Calculate the enthalpy for this reaction:2C(s) + H2(g) ---> C2H2(g)AH° = ??? kJGiven the following thermochemical equations:C₂H2(g) + (5/2)02(g) ---> 2CO2(g) + H2O(l)AH° = -1299.5 kJC(s) + O2(g) -> CO₂(g)H2(g) +(1/2)02(g) ---> H₂O(l)AH° = -393.5 kJAH° = -285.8 kJ+226 kJ+1572 kJ○ -226 kJ-787 kJ

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Answered: Calculate the enthalpy for this…

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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Al203 (s) + 3 CO (g) → 2 Al (s) + 3 CO2 (g) AH = A. Calculate AHreaction for the reaction above using the following known' thermochemical reactions. 2 Al (s) + 3/2 O2 (g) → Al203 (s) AH = - 1675.7 kJ CO (g) + 1/2 O2 (g) → CO2 (g) AH = - 292.7 kJ B. Is this reaction endothermic, exothermic, or both? How do you know? Blank # 1 Blank # 2
2. Use the standard reaction enthalpies given below to determine AH°rxn_for the following reaction: 2NO (g) + O2 (g) → 2NO2 (g); AH°xn = ? Given: N2 (g) + O2 (g) → 2NO (g) AH°rxn = 183 kJ ½ N2 (g) + O2 (g) → NO2 (g) AH°rxn = 33 kJ
The following thermochemical equation is for the reaction of iron(III) oxide(s) with hydrogen(g) to form Fe3O4and water(g). 3Fe2O3(s) + H2(g)----> 2Fe3O4(s)+ H2O(g) H= -6.00kj When 53.8 grams of iron(III) oxide(s) react with excess hydrogen(g), _____ kJ of energy are _____ (absorbed/evolved)
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Determine the enthalpy for the reaction shown below. CS2(l) + 3O2(g) --> CO2(g) + 2SO2(g) ΔH = ? Given: C(graphite) + O2(g) --> CO2(g) ΔH = -393.5 kJ S(s) + O2(g) --> SO2(g) ΔH = -296.8 kJ C(graphite) + 2S(s) --> CS2(l) ΔH = 87.9 kJ ( Change and add the equations to get the target equation)
In the recovery of iron from iron ore, the reduction of the ore is actually accomplished by reactions involving carbon monoxide. Use the following thermochemical equations, Fe,O3() + 3CO(g). 2Fe(s) + 3CO,(g) AH° =-28 kJ 3Fe,O3(6) + CO(g) 2Fe,O4() + CO,(g) AH° = -59 kJ FezO,(s) + CO(g)- 3FcO(s) + CO,(g) AH° = +38 kJ The AH;° for the reaction FeO(s) + CO(g)- Fe(s)+ CO2(g) is -16.8 kJ. Use this data and the data in the following table to calculate the value of AH;° for FeO. Standard Enthalpies of Formation of Typical Substances Substance H,O,() HBr(g) AH? (NI mol-") AH7 (kI mol-1) AH; (KI mol-") AH (KI mol-1) Substance substance substance Ag(s) -187.6 CH() -84.667 NO(g) 90.37 AgBr() - 100.4 -36 CH,OH) -277.63 NO:(g) 33.8 - 127.0 HCI(g) -92.30 Ca(s) N,0(g) 81.57 AlG) HI(g) 26.6 CaBrzG) -682.8 9.67 Al,O,() -1669.8 HNO,() -173.2 CaCO,(s) -1207 N,O,(g) 11 C6) (graphite) H,SO) -811.32 CaCl,() -795.0 Na(s) HC,H,0,() NaHCO,() Na,CO,() NaCI() -110.5 -487.0 -635.5 -947.7 CO,() CH(g) CH,C(g) CHI(g)…
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Using Hess's Law, determine AHf ° for CH4 based on the following reactions. It is known that when methane combustion takes place, 802.37 kJ / mol of heat is released Cgrafito + 2H2 CH4(g) CH4(9) + 202(9) CO29) + 2H2O) A¢H°= -802.37 kJ/mol Cgrafito + O2(g) CO2(g) A:H°= -393.5 kJ/mol 2H2(9) + O2(9) 2H2O(9) A¡H°= -241.83 kJ/mol
The value of AH° for the reaction below is 128.1 kJ CH,OH -Co, + 2H (1) 2(g) 2(g) How may kJ of heat are consumed when 10.1 g of H2(g) is formed as shown in the equation? Given that the atomic mass of C = 12.01 g/mol, H = 1.008 g/mol, O = 16.00 g/mol Show your answers in TWO (2) decimal places. Do not include the units in your final answers.
Calculate the enthalpy change for the reactionP4O6(s) + 2 O2(g) -----> P4O10(s)given the following enthalpies of reaction:P4(s) + 3 O2(g) ---->P4O6(s) ΔH = -1640.1 kJP4(s) + 5 O2(g) ----->P4O10(s) ΔH = -2940.1 kJ
The oxidation of glucose, C6H12O6(s), is described by the following thermochemical equation:C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(l) ΔH = -2772 kJHow much heat, in kilojoules, can be produced by the oxidation of 3.56 g of fuel C6H12O6?Molar mass of C6H12O6 = 180.156 g/mol
Use the standard reaction enthalpies given below to determine AH° rxn 4 SO3(g) →4 S(s) + 602(g) AH°rxn = ? Given: SO2(g) →S(s) + O2(8) 25O2(g) + O2(g) →2SO3(g) 1583 kJ -494.6 kJ -791.4 kJ -293.0 kJ -692.4 kJ AH rxn = +296.8 kJ ΔΗ°, rxn = -197.8 kJ for the following reaction

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