Consider the acid-base reaction below. NH4+ (aq) + CN −(aq) ⇒ NH3(aq) + HCN(aq) K = 1.7 (a) What is the value of AGO at 298 K? ✔ kJ/mol 4.0 -1.32 What are the values of Q and AG at 298 K under the following conditions, and in which direction (→, , or ) is the reaction proceeding. [NH4+] [CN] [NH3] [HCN] (b) 0.10M 0.10M 0.10M 0.10M (c) 0.12M 0.10M 0.17M 0.12M (d) 0.10M 0.10M 0.18M 0.18M (b) 4.0 1.7 (c) 4.0 308 (d) 4.0 Q X x 4.00 4.0 -4.23 4.0 AG X kJ/mol X kJ/mol kJ/mol direction of reaction ос 11 0 00 O O O ↑ ↓ 11 11 ↑↓

Use data to compute AG° at 82.0°C for the following reaction. 4FECI3(s) + 302(g) → 2FE203(s) + 6CI2(3) AH°t (FeCl3(s)) = -399.5 kJ mol-1 AH°t (Fe2O3(s) = -824.2 kJ mol-1 AS° (FeCl3(s)) = 142.3 J mol 1 K-1 AS° (Fe2O3(s)) = 87.4 J mol-1 K-1 AS° (Cl2(g)) = 223.1 J mol-1 K-1 AS° (O2(g)) = 205.152 J mol-1 K1 AG° = i kJ eTextbook and Media Save for Later Attempts: 0 of 3 used Submit Answer

It is observed that a solution of cobalt chloride in water/propanol turns blue at high temperatures and pink at low temperatures. What does this imply for the production or consumption of heat by this reaction? CoCl(H2O)5+(aq) + Cl-(aq) ⇄ CoCl2(H2O)2(aq) + 3H2O(l) The cobalt species on the left is pink and the cobalt species on the right is blue.  Select one: a)The reaction consumes heat, that is, it is endothermic.  b)The reaction produces heat, that is, it is exothermic.  c)The reaction neither consumes nor produces heat.

Question 6 Calculate the AG for the following process at 100 K and 300 K. Use the thermodynamic data from Appendix G in OpenStax Chemistry, 2e. If one exists, calculate the temperature (in K) at which the process switches between spontaneous and non-spontaneous. ZaCl() Zn (aq) + 2 Cl (ag) Report G to the tenths place. AG T= " K ப P

a) For a reaction with AH = -152.6 kJ mol-¹ and AS°= -543.8 J K-¹ mol-¹ at 25 °C, how will AGº change if the reaction temperature is increased? Explain your answer. b) Calculate the equilibrium constant for the reaction at 80 °C, showing your working (assume AH and AS° are temperature independent).

Determine the equilibrium constant for a reaction at 200 K if AG =26.2 kJ/mol. (R = 8.314 J/mol · K)

Calculate AG° for the reaction shown below using the provided thermodynamic properties information. H2O2 (1) → 2 H2O () + O2 (g) Substance AH°; (kJ/mol) AS° (J/(mol•K)) H2O2 (1) - 187.8 232.9 H20 (1) -285.83 69.91 O2 (g) 205.0 -396.4 kJ/mol -350.5 kJ/mol -33.70 kJ/mol -1105 kJ/mol -417.2 kJ/mol

Determine AG (in kJ) for the following reaction at 325 K when the concentrations of the species are as follows: NO₂= 10.00 M, N₂O4 = 14.3 M. AG°f (NO₂) = 51 kJ/mol, AG (N₂O4) = 97.7 kJ/mol. 2 NO2(8) N₂O4(8)

For the reaction A(aq) ---> B(aq) the variation in the standard free enthalpy is 3.50 kJ at 25 oC and 4.64 kJ at 45 oC. Calculate the value of the equilibrium constant for this reaction at 75°C.

Determine the value of K for a reaction where AG° = -29.62 kJ/mol at 298 K. K =