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- Given the data below, H°, for the reaction rxn 2SO2 (g) + O2 (g) → 2SO3 (g) is kJ. AH°; (SO2 (g)) = -297 kJ/mol AH°; (SO3 (g)) = -396 kJ/mol AH°; (SO2C12 (g)) = -364 kJ/mol AH°f (H2SO2 (1)) = -814 kJ/mol AH°; (G2O (1)) = -286 kJ/mol %3D O The AH°F of O2 (g) is needed for the calculation. 99 198 -198 -99Using the accompanying tables, determine. at 25C: C3HB() + 502(g)- 3 CO2(g) + 4H2O(g) the value of AHO the Value of ASO the Value of AGOPlace the folowing tems witn the carrect benetit high specafic mécet •Conesion -Surface tnsicA upa Yaent Qroperties Water temperatures in abike skay इु्य felatincly Cal even thdugh a heat wowe maker the Qr tenapesas ler hot': ihigh peitic heate 3. Conesiun 4. Suoface tension S. goodl schyent उम रठान
- how do you know the state (s,l,g,aq) of a compound?+ O°H +(HO)D)+osH O Ca,0 O HCaz CaSO O CasO, & %Given the following enthalpy change values for the reactions below: A + 2B – C; A,H = 350.1 kJ mol-1 E + F - 2C + D;A,H = 476.2 kJ mol-1 ½ E - G + 2B ; A;H = -229.6 kJ mol-1 Calculate A,H for the following reaction (in kJ mol-1) using Hess's Law: 2A + D - F + 2G
- explan whyConsider the two diagrams that follow. (a) Based on (i), writean equation showing how ΔHA is related to ΔHB and ΔHC.(b) Based on (ii), write an equation relating ΔHZ to the otherenthalpy changes in the diagram. (c) The equations you obtainedin parts (a) and (b) are based on what law? (d) Wouldsimilar relationships hold for the work involved in eachprocess?Using the AH; for SO3(g) and SO2lg) calculate AH° for the following reaction: SO3g)SO2(g) +1/202(3) AH° for SO3(g) = kJ The equations for SO3(g) and SO2(g) are as follows: S(s) +3/2 O2(g)- SO;(g) AH;° = -395.2 kJ/mol S(s) + O2(g) →SO2(g) AH,º = -296.9 kJ/mol e Textbook and Media Hint Save for Later ype'here to search hp fs f8 # & 4 5. 6. 8 %24
- Given the following thermochemical data at 25°C and 1 atm pressure, 3/2 02(g) + 2B(s) - B203(s); AH° = -1264 kJ; O3(g) + 2B(s) - B203(s); AH° = - 1406 kJ; determine AH° for the following reaction at 25°C and 1 atm pressure. 302(g) → 203(g) O a. +980 kJ/mol O b. -980 kJ/mol O C. -2670 kJ/mol O d. +284 kJ/mol e. -284 kJ/molA student determines the value of the equilibrium constant to be 55.2 for the following reaction. C2H4(g) + H,O(g)- →CH;CH2OH(g) Based on this value of Keqi AG° for this reaction is expected to be (greater,less) than zero. Calculate the free energy change for the reaction of 1.64 moles of C,H.(g) at standard conditions at 298K. kJ rxnA;H°(CO2, g) = -393.5 kJ mol'; A;H°(H2O, 1) = -294.6 kJ mol S°(CH3OH, I) = 126.8 J mol' K'; s°(O2, g) = 205.0 J mol"' K'; s°(CO2, g) = 213.6 J mol' K'; A¢H°(H2O, I) = 76.0 J mol Kl Let's consider the reaction of combustion of methanol at 298 K with a standard molar enthalpy of reaction A,H° = -725.2 kJ mol: CH,OH) CO2 (9) + 2 H,Ou O2 (9) (1) (1) Calculate the standard molar enthalpy of formation of methanol at 298 K.
