For the following reaction: A(g) + 2 B(g) ⇌ 2 C(g) Calculate the equilibrium constant K given the following information: The initial pressure of A is 2.755 bar and the initial pressure of B is 1.582 bar The equilibrium pressure of C is 0.460 bar B)For the following reaction: 2 A(g) + B(g) ⇌ C(g) Calculate the equilibrium constant K given the following information: The initial pressure of A is 2.772 bar and the initial pressure of B is 2.645 bar The equilibrium pressure of C is 0.739 bar C)For the following reaction: A(aq) + B(aq) ⇌ 2 C(aq) Given the following information, what is the equilibrium concentration of C in mol L-1? Initial concentration of A = 1.081 mol L-1 Initial concentration of B = 1.081 mol L-1 Initial concentration of C = 0 mol L-1 K = 6.1 x 10-5
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For the following reaction: A(g) + 2 B(g) ⇌ 2 C(g) Calculate the equilibrium constant K...
For the following reaction: A(g) + 2 B(g) ⇌ 2 C(g) Calculate the equilibrium constant K given the following information: The initial pressure of A is 2.755 bar and the initial pressure of B is 1.582 bar The equilibrium pressure of C is 0.460 bar B)For the following reaction: 2 A(g) + B(g) ⇌ C(g) Calculate the equilibrium constant K given the following information: The initial pressure of A is 2.772 bar and the initial pressure of B is 2.645...
For the following reaction: A(g) + 2 B(g) ⇌ 2 C(g) Calculate the equilibrium constant K given the following information: The initial pressure of A is 1.831 bar and the initial pressure of B is 3.460 bar The equilibrium pressure of C is 0.520 bar
For the reaction 2 A(g) + 3 B(g) <-->2 C(g) + 2 D(g), the equilibrium constant at 298 K is 1.605×10-11. If the initial partial pressures of A, and B are 0.564 bar, and 0.728 bar, respectively, determine the partial pressure of D (in bar) once equilibrium has been reached at 298 K.
For the following reaction: A(g) + B(g) ⇌ 2 C(g) Given the following information, what is the equilibrium pressure of C in bar? Initial pressure of A = 2.629 bar Initial pressure of B = 2.629 bar Initial pressure of C = 0 bar K = 9.6 x 10-4
For the following reaction: 2 A(g) ⇌ B(g) + C(g) Given the following information, what is the equilibrium pressure of B in bar? Initial pressure of A = 1.386 bar Initial pressure of B = 0 bar Initial pressure of C = 0 bar K = 8.1 x 10-4 You have 5 attempts at this question.
A.) Given the reaction 2A + B ⇋ 4 C (all gases) concentrations at equilibrium are A = 0.076 M B = 0.829 M If K = 3.32, find the concentration of C and report it in M units. B.) Cu (s) + 2 Ag+ ⇋ Cu2+ (aq+) + 2 Ag(s) K = 7.88 x 104 PbCl2 (s) ⇋ Pb2+ (aq) + 2 Cl- (aq) K = 2.4 x 10-4 AgI (s) ⇋ Ag+ (aq) + I- (aq) K =...
For the following reaction: A(g) ⇌ 2 B(g) Given the following information, what is the equilibrium pressure of B in bar? Initial pressure of A = 1.039 bar Initial pressure of B = 0 bar K = 7.3 x 10-5 Using the quadratic equation my answer was 4.34*10^-3 or 0.00434 bar and apparently it is wrong!!!!! am i doing something wrong?
For the reaction 2 A(aq) ⇋ 2 B(g) + C(g), the equilibrium constant is 5.20 at 25.0oC. If the concentrations of B(aq) and C(aq) are each 0.278 M, what concentration of A(aq) is required to have a ΔG value of -10.0 kJ/mol?
Question 3 35 pts Determine the value of the equilibrium constant (K) for the reaction listed below based on the concentrations provided. Alaq) + 2 B(aq) = 3(aq) + D(aq) Reagent/Product A B C D 0.17 0.69 149 0.87 Concentration (mol/L) Question 4 35 pts Determine the equilibrium molar concentration of C in the following reaction if the initial molar concentration of Ais 0.10 M and Bis 0.25 M. The equilibrium constant for the reaction is 78. A(aq) + B(aq)...
Thank you Question 5: (1 point) At 390 K, the equilibrium constant, K., for the reaction below is 1.8 x 10-?. PCIs (g) - PC1; (g) + Cl2 (g) Assume a quantity of PCIs (g) is placed in a rigid 10 L vessel and the system is allowed to reach equilibrium at a constant temperature of 390 K. Identify whether each of the following statements is true or false. At equilibrium, if the vessel contains I mole of PCs (g)...