For the reaction CO₂(g) + H₂(g) → CO(g) + H₂O(g) AH = 41.2 kJ and AS = 42.1 J/K The equilibrium constant for this reaction at 342.0 K is Assume that ΔΗ° and AS are independent of temperature. Submit Answer Retry Entire Group 9 more group attempts remaining

19 Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) AHf AGf AS° AHf (kJ/mol) AGf (kJ/mol) AS° Substance (kJ/mol) (kJ/mol) (J/mol-K) Substance (J/mol-K) Aluminum Chlorine CI (g) C (аq) Cl2 (g) HCI (aq) HCI (g) Chromium Al (s) AIC13 (s) 28.32 121.7 105,7 - 131,2 165.2 - 705.6 - 630.0 109.3 - 167.2 56.5 Al203 (s) - 1669.8 1576.5 51.00 222,96 - 131.2 -95.27 - 167.2 56.5 186,69 Barium - - Ba(s) BaCO3(s) BaO(s) Beryllium Be(s) 63.2 -92.30 - 1216,3 - 553.5 - 1137.6 112.1 Cr (g) Cr (s) Cr203 (s) Cobalt Со (g) Copper Cu (s) CuCl2 (s) CuO (s) - 525.1 70.42 397.5 352.6 174.2 23.6 9.44 - 1139.7 - 1058.1 81.2 BeO(s) Be(ОН)2(8) 13.77 50.21 - 608.4 -579,1 - 817.9 - 905.8 439 393 179 Bromine 111.8 - 120.9 Br(g) Br-(aq) Br2(g) Br2(1) HBr(g) Calcium Ca(g) Ca(s) CaCO3 (s, calcite) CaCl2(s) CaF2(s) CaO(s) Ca(OH)2(s) CaSO4(s) 82.38 174.9 33.30 108.1 - 102.8 - 167,7 - 128,3 - 147.9 80.71 - 205.9 30,71 3.14 245.3 - 156,1 42,59 - Cu20 (s) Fluorine F (g) F- (aq) F2 (g) HF (g) Hydrogen 152.3…

For a certain chemical reaction, the equilibrium constant K = 2.2 x 10" at 5.00 °C. Calculate the standard Gibbs free energy of reaction. Round your answer to 2 significant digits. AG° = kJ ? Expnation Check 2021 McGra Education Alr oa ey Meseved Tms MacBook Ain

For the reaction 2HBr(g) + Cl₂ (g) → 2HCl(g) + Br₂ (g) AH = -81.1 kJ and AS° = -1.20 J/K The equilibrium constant for this reaction at 288.0 K is | Assume that ΔΗ° and AS are independent of temperature. Submit Answer Retry Entire Group 9 more group attempts remaining

< ✓ 11 Question 25 of 25 (1 point) | Question Attempt: 1 of 2 ✓ 12 ✓ 13 ✓ 14 Here are some facts about the reaction: ✓ 15 At -5.67 °C the concentration equilibrium constant K = 7.0 for a certain reaction. с • If the reaction is run at constant pressure, 101. kJ/mol of heat are absorbed. X 16 -1 1 • The constant pressure molar heat capacity C₂ = 2.23 J-mol K Р Using these facts, can you calculate Kat 9.4 °C? • If the reaction is run at constant pressure, the volume increases by 13.%. If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether Kat 9.4 °C will be bigger or smaller than Kat -5.67 °C? O Yes. O No. 0 17 Yes, and K will be bigger. No. Yes, and K will be smaller.

M req For the reaction E 20 H₂(g) + Cl₂(g) → 2HCl(g) AH = -185 kJ and AS = 20.0 J/K The equilibrium constant for this reaction at 261.0 K is Assume that ΔΗ° and AS are independent of temperature. Submit Answer SA 4 000 000 R F Show Hint DE LO % 5 Retry Entire Group [Review Topics] [References] Use the References to access important values if needed for this question. T G Cengage Learning Cengage Technical Support < C 6 9 more group attempts remaining Y H & 7 U 8 J I 9 K 0 0 P Previous Next Email Instructor Save a +

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3. Calculate AS at 25°C and 1 atm pressure in J/(mol-K) for the following reaction CH4(8) + N₂(g) + 164 kJ → HCN(g) + NH3(8) AG° = 159 kJ. [a] 1x10² [b] 2 [c] 4x10² [d] 2x10¹ [e] 7x10¹

Use the data below to calculate the value of the equilibrium constant for the following reaction at 298 K. Please give your answer with 2 significant figures. 3 NO2(g) + H2O(e) → 2 HNO3(e) + NO(g) AfG [H2O(l)] = -237.2 kJ mol-1 ; AFG°[HNO3(e)] = -79.9 kJ mol-1 ; AfG [NO(g)] = 86.7 kJ mol-1; AfG°[NO2(g)] = 51.8kJ mol-1

Hydrogen bromide dissociates into its gaseous elements, H2 and Br2, at elevated temperatures. AH;, kJ/mol S° , J/(mol-K) HBr(g) -36.44 198.6 H2 (9) 130.6 Bra(9) 30.91 245.3 a. Calculate the percent dissociation at 337°C and 1.00 atm. (Enter your answer to three significant figures.) Percent dissociation % b. What would be the percent dissociation at 337°C and 10.0 atm? (Enter your answer to three significant figures.) Percent dissociation ]% c. Use data above and any reasonable approximation to obtain K. (Enter your answer to three significant figures.) K