For the system: I2 (g) + H2 (g) ---> 2HI (g) DH = -9.4 kj. K = 62.5 at 800 K. What is the equilibrium constant at 333oC?
The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K. A mixture of H2, I2 and HI, each at 0.020 M, was introduced into a container at 700 K. Which of the following is true? At equilibrium, [H2] = [I2] = [HI]. No net change occurs because the system is at equilibrium. The reaction proceeds to the left producing more H2(g) and I2(g). The reaction proceeds to the right producing more HI(g). At equilibrium,...
ΔGf°(I2(g)) = 19
kJ/mol
7. For the reaction H2(g) +12(g) = 2HI(g) K = 50.0 at 721 K (a) What is AG at 721 K? (b) What is Kat 25 °C? (AG HI(g) = +1.7 kJ/mol)
A student ran the following reaction in the laboratory at 673 K: H2(g) + I2(g) 2HI(g) When she introduced 0.228 moles of H2(g) and 0.256 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 6.53×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.
The equilibrium constant K for the reaction H2(g) + I2(g) 2HI(g) is 51 at 300oC. A 2 L flask was filled with 1 mol H2 and 1 mol I2 at 300oC and the reaction was allowed to come to equilibrium. (i) Calculate the equilibrium concentrations of all three species. If this reaction was performed with the same quantities but at a higher pressure what would be the effect on the position of equilibrium? (ii) If an equilibrium reaction as drawn...
Consider the reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.69 −L flask at 500 K initially contains 0.377 g H2 and 17.93 g I2. At equilibrium, the flask contains 17.72 g HI. Calculate the equilibrium constant at this temperature.
The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K. H2(g) + I2(g) 2HI(g) If ΔH° for this reaction is -10.4 kJ, what is the value of Kp at 577 K? Kp =
A student ran the following reaction in the laboratory at 647 K: 2HI(g) H2(g) + I2(g) When she introduced 0.395 moles of HI(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 3.95×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.
Hydrogen iodide undergoes decomposition according to the equation 2HI (g) yields H2(g) + I2 (g) The equilibrium constant Kp at 500 K for this equilibrium is 0.060. Suppose 0.176 mol of HI is placed in a 5.00- L container at 500 K. What is the equilibrium concentration of H2?
Expression for equilibrium constant (k) for reversible reaction H2 + I2 <-> 2HI is:
A student ran the following reaction in the laboratory at 686 K: H2(g) + I2(g) 2HI(g) When she introduced 0.200 moles of H2(g) and 0.230 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 6.18×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc=?