Calculate the value of AG temperature for the following reaction at 289 KK 2.9 10- and...
Question (1 point) 2nd attempt Calculate the value of AGеxn for the following reaction at 289 K. Ka = 2.9 10-8 and ass temperature. HCIO(aq) +H20(l) — ClO (aq) + H20+ (aq) x 10 kJ/mol - 1st attemnt
Use the data to determine the value of the AG pxn for this reaction on the surface of Mars where the average temperature is 210 K: Ca(CIO4)2(s) CaCl2(s) + 402(9) AH (kJ/mol) AS° (J/K mol) O2(g) 205.0 CaCl(s) -795.8 104.6 Ca(CIO)2(s) -736.8 233 O-2.06 x 10% kJ O-1.47 x 10° kJ +4.03 x 103 kJ +8.83 x 107 kJ
9. Determine the value of AG° at 25 °C for the reaction below given the following data: CH (g) AG° = 68 kJ/mol, H.O(g) AG -229 kJ/mol, CH,H,OH(aq) AG =-175 kJ/mol CH. (g) + H2O (g) →CH,H,OH(aq) 10. Chloroform, CHCI, has a normal boiling point of 61 °C and it enthalpy of vaporization is 29.24 kJ/mol, what is its entropy of vaporization in J/mol Kat 61 °C? Before you calculate it write a chemical equation for this process and predict...
Use the data given to calculate the value of Κ for the reaction at 5°C Ag+(aq) + Cl− (aq) AgCl(s) AgCl(s) Ag+(aq) Cl− (aq) S° (J K−1 mol−1) 96.2 72.68 56.4 ΔH°f (kJ/mol) −127.07 105.58 −167.2 a. 5.7 × 109 b. 1.0 c. 3.7 × 1010 d. 1.3 × 106 e. 1.9 × 1012
Which of the following best describes this dissociation reaction? (Hint: Remember that AG - AH - TAS, how does the entropy term change at different temperatures?) NH, NO3(s) + NH4 + (aq) + NO3-(aq) AH- +28.05 kJ/mol AS- +108.7J/mol*K Spontaneous at al temperatures Not spontaneous at any temperature Spontaneous at high T but not low T Spontaneous at low T but not high T
Thomas Eember 2 2019 1. Calculate AG for a reaction give e AG for a reaction given AH = 15.4 kJ/mole and AS = 2.0 J/K at 298 K. Is this reaction spontaneous in the forward direction? 2. Calculate the AG* for the net reaction given the following two reactions: Reaction 1: A+BC AGⓇ = 5 kJ/mol Reaction 2: C+ D EAGⓇ =-12 kj/mol 3. If the internal pH of a muscle cell is 6.8, what is the (HPO4+1/[H2PO4 ratio...
(9) A spontaneous process has the change of free energy (a) AG>0 (c) AG = 0 (b) AG <O (d) AH>0 and AS <O (10) A chemical reaction has AH = 10 kJ. AS = 50 J/K at temperature T = 300 K. the reaction AG = J. (a) 5000 (b) -5000 (c) 10000 (d) 50 (11) For reaction: Ag (s) + 2 Cl2 (g) Ag° (aq) +CI (aq), the standard free energy of formation: AGf° (Ag*) = 77.1 kJ/mol,...
Apple Bing GOOJU TUU Smartworks Dashboard W. W. Norton & Comp... Digital Resources for Chemistry atoto @kean.edu < CH14... d. 70% 11/05/19 This is a Numeric Entry question / It is worth 1 point/ You have unlimited attempts/There is a 5% attempt penalty See page 653 14 Question (1 point) 1st attempt W See Periodic Table Calculate the value of AGixn for the following reaction at 294 K. K -2.9 x 10-8 and assume Kdoes not change significantly with temperature....
(9) A spontaneous process has the change of free energy (a) AG > 0 (b) AG <0 (c) AG = 0 (d) AH >0 and AS <0 (10) A chemical reaction has AH = 10 kJ, AS = 50 J/K at temperature T = 300 K, the reaction AG = (a) 5000 (b)-5000 (c) 10000 (d) 50 (11) For reaction : Ag (s) + 1/2 Cl2 (g) = Agt (aq) + CI+ (aq), the standard free energy of formation: AGE"...
Consider the following reaction and its AG at 25.00 °C. Mg(s) + Ni2+ (aq) Mg2+ (aq) + Ni(s) AG = -408.0 kJ/mol Calculate the standard cell potential, Ecell for the reaction. 2.11 V Enter numeric value Calculate the equilibrium constant, K, for the reaction. K= 3.30 x1071 Incorrect