In thermodynamic of the dissolution of Borax lab, the student's graph is below. Calculate AS? (R= 8.314 x 10-3 kJ/mole K) LN of Ksp vs 1/Temperature in Kelvin LN Ksp 0 0.0031 0.0032 0.0033 0.0034 0.0035 0.0036 0.0037 -2 -4 -6 y=-9104.5x + 26.39 R2 = 0.9713 Temperature in K-1 Series1 .........Linear (Series1) OA) 0.008075 kJ/mol K B) -75.69 kJ/mol K OC) -0.008075 kJ/mol K OD) -0.2194 kJ/mol K OE) 75.69 kJ/mol K OF) 0.2194 kJ/mol K

In thermodynamic of the dissolution of Borax lab, the student's graph is below. Calculate AS? (R= 8.314 x 10-3 kJ/mole K) LN of Ksp vs 1/Temperature in Kelvin LN Ksp 0 0.0031 0.0032 0.0033 0.0034 0.0035 0.0036 0.0037 -2 -4 -6 y=-9104.5x + 26.39 R2 = 0.9713 Temperature in K-1 Series1 .........Linear (Series1) OA) 0.008075 kJ/mol K B) -75.69 kJ/mol K OC) -0.008075 kJ/mol K OD) -0.2194 kJ/mol K OE) 75.69 kJ/mol K OF) 0.2194 kJ/mol K

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions

Section5.5: Enthalpy Changes For Chemical Reactions

Problem 1RC: 1. For the reaction 2 Hg(l) + O2(g) → 2 HgO(s), ∆rH° = 181.6 kJ/mol-rxn. What is the enthalpy change...

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1. For the reaction 2 Hg(l) + O2(g) → 2 HgO(s), ∆rH° = 181.6 kJ/mol-rxn. What is the enthalpy change to decompose 1.00 mol of HgO(s) to O2(g) and Hg(l)? 3633 kJ −90.8 kJ 90.8 kJ 363.3 kJ
In thermodynamic of the dissolution of Borax lab, the student's graph is below. Calculate AS? (R= 8.314 x 10-3 kJ/mole K) LN of Ksp vs 1/Temperature in Kelvin LN Ksp 0 0.0031 0.0032 0.0033 0.0034 0.0035 0.0036 0.0037 -2 4 -6 -8 y=-9104.5x + 26.39 R2 = 0.9713 Temperature in K-1 Series1 ......... Linear (Series1) A) 0.008075 kJ/mol K B) -75.69 kJ/mol K OC) -0.008075 kJ/mol K OD) -0.2194 kJ/mol K E) 75.69 kJ/mol K OF) 0.2194 kJ/mol K
For the reaction Na2CO3 (9) + 2HCI9) → NaCls) + CO2 (g) + H2O() AH is -144.1 kJ. What is AU. O -141.62 -146.58 +141.62 +146.58
Macmillan Learning ■ 2023-05-02.png Consider a general reaction Keg = enzyme A(aq) B(aq) The AG" of the reaction is -7.780 kJ. mol-¹. Calculate the equilibrium constant for the reaction at 25 °C. AG = 23 -10 What is AG for the reaction at body temperature (37.0 °C) if the concentration of A is 1.6 M and the concentration of B is 0.60 M? Type here to search L 81 99+ (DELL o W 46°F Rain showers 179% x J kJ. mol-¹ ENG 10:16 PM US 5/2/2023
Please solve this
AG; (kJ/mol) AH; (kJ/mol) AS; (kJ/mol) AV; (kJ/mol) -32.84 CH4 (aq) + SO4? (aq) E> HCO3 (aq) + HS (aq) + H2O) 1.76 115.99 4.97 2.1 Given the thermodynamic data for the overall reaction, sketch the relative stability of CH4 (ag) + S022- (ag) compared to HCO3 (aq) + HS (aq) + H2OU) in Pressure-Temperature space. Which side of the reaction is favored at high temperature? and which side of the reaction is favored at high pressure? Why?