Consider the data in the table. Compound Melting point (°C) Δ H fus (kJ/mol) Boiling point (°C) Δ H vap (kJ/mol) HF −83.11 4.577 19.54 25.18 HCl −114.3 1.991 −84.9 17.53 HBr −86.96 2.406 −67.0 19.27 HI −50.91 2.871 −35.38 21.16 Using the data in the table, calculate Δ S fus and Δ S vap for HBr . Δ S fus = J / ( K ⋅ mol) Δ S v a p = J / ( K ⋅ mol) Determine the entropy change when 7.50 mol HBr ( l ) freezes at atmospheric pressure. Δ S = J / K
Consider the data in the table. Compound Melting point (°C) Δ H fus (kJ/mol) Boiling point...
Consider the data in the table. Compound Melting point (°C) AHfus (kJ/mol) Boiling point (°C) AH ap (kJ/mol) HF -83.11 4.577 19.54 25.18 НСІ -114.3 1.991 -84.9 17.53 HBr - 86.96 2.406 -67.0 19.27 HI -50.91 2.871 -35.38 21.16 Using the data in the table, calculate ASfus and ASvap for HI. ASfus = J/(K.mol) AS vap = J/(K · mol) Determine the entropy change when 6.50 mol HI(1) boils at atmospheric pressure. AS = J/K
Consider the data in the table. Compound Melting point (°C) AHus (kJ/mol Boiling point (°C) AHap (kJ/mol HF ---83.11 4.577 19.54 25.18 HC1 -114.3 1.991 -84.9 17.53 HBr -86.96 2.406 -67.0 19.27 -50.91 2.871 -35.38 21.16 Using the data in the table, calculate A Stus and AS for HBr. HI A Stus = 12.93 J/K mol) AS - 93.54 J/(K.mol) Determine the entropy change when 3.90 mol HBr(I) freezes at atmospheric pressure. as - 364.82
Consider the data in the table. Compound Melting point (°C) AH (kJ/mol) Boiling point (°C) AHap (kJ/mol HF -83.11 4.577 19.54 25.18 HCI -114.3 1.991 -84.9 17.53 HBr -86.96 -67.0 19.27 HI -50.91 -50.91 2.871 -35.38 21.16 Using the data in the table, calculate ASfus and AS vap for HI. 2.406 A Stus = 24.1 J/(K mol) ASvap = J/(K.mol) Determine the entropy change when 7.50 mol HI(1) freezes at atmospheric pressure. AS = J/K Question Source: MRG - General...
OLLILEI UM ALLI LUUIU. Compound Melting point (°C) A Hus (kJ/mol) Boiling point (°C) AHvap (kJ/mol) HF -83.11 4.577 19.54 25.18 HCI -114.3 1.991 -84.9 17.53 HBO -86.96 2.406 -67.0 19.27 HI -50.91 2.871 -35.38 21.16 Using the data in the table, calculate AS tus and ASvap for HCL. Astus = AS = J/(K.mol) ASvap = J/(K.mol) Determine the entropy change when 5.70 mol HCI) melts at atmospheric pressure. AS = | J/K
HF Consider the data in the table. Compound Melting point (°C) AH -83.11 HCI -114.3 HBr -86.96 HI -50.91 4.577 (kJ/mol) Boiling point (°C) A Hvap (kJ/mol) 19.54 25.18 1.991 -84.9 17.53 2.406 -67.0 19.27 2.871 -35.38 21.16 Using the data in the table, calculate ASfus and AS vap for HI. Astu = 12.9 J/(K.mol) ASvap = 89.0 J/(K.mol) Determine the entropy change when 3.40 mol HI(g) condenses at atmospheric pressure. рук AS = 44.0
HF HCI HBr H86.96 83.11 - 114.3 4.577 1.991 2.406 2 871 19.54 84.9 67.0 35.38 25.18 1753 19.27 21.16 -50.91 calculate AStus and ASap for HF. Number Number As...- 24.1 J/(K- mol J/ (k mo AS 86.1 Determine the entropy change when 6,90 mol of HF(s) melts at atmospheric pressure. Number J/K Tools O Pevious @ checs Atswer O nt
1. If If Kc=0.425 at 40.°C and Kc=0.670 at 90.°C, what is ΔH° for the reaction? X↽−−⇀Y kj 2.Consider a general reaction A(aq)⇌enzymeB(aq) The ΔG°′ of the reaction is −7.500 kJ·mol−1. Calculate the equilibrium constant for the reaction at 25 °C. Keq′= What is ΔG for the reaction at body temperature (37.0 °C) if the concentration of A is 1.7 M and the concentration of B is 0.65 M? ΔG= 3. Attempt 9 Consider the data in the table. Compound...