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Use the values given in the textbook (Appendix B) for the following question. Click here for...
please show your work. thank you. The reusable booster rockets of the space shuttle use a...
please show your work. thank you.
The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel A possible reaction is: 3Al(s) +3NH CIO,(s) Al2O3(s) + AlCly(s) + 3NO(g) + 6H20(g) Calculate AHo for this reaction using the standard enthalpies of formation found in Appendix B of your book and ammonium perchlorate's standard enthalpy of formation ΔΗ:--295 kJ/mol
step by step clearly The solid-fuel rockets of the space shuttle are based on the following...
step by step clearly
The solid-fuel rockets of the space shuttle are based on the following reaction between ammonium perchlorate and aluminum: 3 NH4CIO4(s) + 3 Al(s) = Al2O3(s) + AlCl3(g) + 3 NO(g) + 6 H2O(g) If either reactant is in excess, unnecessary mass will be added to the shuttle, so a stoichiometric mixture is desired. What mass of each reactant should be used for every kilogram of the fuel mixture?
2. The launch of the Space Shuttle was assisted by solid propellant rockets containing aluminum as...
2. The launch of the Space Shuttle was assisted by solid propellant rockets containing aluminum as the fuel and ammonium perchlorate, NH4CIO4, as the oxidizer; the two powders were bound together by a rubbery polybutadiene binder. Neglecting the binder (which is also a fuel) a balanced reaction equation is shown below. Use the listed values of the formation enthalpies to calculate Δ,H° for this reaction. 2A1(s) + 2 NH4Clo,(s) Al2O3(s) + N2(g) + → 3H2O(g) + 2HCl(g) +O2(g) -295.3 -1675.7...
The solid rocket boosters of the space shuttle employed the following oxidation/reduction reaction: 10 Al (s)...
The solid rocket boosters of the space shuttle employed the following oxidation/reduction reaction: 10 Al (s) +6NH4CLO4 (s) --> 4Al2O3 (s) +2AlCl3 (s) + 12 H2o (g) + 3N2 (g) ?Hf 0 for NH4ClO4= -295.3 KJ/mol Al=0 KJ/mol Al2O3= -1676 KJ/mol AlCl3= -704.2 KJ/mol H2O= -241.82 KJ/mol N2= 0 KJ/mol Calculate the standard enthalpy of this reaction. How much energy is released when 100,000 kg of ammonium perchlorate (and excess aluminum) is burned?
2. Calculate the enthalpy for the reaction below at standard conditions using Appendix G in your...
2. Calculate the enthalpy for the reaction below at standard
conditions using Appendix G in your textbook. [Report the answer to
three sig fig, without unit labels, and using +/- signs to indicate
if the reaction is endo- or exothermic.] 2 Al(s) + Fe2O3(s) -->
Al2O3(s) + 2 Fe(s)
Substance AH (kJ mol-) AG; (kJ mol-1) Sº (JK-1 mol-2) aluminum 0 0 28.3 324.4 285.7 164.54 -531 -485 -321.7 Al(s) Al(g) Al3+ (aq) Al2O3(s) AlF3(s) AICI3(s) AlCl3.6H2O(s) -1676 -1582 50.92...
a) Complete the table below using data given in the Appendix of your textbook. 2 CH18...
a) Complete the table below using data given in the Appendix of your textbook. 2 CH18 (1) + 25 O2 (g) → 16 CO2 (g) +18 H20 (1) O2(g) CO2 (g) H20 (1) C4H8 (1) -208.4 kJ/mol AH® (kJ/mol) sº (J/molK) 463.7 JK 'mol b) Calculate AG° combustion at 25°C for octane, CsH18 (1). Give your answer in kJ/mol of CH18 (1). c) Consider the reaction, 3 Fe203 (s) + 3 C(s) + 4 Fe (s) + 3 CO2 (g)...
Review Intelligent Tutoring Problem 12-03 Use data from Appendix D of the textbook or use google...
Review Intelligent Tutoring Problem 12-03 Use data from Appendix D of the textbook or use google to do the following calculations for the reaction NiO(s) + CO(g) = Ni(s) + CO2(g). The standard ENTHALPY change in KJ/mol^-1 is -43.3 QUESTION: Calculate the standard entropy change (in J K-1 mol-1).
Use the ΔH°f values provided to determine ΔH°rxn for the following reaction CH4(g) + 3 Cl2(g)...
Use the ΔH°f values provided to determine ΔH°rxn for the following reaction CH4(g) + 3 Cl2(g) → CHCl3(l) + 3 HCl(g) ΔH°rxn = ? ΔH°f (kJ/mol): -75 -134 -92 A. +662 kJ B. +117 kJ C. -151 kJ D. -335 kJ The equation that corresponds to the enthalpy of formation for NH3(g) is A. N(g) + 3H(g) → NH3(g) B. N(g) + 3/2 H2(g) → NH3(g) C. 1/2 N2(g) + 3H(g) → NH3(g) D. 1/2 N2(g) + 3/2 H2(g) →...
Part A Several reactions and their standard reaction enthalpies at 298.15 K are given here: Al_C3(s)...
Part A Several reactions and their standard reaction enthalpies at 298.15 K are given here: Al_C3(s) + 12H2O(l) + 4Al(OH),(s) + 3CH4(g) 2Al(s) + O2(g) + Al2O3(s) 1 A1,03(s) + H2O(l) + Al(OH)3(s) AH (kJ. mol-?) –1683.0 -1675.7 -9.6 The standard enthalpies of combustion of graphite and CH4(8) are -393.51 and --890.35 kJ. molº respectively. Calculate the standard enthalpy of formation of Al4C3(s) at 25°C.
4) (a) Use the standard entropy values (AS") in the Appendix to solve for ?5° of...
4) (a) Use the standard entropy values (AS") in the Appendix to solve for ?5° of each reaction at 25°C. (b) Solve for AG° ron for both reactions as well using the standard free energy values. (AG) 2H20(liquid)2H2(g) + O2(g) Al2O3(s) 3 H2(g) 2 Al(s)3 H20(g) 5) AH° 180.7 kJ; AS 24.7 JIK 25°C N2(8) O2(g)-2 NO(g) (a)Calculate the standard free-energy change for the reaction at 25°C. (b) Calculate ?G at 500°C using the ?G° value calculated from part a.
please show your work. thank you.
The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel A possible reaction is: 3Al(s) +3NH CIO,(s) Al2O3(s) + AlCly(s) + 3NO(g) + 6H20(g) Calculate AHo for this reaction using the standard enthalpies of formation found in Appendix B of your book and ammonium perchlorate's standard enthalpy of formation ΔΗ:--295 kJ/mol
step by step clearly
The solid-fuel rockets of the space shuttle are based on the following reaction between ammonium perchlorate and aluminum: 3 NH4CIO4(s) + 3 Al(s) = Al2O3(s) + AlCl3(g) + 3 NO(g) + 6 H2O(g) If either reactant is in excess, unnecessary mass will be added to the shuttle, so a stoichiometric mixture is desired. What mass of each reactant should be used for every kilogram of the fuel mixture?
2. The launch of the Space Shuttle was assisted by solid propellant rockets containing aluminum as the fuel and ammonium perchlorate, NH4CIO4, as the oxidizer; the two powders were bound together by a rubbery polybutadiene binder. Neglecting the binder (which is also a fuel) a balanced reaction equation is shown below. Use the listed values of the formation enthalpies to calculate Δ,H° for this reaction. 2A1(s) + 2 NH4Clo,(s) Al2O3(s) + N2(g) + → 3H2O(g) + 2HCl(g) +O2(g) -295.3 -1675.7...
2. Calculate the enthalpy for the reaction below at standard
conditions using Appendix G in your textbook. [Report the answer to
three sig fig, without unit labels, and using +/- signs to indicate
if the reaction is endo- or exothermic.] 2 Al(s) + Fe2O3(s) -->
Al2O3(s) + 2 Fe(s)
Substance AH (kJ mol-) AG; (kJ mol-1) Sº (JK-1 mol-2) aluminum 0 0 28.3 324.4 285.7 164.54 -531 -485 -321.7 Al(s) Al(g) Al3+ (aq) Al2O3(s) AlF3(s) AICI3(s) AlCl3.6H2O(s) -1676 -1582 50.92...
a) Complete the table below using data given in the Appendix of your textbook. 2 CH18 (1) + 25 O2 (g) → 16 CO2 (g) +18 H20 (1) O2(g) CO2 (g) H20 (1) C4H8 (1) -208.4 kJ/mol AH® (kJ/mol) sº (J/molK) 463.7 JK 'mol b) Calculate AG° combustion at 25°C for octane, CsH18 (1). Give your answer in kJ/mol of CH18 (1). c) Consider the reaction, 3 Fe203 (s) + 3 C(s) + 4 Fe (s) + 3 CO2 (g)...
Part A Several reactions and their standard reaction enthalpies at 298.15 K are given here: Al_C3(s) + 12H2O(l) + 4Al(OH),(s) + 3CH4(g) 2Al(s) + O2(g) + Al2O3(s) 1 A1,03(s) + H2O(l) + Al(OH)3(s) AH (kJ. mol-?) –1683.0 -1675.7 -9.6 The standard enthalpies of combustion of graphite and CH4(8) are -393.51 and --890.35 kJ. molº respectively. Calculate the standard enthalpy of formation of Al4C3(s) at 25°C.
4) (a) Use the standard entropy values (AS") in the Appendix to solve for ?5° of each reaction at 25°C. (b) Solve for AG° ron for both reactions as well using the standard free energy values. (AG) 2H20(liquid)2H2(g) + O2(g) Al2O3(s) 3 H2(g) 2 Al(s)3 H20(g) 5) AH° 180.7 kJ; AS 24.7 JIK 25°C N2(8) O2(g)-2 NO(g) (a)Calculate the standard free-energy change for the reaction at 25°C. (b) Calculate ?G at 500°C using the ?G° value calculated from part a.
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