Study the following thermochemical data very carefully:Clelg)lag)ICI(g)Ia(s)2C(g)21(g)I(g) + CI(g)la(g)AH = 242.3 kJAH = 151.0 kJAH = 211.3 kJAH = 62.8 kJI2(s) reacts with Clag) to produce ICI(g).Write the chemical equation to produce ONLY one mole of ICI(g)

Desired equation is as follows. 12I2g+12Cl2g→IClg

Answered: Study the following thermochemical data…

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 standard enthalpy of formation of NiSO 4(s) at 25 °C is -872.9 kJ/mole. The chemical equation to which this value Ni(s) + S(s) + 2 O2(g) → NiSO4(s) 1/2 Ni(s) + 1/2 S(s) + 1/2 O2(g) → 1/2 NiSO4(s) NiSO4(s) → Ni(s) + S(s) + 4 O(g) Ni(s) + S(s) + 4 O(g) → NiSO4(s)
THERMODYNAMICS: Calculate the value of AH (in kJ) for the reaction, 2AR3 (g) + Q (s) → A2R4 (g) + QR2 (s) given the following hypothetical thermochemical equations: AH = -84 kJ AH = -151.3 kJ AH = -537.5 kJ 2AR3 (g) + 2AX (g) → A2R4 (g) + 2XAR (g) AX (g) + ½R2 (g) → XAR (g) Q (s) + R2 (g) → QR2 (s) (Round off final answer to ONE decimal place) Round your answer to 1 decimal place.
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(s) + 3CO(g)→ 2Fe(s) + 3CO,(g) AH° = -28 kJ 3Fe,O3() + CO(g) 2Fe3O4() + Co,(g) AH = -59 kJ FezO,(s) + CO(g)→ 3FCO(s) + CO,(g) AH° = +38 kJ The AH° for the reaction FeO() + 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 AH; (KI mol-1) AH; (kl mol-1) 90.37 Substance Substance AH (KI mol-1) Substance AH; (KI mol-1) Substance Ag(s) AgBr() H,O,(/) -187.6 CH.(g) -84.667 NO(g) - 100.4 - 127.0 HBr(g) -36 CH,OH(/) -277.63 NO,(g) 33.8 AgCI(s) HCIg) -92.30 Ca) 81.57 Al() HI(g) 26.6 CaBr,() -682.8 9.67 Al,0,) -1669.8 HNO,() -173.2 CaCO() - 1207 11 CG) (graphite) H,SO,() -811.32 CaCl,() -795.0 Na(s) CO(g) HC,H,0,) NaHCO,) Na,CO,() -110.5 -487.0 CaO() -635.5 -947.7 CO.(g) -393.5 Hg(/) Ca(OH),()…
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(s) + 3CO(g) 2Fe(s) + 3CO,(g) AH° = - 28 kJ 3Fc,O3() + CO(g) 2Fe3O4() + CO,(g) AH = -59 kJ FezO4(s) + CO(g) 3FcO(s) + CO,(g) AH° = +38 kJ to calculate AH° for the reaction FeO() + CO(g) Fe(s) + CO2(g) AH° = i kJ
THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) – 4Q2 (g) + 3J2X (1) AH = -1,070 kJ 4QJ3 (g) + 3X2 (g) → 202 (g) + 6J2X (1) AH = -1,580.2 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (g) + % X2 (g) –→ Q2X (g) (Round off the final answer to ONE decimal place. Do not include unit.)
20) Given the following thermochemical equations, 4NH3(g) + 7O2(g) → 4NO2(g) + 6H2O(g) ΔHo = -1132 kJ6NO2(g) + 8NH3(g) → 7N2(g) + 12H2O(g) ΔHo = -2740 kJ calculate the value of ΔH° (in kilojoules) for the reaction 4NH3(g) + 3O2(g) → 2N2(g) + 6H2O(g)
Given: 4AICI3(s) + 302(g) → 2Al,O3(s) + 6C12(g); AH=-529.0 kJ determine AH for the following thermochemical equation. Cl,(3) + Al,O;(s) → AICI,(9) + 02(g) O +88.2 kJ O +264.5 kJ O +176.3 kJ O -176.3 kJ O +529.0 kJ
THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) – 4Q2 (9) + 3J2X (1) AH = -1,017.3 kJ 4QJ3 (g) + 3X2 (g) → 202 (9) + 6J2X (1) AH = -1,548.8 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (g) + % X2 (g) –→ Q2X (g) (Round off the final answer to ONE decimal place. Do not include unit.)
Using the following thermochemical equations; (a) CaO (s) + Cl2 (g) → CaOCl2 (s) ΔH°= -110.9 kJ(b) CaO (s) + H2O (l) → Ca(OH)2 (s) ΔH°= -65.1 kJ(c) H2O (l) + CaOCl2 (s) + Br2 (l) → Ca(OH)2 (s) + Br2 (l) +2 NaCl (s) ΔH°= -60.2 kJDetermine the value of ΔH° in kJ for the following reaction:½ Cl2 (g) + NaBr (s) → ½ Br2 (l) + NaCl (s)
THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) – 4Q2 (g) + 3J2X (1) AH = -1,096.4 kJ 4QJ3 (g) + 3X2 (g) → 202 (g) + 6J2X (1) AH = -1,548.8 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (g) + % X2 (g) –→ Q2X (g) (Round off the final answer to ONE decimal place. Do not include unit,.)
Given the following thermochemical equations: C2H29) + 5 02(9) 2C02(g) + H201) AH° = -1229.5 kJ AH° = -393.5 kJ C(6) + 02(g) → C02(g) 1 H2(9) +5 02(9) → H20) AH° = -285.5 kJ 2 Calculate the enthalpy (in kJ) for this reaction: 206) + H2(g) → C,H2(9)
Use the following thermochemical equations:(a) 2 NaCl (s) + H2O (l) → 2 HCl (g) + Na2O (s) ΔH°=507.31 kJ(b) NO(g) + NO2 (g) + Na2O (s)→ 2 NaNO2 (s) ΔH°=-427.14 kJ(c) NO(g) + NO2 (g) → N2O (g) + O2 (g) ΔH°=-42.68 kJ(d) 2 HNO2 (l) → N2O (g) + O2 (g)+ H2O (l) ΔH°=34.35 kJto determine the value of ΔH° in kJ for the following reaction:HCl (g) + NaNO2 (s) HNO2 (l) + NaCl (s)

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Study the following thermochemical data very carefully: Clelg) lag) ICI(g) Ia(s) 2C(g) 21(g) I(g) + CI(g) la(g) AH = 242.3 kJ AH = 151.0 kJ AH = 211.3 kJ AH = 62.8 kJ I2(s) reacts with Clag) to produce ICI(g). Write the chemical equation to produce ONLY one mole of ICI(g)