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 =
The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K. H2(g) + I2(g)...
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) ---------->2HI(g) 1) Calculate the equilibrium concentrations of reactants and product when 0.309 moles of H2 and 0.309 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] = M? [I2] = M? [HI] = M? 2.The equilibrium constant, K, for the following reaction is 1.20×10-2 at 500 K: PCl5(g)------->PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a...
The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) 2HI(g) Calculate the equilibrium partial pressures of all species when H2 and I2, each at an intitial partial pressure of 1.65 atm, are introduced into an evacuated vessel at 698 K.
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.293 moles of H2 and 0.293 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] = M [I2] = M [HI] = M
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.276 moles of H2 and 0.276 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] = _____M [I2] =______M [HI] =______M
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2 (g) + I2 (g) ---> 2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.301 moles of H2 and 0.301 moles of I2 are introduced into a 1.00 L vessel at 698 K. [ H2 ] = _______ M [ I2 ] = ________ M [ HI ] = _______ M
Consider the following equilibrium with a Kc = 55.6 at a temperature of 698 K. H2(g) + I2(g) <--> 2HI(g) ΔH0 = + 26.5 kJ / mol If the initial concentrations were [H2] = 0.12 M; [I2] = 0.041 M; and [HI] = 2.6 M. Is the system at equilibrium, and if not, in which direction must it shift to establish equilibrium? Justify your answer. At the same 698 K, 0.50 mol of H2 and 0.88 mol of I2 are...
The equilibrium constant, K, for the following reaction is 55.6 at 698 K: H2(g) + 12() 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.293 moles of H, and 0.293 moles of I, are introduced into a 1.00 L vessel at 698 K. [Hz] = [12] =
The equilibrium constant, Ky, for the following reaction is 55.6 at 698 K: H2(g) +12(g) =2HI(g) Calculate the equilibrium partial pressures of all species when H, and 13, each at an intitial partial pressure of 1.24 atm, are introduced into an evacuated vessel at 698 K. atm atm P1 PHI atm
Consider the following reaction where Kc = 55.6 at 698 K: H2(g) + I2(g) <------>2HI(g) A reaction mixture was found to contain 4.14×10-2 moles of H2(g), 3.91×10-2 moles of I2(g) and 0.258 moles of HI(g), in a 1.00 Liter container. Indicate True (T) or False (F)for each of the following: ___TF 1. In order to reach equilibrium HI(g) must be consumed. ___TF 2. In order to reach equilibrium Kc must decrease. ___TF 3. In order to reach equilibrium H2 must...
Consider the following reaction where Kc = 55.6 at 698 K: H2(g) + I2(g) --- 2HI(g) A reaction mixture was found to contain 2.56×10-2 moles of H2(g), 3.71×10-2 moles of I2(g) and 0.257 moles of HI(g), in a 1.00 Liter container. Indicate True (T) or False (F) for each of the following: ___TF 1. In order to reach equilibrium HI(g) must be produced. ___TF 2. In order to reach equilibrium Kc must increase. ___TF 3. In order to reach equilibrium...