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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THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) → 4Q2 (g) + 3J2X (l) ΔH = -1,090.6 kJ 4QJ3 (g) + 3X2 (g) → 2Q2 (g) + 6J2X (l) ΔH = -1,581.1 kJ Calculate the value of ΔH (in kJ) for the reaction: Q2 (g) + ½ X2 (g) → Q2X (g) (Round off the final answer to ONE decimal place. Do not include unit.)
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
Hydrazine, N2H41), is used in rocket fuels. The thermochemical equation for the combustion of hydrazine is N2HA) + 02(g) → N2(g) + H20 () AHồ = - 622.4k). What quantity of heat is liberated by the combustion of 1.00 g of N,Hall)?
Given the heat of formation of the following compounds from their elements: AH°F = -393.5 kJ/mol AH°f = -285.9 kJ/mol CH;OH(1) AH°F = -238.6 kJ/mol CO((g) H;O(1) What is the value of AH® for the reaction; CH;OH() + 3/2 O:(2) – CO.(g) + 2 H;O(1) A) -726.7 kJ B) -416.9 kJ C) -346.2 kJ D) -440.8 kJ E) -1203.9 kJ
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)
Calculate the AH° for the reaction: 2C2H6 (g) + 7 O2 (g) 4CO2 (g) + 6H2O (g) Using the following thermochemical data: 2C (s) + 3H2 (g) C2H6 (g) AHO = - 84.5 kJ 2H2 (g) + O2 (g) 2H20 (1) AH° = - 571.5 kJ %3D H20 (g) H20 (I) AH = - 44.0 kJ CO2 (g) C (s) + O2 (g) AH = + 393.5 kJ Units don't need to be typed in the answer. Add negative sign (-) if the answer is negative (eg. -23.96)
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)…
The value of AH° for the reaction below is 128.1 kJ CH ,OH CO24) OH () + 2H 2(g) How may kJ of heat are consumed when 5.7 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.
THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) → 4Q2 (g) + 3J2X (I) AH = -1,096.4 kJ 4QJ3 (g) + 3X2 (g) → 2Q2 (g) + 6J2X (1) AH = -1,548.8 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (g) + ½ X2 (g) → Q2X (g)

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