What is AS surr for a reaction at 15.2 °C with AHsys = 13 kJ mol¹? Express your answer in J mol¹ K-1 to at least two significant figures. Answer:
Q: 4355.5 kJ/mol 16,091 kJ/mol
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- Automobiles and trucks pollute the air with NO. At 2000.0°C, Kc for the reactionN2(g)+O2(g)2NO(g)At 2000.0°C Kc = 4.100 × 10–4 and ΔH° = 180.6 kJ. What is the value of Kc at 41.00°C?Calculate Ksp for the salt NaCl at 25°C. Substance ΔGf°(in kJ/mol) Na+(aq) –262.0 Cl–(aq) –131.0 NaCl(s) -383.6Say 0.0101 moles of gas in a car engine cylinder under a pressure of 608 kPa at 606 K expandsadiabatically and reversibly until it is at 1 atm pressure. The Cv,m of the gas is 20.8 J/K/mol whileCp,m = 29.12 J/K/mol, so what is q, Tf, U, w, Vf, and H?Hint: (Pi/Pf)= (Ti/Tf)^ (CV+nR/nR)
- A potential chemical reaction at 25.0 °C has a ΔHrxn of 163 kJ and a ΔSrxn of -354.3 J/K. What is the ΔGrxn in kJ.Compute ΔGo at 200.0 oC for each of the following reactions, which are important in the chemistry of coal. Assume that coal has the same thermodynamic properties as graphite. Substance ΔHo(kJ/mol) So(J/(mol*K)) C(graphite) 0 5.7 H2O(g) -241.83 188.835 CO(g) -110.5 197.7 H2(g) 0 130.680 O2(g) 0 205.152 CO2(g) -393.5 213.8 C(s, coal) + H2O(g) CO(g) + H2(g) C(s, coal) + O2(g) CO2(g) C(s, coal) + 1/2O2(g) CO(g) CO(g) + H2O(g) CO2(g) + H2(g)14. Determine the ΔUoreaction at 25 °C (in kJ/mol) for the following reaction: 5PbO2(s) + 4P(s, white)→P4O10(s) + 5Pb(s) 16. Using standard heats of formation, determine ΔH for the following reactions. Report your answers to the nearest 0.1 kJ. Fe2O3(s) + 3H2O(l)2Fe(OH)3(s) B2O3(g) + 3H2O(l)2H3BO3(s)
- Calculate ΔHrxn for the following reaction: CaO(s)+CO2(g)→CaCO3(s) Use the following reactions and given ΔH values: Ca(s)+CO2(g)+1/2O2(g)→CaCO3(s) , ΔH= -812.8 kJ 2Ca(s)+O2(g)→2CaO(s), ΔH= -1269.8 kJ Express your answer using four significant figures.Calculate ΔHrxn for the following reaction: CaO(s)+CO2(g)→CaCO3(s) Use the following reactions and given ΔH values: Ca(s)+CO2(g)+12O2(g)→CaCO3(s), ΔH= -812.8 kJ2Ca(s)+O2(g)→2CaO(s), ΔH= -1269.8 kJ Express your answer using four significant figures.SHOW CLEAR SOLUTION: To a test tube containing 10.0 ml of 0.50 M HCl solution in a calorimeter, 0.05482 g of solid MgO (MW = 40.30 g/mol) at the same temperature was added. A change in temperature of 6.2°C was recorded. In a separate experiment, the heat capacity of the calorimeter was determined to be 0.293 kJ/°C. D. Calculate the experimental ΔHrxn (in kJ/mol) for the reaction between MgO andHCl.E. If the theoretical ΔHrxn of the reaction between MgO and HCl is -1349 kJ/mol, calculate the %error.
- Calculate the ΔG° (kJ/mol) for the following reaction at 152 °C, using the following data. Eneter your answer with the correct number of sig figs, without units. C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g) ΔHf◦ (kJ/mol) S◦(J/K.mol) C3H8 (g) -104.7 270.2 O2(g) 0 205.0 CO2(g) -393.5 213.7 H2O(g) -241.8 188.7Calculate the value of ΔGo in kJ for the combustion of 1 mole of methane to form carbon dioxide and gaseous water at 298 K.(value ± 2) So given below in J/mol K S° (CH4(g)) = 186. S° (O2(g)) = 209. S° (CO2(g)) = 217. S° (H2O(g)) = 188. ΔHfo given in kJ/mol ΔHfo (CH4(g)) = -74. ΔHfo (CO2(g)) = -399. ΔHfo (H2O(g)) = -231.Suppose that the gas-phase reaction 2 NO(g) + O2(g)------->2 NO2(g) were carried out in a constant-volume containerat constant temperature. (a) Would the measured heatchange represent ΔH or ΔE? (b) If there is a difference, whichquantity is larger for this reaction? (c) Explain your answer topart (b).
