Determine the equilibrium constant (Keq) at 25°C for the reaction?
Cl2(g) + 2Br- (aq) -> Cl- (aq) + Br2(l)
A. 1.5 × 10-10 B. 6.3 × 109 C. 1.3 × 1041 D. 8.1 × 104 E. 9.8
Determine the equilibrium constant (Keq) at 25°C for the reaction?Cl2(g) + 2Br- (aq)? 2Cl- (aq) + Br2(l)A. 1.5 × 10-10 B. 6.3 × 109 C. 1.3 × 1041 D. 8.1 × 104 E. 9.8Please show your work.
5. Determine the equilibrium constant (Keg) at 25°C for the reaction Cla(g)+2Br (aq) 늑 2C1-(aq) + Br2(1) A) 1.5×10-10 B) 6.3×109 C) 1.3×1041 D) 8.1 x 104 E) 9.8
2 Determine the equilibrium constant, Keq, at 25°C for the reaction 2Br (aq) +12/5) = Br261 +21+ (aq). Multiple Choice 17 x 1054 5.7 x 10-55 57 10-19 18.30 19 1018 M
Calculate the equilibrium constant for each of the reactions at 25 ∘C. Standard Electrode Potentials at 25 ∘C Reduction Half-Reaction E∘(V) Pb2+(aq)+2e− →Pb(s) -0.13 Zn2+(aq)+2e− →Zn(s) -0.76 Br2(l)+2e− →2Br−(aq) 1.09 Cl2(g)+2e− →2Cl−(aq) 1.36 MnO2(s)+4H+(aq)+2e− →Mn2+(aq)+2H2O(l) 1.21 Pb2+(aq)+2e− →Pb(s) -0.13 Br2(l)+2Cl−(aq)→2Br−(aq)+Cl2(g) Express your answer using two significant figures.
20 Calculate the equilibrium constant, Keq, at 25 egrees C for the reaction: 2Br-(aq) + 12(5) - Br2(1) + 21-(aq). (Eored.cathode=0.54V and Eored, anode=1.CJV) S (4 Puan) 1.11x10-16 1.62x10-18 1.52x10-16 1.25x10-18 2.25x10-16
Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25 ∘C Reduction Half-Reaction E∘(V) Fe3+(aq)+3e− →Fe(s) -0.036 Sn2+(aq)+2e− →Sn(s) -0.14 Ni2+(aq)+2e− →Ni(s) -0.23 O2(g)+2H2O(l)+4e− →4OH−(aq) 0.40 Br2(l)+2e− →2Br− 1.09 I2(s)+2e− →2I− 0.54 A) 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq) (answers are not 4.1x10^5, 3.3x10^3, 2.7x10^10, or 2.6x10^10) B) O2(g)+2H2O(l)+2Ni(s)→4OH−(aq)+2Ni2+(aq) C) Br2(l)+2I−(aq)→2Br−(aq)+I2(s) (answer is not 1.7x10^18)
9. What does it mean if Keq < 1, at equilibrium? The concentration of reactants is greater than the concentration of products. b. The concentration of products is greater than the concentration of reactants. The rate of the forward reaction is greater than the rate of the reverse reaction. c. d. The rate of the reverse reaction is greater than the rate of the forward reaction. e. The concentration of products and reactants are about the same. Which of the...
Determine the numerical value of Keq at 25 °C for the electrochemical reactions below. I haven’t lectured on this in class, but the “how-to” is clearly illustrated in the textbook in Chapter 19. (a) PbO2(s) + 4 H+(aq) + 2 Cl–(aq) → ← Pb2+(aq) + 2 H2O(l) + Cl2(g) (acidic solution) Keq____________________________ (b) 3 O2(g) + 2 Br–(aq) → ← 2 BrO3–(aq) (basic solution) Keq____________________________
For the reaction, Br2(g) ⇌ 2Br(g) the equilibrium constant, Kc is 1.10 × 10−3 at 1280°C. Determine the initial and equilibrium concentrations of Br if the initial and equilibrium concentrations of Br2 are 5.90 × 10−3 M and 5.20 × 10−3 M, respectively. [Br]i = M [Br]e = M
If the equilibrium constant (Keq) for a reaction (CaCO3(s) → Ca2+ + CO32-) at 25 °C is 3.3*10-9, what is the ΔG° for the reaction (round your answer to the nearest kJ/mol)?