The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel. A possible reaction is 3A1(s) + 3NH, ClO4(s) → Al, O, (s) + AIC13 (s) + 3NO(g) + 6H2O(g) Calculate AH° for this reaction. Substance and State AH£° (kJ/mol) Al(s) Al, O3(s) AlCl3 (s) H2O(g) NO(g) NH, CIO4(s) -1676 -704 -242 90. -295 AH° kJ Submit Answer Try Another Version 1 item attempt remaining

The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel. A possible reaction is 3A1(s) + 3NH, ClO4(s) → Al, O, (s) + AIC13 (s) + 3NO(g) + 6H2O(g) Calculate AH° for this reaction. Substance and State AH£° (kJ/mol) Al(s) Al, O3(s) AlCl3 (s) H2O(g) NO(g) NH, CIO4(s) -1676 -704 -242 90. -295 AH° kJ Submit Answer Try Another Version 1 item attempt remaining

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...

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The Haber process is used to manufacture ammonia from nitrogen and hydrogen in the presence of an iron catalyst. The reaction, shown in this equation, is exothermic: N 2 (g)+3H 2 (g) rightleftharpoons 2N*H_{3}(g) + Heat Which statement correctly describes the chemical reaction? The energy needed to break the chemical bonds of 1 mole of nitrogen and 3 moles of hydrogen is greater than the energy released by the formation of 3 moles of ammonia. The energy needed to break the chemical bonds of 1 mole of nitrogen and 3 moles of hydrogen is less than the energy released by the formation of 3 moles of ammonia. The energy released by breaking the chemical bonds of 1 mole of nitrogen and 3 moles of hydrogen is greater than the energy needed to form 3 moles of ammonia. The energy released by breaking the chemical bonds of 1 mole of nitrogen and 3 moles of hydrogen is less than the energy needed to form 3 moles of ammonia.
The enthalpy for the formation of 1 mole of NH3(aq)NH3(aq) is -80.29 kJ/molkJ/mol. What is the enthapy for the formation of 3 moles of NH3(aq)NH3(aq)?
Suppose you burned 0.300 g of C(s) in an excess of Oz(g) in a constant-volume calorimeter to give CO2(g). C() +0s (8) → CO,(3) The temperature of the calorimeter, which contained 767 g of water, Increased from 26.15 °C to 28.56 °C. The heat capacity of the bomb is 870. J/K. Calculate AU per mole of carbon. (The specific heat capacity of liquid water is 4.184 J/g K.) AU- k/mol C
Iron can be extracted from the iron(III) oxide found in iron ores (such as haematite) via an oxidation-reduction reaction with carbon. The thermochemical equation for this process is: 2 Fe203(s) + 3 C(s) → 4 Fe(1) + 3 CO2(g) AH° = +467.9 kJ
Are the reactions endothermic or exothermic? What observation supports this?
Aqueous solutions of calcium chloride and sodium hydroxide react to form solid calcium hydroxide. The balanced net ionic equation is: A) Ca+2(aq) + 2OH-(aq) + 2Na+(aq) + 2Cl-(aq) → Ca(OH)2(s) B) Ca+2(aq) + 2OH-(aq) + Na+(aq) + Cl-(aq) → Ca(OH)2(s) C) Ca+2(aq) + 2OH-(aq) → Ca(OH)2(s) D) CaCl2(aq) + 2NaOH(aq) → CaOH(s) + NaCl(aq) E) CaCl2(aq) + 2NaOH(aq) → Ca(OH)2(s) + 2NaCl(aq)
The following table contains some standard enthalpies of formation, AH, at 298 K. Substance diamond graphite carbon tetrachloride carbon tetrachloride carbon tetrafluoride methane carbon monoxide carbon dioxide chlorine gas Cl₂ (g) hydrochloric acid fluorine gas hydrofluoric acid hydrogen oxygen water water hydrogen peroxide hydrogen peroxide ΔΗ (kJ/mol) 1.88 Formula C(s) C(s) 0 CCl4 (g) -106.7 CC14 (1) -139.3 CF4 (g) CH4 (g) -74.8 CO(g) -110.5 -679.9 CO₂(g) -393.5 0 HCl(g) -92.30 F2 (g) 0 HF (g) -268.61 H₂(g) 0 O2 (g) 0 H₂O(g) -241.82 H₂O(1) -285.83 H₂O2(g) -136.10 H₂O2 (1) -187.8
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
25.00 mL of 0.4600 M phosphoric acid are reacted with 94.00 mL of 0.7970 M sodium hydroxide. The sodium hydroxide is in excess. Initially, both solutions are at room temperature, 24.692°C. After the reaction is complete, the temperature of the solution has increased to 30.347°C. What is the enthalpy of the reaction in kJ/mol acid? Assume the density of the solution is 1.00g/mL and the specific heat of the solution is the same as water (4.184 J/g-K).
In a coffee cup calorimeter, 3.00 g of NaOH (molar mass 40.00g/mol) was mixed with 75.0 mL of 1.00M HNO3. If the initial temperature of the HNO3 was 31.3°C and the final temperature of the solution was 22.3°C, determine AH for the reaction in kJ/mol. NaOH(s) + HNO3(aq) ===> NaNO3(aq) + H2O) The density and the specific heat capacity of the resulting solution are 1.00 g/ml and 4.18 J/°C.g, respectively. Units do not need to be typed, simply enter the correct number. If the sign of AH is negative put a negative sign (-) in the answer. Answer: