calculate the enthalpy of decomposing hydrogen iodide to produce hydrogen and iodine. 2HI(g) → I2(s) + H2(g) I2(s) → I2(g) ΔH⁰ = 124.8 kJ/mol I2(g) + H2(g) → 2HI(g) ΔH⁰ = - 73.0 kJ/mol
The presence of a catalyst the enthalpy (AH) difference between products and reactants. (A) (B) Decreases Has no effect on