Consider the following chemical reaction at 25°C: CH3CO2H(aq) =H+(aq) + CH3CO; (aq), Ka = 1.83x10-5 Compute AG at...
Given CH3CO H(aq) = H(aq) + CH3CO2 (aq) at 25°C, Kg = 1.83 x 102. What is AG at 25°C for a solution in which the initial concentrations are: [CH3CO2H]o = 0.10 M [H]o = 6.4 x 10-8M [CH3CO2 lo = 0.010 M Select one: a.-19.7 kJ 5.-73.8 kJ C. 27.0 kJ d. 19.7 kJ e. 73.8 kJ
cace). The Ka for acetic acid. HCHO(ag) is 1.8 X 10 at 25°C Write the chemical reaction that chemical reaction that describes the dissociation of acetic acid. C2 1 2 0 2 (aq) + H3 1 C2 H 3 O 2 caq) + H 2 O (1) Given the following standard enthalpies of formation Substance AH® (kJ/mol) (T= 25°C) HC2H3O2(aq) -485.76 C2H302 (aq) -486.01 H(aq) Calculate the K, at 35 °C. Qualitatively, how would expect the pH of a solution...
(a) Calculate ?G for the reaction: 2H,000 H()+OH (ag) at 25 C given the following initial concentrations. HO] 1.0x 10-12 M and (OH]- 20 x10* M (b) Predict the direction in which the reaction will proceed spontaneously to establish equilibrium. 10. The AG° for the reaction: N,(g)+3H,(g)0 2NH,(g) is 33.3 kJ/mol at 25°C. What is the value of Kp?
Consider a general reaction A(aq) = B(aq) The AG of the reaction is -3.490 kJ - mol. Calculate the equilibrium constant for the reaction at 25°C. Kin= 0.333 What is AG for the reaction at body temperature (37.0 °C) if the concentration of Ais 1.8 M and the concentration of Bis 0.65 M? AG -9.561 kJ mol
Consider a general reaction enzyme A(aq) = B(aq) The AG*' of the reaction is –5.650 kJ. mol-?. Calculate the equilibrium constant for the reaction at 25 °C. Keq = What is AG for the reaction at body temperature (37.0 °C) if the concentration of A is 1.9 M and the concentration of B is 0.60 M? AG= kJ. mol-1
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...
Consider a general reaction czyme A(aq) = B(aq The AG of the reaction is - 7.190 kJ. mol. Calculate the equilibrium constant for the reaction at 25 °C. Kg = .00126 What is AG for the reaction at body temperature (37.0 °C) if the concentration of A is 1.7 M and the concentration of B is 0.75 M? AG = -9,3 kl. mol-
Consider the unbalanced reaction of : Fe^+3 (aq) +Hg2^+2(aq) Fe^+2(aq) +Hg^+2(aq) which has a Kc= 9.1x10^-6 at 298 K and has a delta G^o= 28.75 kJ/mol. Calculate delta G in kJ/mol when [Fe^+3]=0.20 M, [Hg2^+2]=0.10M, [Fe^+2]=0.010M, and [Hg^+2]= 0.025M
Consider a general reaction enryme A(aq) = B(aq) The AG® of the reaction is - 7.190 kJ. mol"!. Calculate the equilibrium constant for the reaction at 25 °C. Kq= What is AG for the reaction at body temperature (37.0 °C) if the concentration of A is 1.7 M and the concentration of B is 0.75 M? AG = kl. mol-1
The equilibrium constant for the reaction Agl(s) — Ag+ (aq) +1 (aq) is the solubility product constant, Ksp = 8.3 x 10-17 at 25°C. Calculate AG for the reaction when [Ag+]=1.5 x 10-3 M and [Br] =1.5 x 10-2 M. Is the reaction spontaneous or nonspontaneous at these concentrations? AG = 98 kJ/mol, spontaneous AG = 92 kJ/mol, nonspontaneous AG = -65 kJ/mol, spontaneous AG = 65 kJ/mol, nonspontaneous AG = -92 kJ/mol, spontaneous