What is A, H° for the following chemical reaction? CS2(g) + 2H₂O(1)→CO₂(g) + 2H₂S(9) You can use the following table of standard heats of formation (AFH) to calculate the enthalpy of the given reacti Element/ Compound H(g) H₂(g) H₂O(l) CS₂(g) C(g) C(s) Standard Heat of Formation (kJ mol-¹) 218 0 -285.8 116.7 71 0 Element/Compound N(g) 0₂ (9) O(g) H₂S(g) CO₂(g) HNO3(aq) Standard Heat of Formation (kJ mol-¹) 473 249 -20.60 -393.5 -206.6 Express the standard enthalpy of reaction to three significant figures and include the appropriate units. ▸ View Available Hint(s)

What is A, H° for the following chemical reaction? CS2(g) + 2H₂O(1)→CO₂(g) + 2H₂S(9) You can use the following table of standard heats of formation (AFH) to calculate the enthalpy of the given reacti Element/ Compound H(g) H₂(g) H₂O(l) CS₂(g) C(g) C(s) Standard Heat of Formation (kJ mol-¹) 218 0 -285.8 116.7 71 0 Element/Compound N(g) 0₂ (9) O(g) H₂S(g) CO₂(g) HNO3(aq) Standard Heat of Formation (kJ mol-¹) 473 249 -20.60 -393.5 -206.6 Express the standard enthalpy of reaction to three significant figures and include the appropriate units. ▸ View Available Hint(s)

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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Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? endothermicexothermic (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 13.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = kJ(e) Calculate E when 360.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K kJ HopHelpCh5N1
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
Thermochemistry and Stoichiometry
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? endothermicexothermic (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 13.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = kJ(e) Calculate E when 360.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K kJ HopHelpCh5N1
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Using the reaction enthalpy data shown, determine the amount of heat released in each situation: 2Ca (s) + O2 (g) ----> 2 CaO (s) ΔHrxn = -1,269.8 kJ a) if calcium reacts with 3.00 moles of O2 b) if 8.00 moles of calcium reacts with O2 c) if calcium and oxygen react to form 1.00 mole of CaO
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