CompoundsAgBr(s) -100.4 Cacl2(s) -795.8H2O(g)-241.8 NH4NO3(s)-365.6AgCl(s)-127.1 Caco3(s) -1206.9H2O(1)|-285.8NO(g)+90.2Agl(s)-61.8 Cao(S)-635.1H2O2(1)-187.8NO2(g)+33.2AGNO3(s) -124.4 Ca(OH)2(s) -986.1H25(g)-20.6 N204(g)+9.2Ag20(s)-31.0 CasO4(s) |-1434.1 H2S04() -814.0Nacl(s)-411.2Al203(s) |-1675.7 Cdcl2(s) -391.5HgO(s)-90.8NaF(s)-573.6Bacl2(s) -858.6 cdo(s) -258.2KBr(s)|-393.8 NaOH(s) |-425.6BaCO3(s) -1216.3 Cr203(s) -1139.7KCI(s)-436.7NIO(s)|-239.7BaO(s) -553.5CuO(s)-157.3KCIO3(s)-397.7PbBr2(s) -278.7BaSO4(s) |-1473.2 Cu20(s) -168.6 KCIO4(s)-432.8 PbCl2(s) -359.4CC14(1) |-135.4Cus(s)KNO3(s)PbO(s)|-219.0-53.1-494.6CHCI3(I) -134.5 Cu2s(s)-79.5MgCl2(s) -641.3PbO2(s) -277.4CH4(g)-74.8 Cuso4(s) -771.4 MgCO3(5) -1095.8 PCI3(g)|-287.0C2H2(g) +226.7 Fe(OH)3(s) -823.0Mgo(s)-601.7PCI5(9) -374.9C2H4(g) +52.3 Fe203(s) -824.2 Mg(OH)2(5) -924.5SIO2(s)-910.9C2H6(g) -84.7 Fe304(s) |-1118.4 MgSO4(s) |-1284.9 Sno2(s) -580.7C3H8(g) |-103.8 HBr(g)-36.4MnO(s)SO2(g) -296.8-385.2|снзон(-238.7HCl(g)-92.3MnO2(s)-520.0SO3(g)-395.7C2H5OH() -277.7HF(g)-271.1NH3(g)-46.1Znl2(s)|-208.0Colg)-110.5HI(g)+26.5N2H4(1)+50.6ZnO(s)|-348.3CO2(g) -393.5 HNO3() -174.1NH4Cl(s)-314.4ZnS(s)-206.0CationsAnionsAg+(aq) +105.6 Hg2+(aq) +171.1Br2(aq)-121.6НРО4|-1292.1Al3+(ag) -531.0K+(aq)|-252.4| CO32-(aq) -677.1 HSO4-(aq) -887.3Ba2+(aq) -537.6 Mg2+(aq) -466.8Cl-(aq)-167.2I-(aq)-55.2Ca2+(ag) -542.8 Mn2+(aq) -220.8 ClO3-(aq) -104.0 Mn04-(aq) -541.4Cd2+(ag) -75.9Na+(aq) -240.1 Cl04-(aq) -129.3 NO2-(aq) |-104.6Cu+(aq)+71.7 NH4+(ag) -132.5 Cro42-(ag) -881.2 NO3-(ag) -205.0Cu2+(aq) +64.8 Ni2+(aq) -54.0 Cr2072-(ag) -1490.3 OH2(aq) -230.0Fe2+(aq) -89.1 Pb2+(aq)-1.7F-(aq)-332.6 PO43-(ag) |-1277.4Fe3+(ag) -48.5Sn2+(aq)-8.8нсо3-(aq) |-692.0S2-(aq)+33.1H+(aq)0.0Zn2+(ag) -153.9 H2PO4-(ag|-1296.3 SO42-(ag) -909.3 34. Use Hess's law to calculate AH for the decomposition of CS2(1) to itselements.CS;(1) –C(s) + 2S(s)Use Table 8.3 and the following thermochemical equations:(1) formation of CO, from its elements at 25°C(2) formation of SO, from its elements at 25°C(3) CO,(g) + 2S0,(g) CS,(1) + 3 O2(g)AH = +1103.9 kJ

Use Hess’s law to calculate to calculate delatH for the decomposition of CS2 to its elements. Hess’s…

34. Use Hess's law to calculate AH for the decomposition of CS2(1) to its elements. CS:(1) → C(s) + 2S(s) Use Table 8.3 and the following thermochemical equations: (1) formation of CO, from its elements at 25°C (2) formation of SO, from its elements at 25°C (3) CO.e) + 2S0(e) → CS.(1) + 30,(0) AH = +1103.9 kl

34. Use Hess's law to calculate AH for the decomposition of CS2(1) to its elements. CS:(1) → C(s) + 2S(s) Use Table 8.3 and the following thermochemical equations: (1) formation of CO, from its elements at 25°C (2) formation of SO, from its elements at 25°C (3) CO.e) + 2S0(e) → CS.(1) + 30,(0) AH = +1103.9 kl

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...

See similar textbooks

Similar questions

Automobiles and trucks pollute the air with NO. At 2000.0°C, Kc for the reaction is 7.42 × 10–4, and ΔH for the reaction is 180.6 kJ.N2(g)+O2(g)2NO(g) What is the value of Kc at 1000.0°C?
the first picture is the question and the second picture is the expected answer (please apply thermochemistry and their formula)
Use the data below to determine the ΔHrxn for the following reaction: S=S(g) + H2(g) è H-S-S-H(g) (S=S: 425 kj/mol; S-S: 286 kj/mol, H-S: 363 kj/mol, H-H: 432 kj/mol )
A metal oxide MO was reduced with carbon, as follows. 2 MO(s) + C(s) → 2 M(s) + CO2(g) The reaction of 0.790 mol of MO(s) with excess carbon released 227 kJ of heat at constant pressure. What is ΔrH (in kJ/mol) for this reaction? Round your answer to the tenths (0.1) place.
People have said diamonds are forever. However, let's look at the reaction of a diamond turning into graphite. Use your textbook or the world wide interwebs to look up the necessary information to calculate the Δ Grxn for diamond turning into graphite and enter the value for Δ Grxn (in kJ/mol):
Unit Name: Thermodynamic Chemistry investigate and analyse energy changes and rates of reaction in physical and chemical processes, and solve related problems; If 3.65g of butane is burned underneath a cup holding 1.00 L of water at 21.0oC, what will the final temperature of the water be (ΔHcomb = -3325 kJ/mol)?
Calculate the AS°rxn for the reaction 2NO,(g) → N204(g) at 530 K. [The standard molar heat capacities for each compound are: N,O4 (79.2 J/K · mol), NO2 (37.2 J/K · mol).] ЈK mol
None
1. When sodium bicarbonate is reacted with excess hydrochloric acid, carbon dioxide is produced according to the reaction belowNaHCO3 (s) + HCl(aq)  NaCl(aq) + CO2 (g) + H2O (l) ΔHrxn = 28.5 kJ/mola. What is the sign of q for the reaction?b. How much heat is required when 75.0 g of NaHCO3 react with excess HCl?c. How much heat is required if 1.4 kg of CO2 is produced?
Use the following information to answer the question: What is the ΔH (in kJ/mol) for the following reaction? (Show work) CS2(l) + 3 O2(g) → CO2(g) + 2 SO2(g) Given: C(s) + O2(g) → CO2(g); ΔHf = -393.5 kJ/mol S(s) + O2(g) → SO2(g); ΔHf = -296.8 kJ/mol C(s) + 2 S(s) → CS2(l); ΔHf = 87.9 kJ/mol
When a 25.0 g sample of AgNO3 dissolves in 100.0 g of water in a calorimeter, the temperature drops from 22.3 °C to 15.9 °C. Calculate ΔH for the process: AgNO3(s) → Ag+(aq) + NO3 -(aq) c = 4.184 J/g∘C