Consider this chemical reaction: $C_2H_6(g) + 2I_2(s) \rightleftharpoons C_2H_4I_2(l) + 2HI(g)$ Which substance(s), if any, will NOT appear in the equilibrium constant expression? Select all correct answers. HI(g)
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2HI(g) --> H2(g) + I2(g) Keq = 0.0199 If 0.24 moles of each HI, I2, and H2 are mixed in a 3-L container, what happens as the reaction proceeds to equilibrium? a. The concentration of all materials remains the same. b. The H2 concentration increases more than the I2 concentration. c. The HI concentration increases. d. The H2 and I2 concentrations increase equally.
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Consider the following equilibrium: H2(g) + I2(s) → 2HI(g) Which of the following statements about the equilibrium is false? Answer choices: a) Adding more H2(g) does not increase the equilibrium constant. b) This is a homogeneous equilibrium. c) If the pressure on the system is increased by changing the volume, the right side is favored. d) Removing HI as it forms does not force the equilibrium to the right. e) If the system is heated, the right side is favored.
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For the reaction H2(g) + I2(g) ⇌ 2HI(g), Kc = 50.2 at 445°C. If [H2] = [I2] = [HI] = 1.75 x 10^-3 M at 445°C, which one of these statements is true? A) The system is at equilibrium, thus no concentration changes will occur. B) The concentrations of HI and I2 will increase as the system approaches equilibrium. C) The concentration of HI will increase as the system approaches equilibrium. D) The concentrations of H2 and HI will fall as the system moves toward equilibrium.
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