T = 289 K
ΔGo = 3.79 KJ/mol
ΔGo = 3790 J/mol
use:
ΔGo = -R*T*ln Kc
3790 = - 8.314*289.0* ln(Kc)
ln Kc = -1.5774
Kc = 0.2065
Kc is defined as concentration of product by concentration of reactant with each concentration term raised to power that is equal to its stoichiometric coefficient in balanced equation
So,
Kc = [C]^3 / [A][B]^3
0.2065 = [C]^3 / (0.82 * 0.56^3)
0.2065 = [C]^3 / 0.144
[C]^3 = 0.02974
[C] = 0.310 M
Answer: 0.310 M
Question 15 1 pts Given that AGºrxn = 3.79 kj for the following reaction at 289...
Question 15 1 pts Given equilibrium concentrations of A = 0.138 M; B = 0.154 M and C = 0.071 M at 308 K, calculate AGºrxn for the following reaction in kj. Enter the result to 2 decimal places and no units. 2A + 1B → 2C
Question 17 1 pts Use the values from the table and calculate the equilibrium constant kat 396 Kelvin. Enter the result with 3 s.f. and scientific notation. 1A + 1B → 2C + 1D compound B AGⓇkj/mol - 12.5 -14.4 - 11.9 -11.8
Question 12 1 pts Use the values from the table and calculate AGºrxn at 306 K in kJ. Enter the result no decimal places and no units. 2A + 1B 2C + 3D compound AH®, kj/mol sºj/molK -78 194 -82 183 -80 137 -75 200
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. Calculate the equilibrium concentration of Cl2 in that results from the decomposition of COCl2 with an initial concentration of 0.3166 M. COCl2(g) ⇌ CO(g)...
Question 1 1 pts Calculate AG at 25 °C, in kJ, f or the following reaction, at Fe 0.82, PH2-1.668 (atm), and[H] 0.339 M. Fe(s) 2H (aq) Fe2H2(g) ΔGo for Fe2+--78.9 kJ/mol
15.Calculate K for the following reaction given the following equilibrium concentrations of Ha CO, and H2O: (7p) PCIs(g)_ PCI3(g) + Cl2(g) K-? Equilibrium Concentrations (M): .200 040 080 15.Calculate K for the following reaction given the following equilibrium concentrations of Ha CO, and H2O: (7p) PCIs(g)_ PCI3(g) + Cl2(g) K-? Equilibrium Concentrations (M): .200 040 080
Question 23 10 pts The entropy change for the reaction ( ASºrxn) shown below is -121.8 J/K. Calculate AS°surr, AS°univ and AGºrxn at 298 K. N2(g) + 2O2(g) + 2NO2(g) AH°rxn = 66.4 kJ • (a) AS surr = [Select ] • (b) AS°univ = [Select ] • (c) AGºrxn = [Select ]
10. Calculate for the following reaction given the following equilibrium concentrations of H, CO, and H20. PCis(g) – K = "? PCI;(g) + .040 Chi(g) .080 Equilibrium Concentrations (M): 200 080 K Calculations: Solving for an Equilibrium Concentration when K and all other Equilibrium Concentrations are Given 11. What is the equilibrium concentration of Br; if (HBr) - 0.35 M and [H:) - 0.22 M at equilibrium? H:(g) + Brz(g) 2HBr(g) K = 62.5
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. The reaction below is not at equilibria and Q = 1.7. The equilibrium constant is K = 0.230. 2SO3(g) ⇌ 2SO2(g) + O2(g)...
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