The equation for the formation of hydrogen iodide from H_2 and l_2 is: H_2(g) + I_2(g)...
Hydrogen iodide undergoes decomposition according to the equation 2HI(g) reversiblearrow H_2(g) + I_2(g) The equilibrium constant K_P at 500 K for this equilibrium is 0.060. Suppose 0.316 mol of HI is placed in a 8.00-L container at 500 K. What is the equilibrium partial pressure of I_2(g)? (R = 0.0821 L middot atm/(K middot mol)) 0.040 atm 0.020 atm 0.062 atm 0.0078 atm 0.32 atm
K_c for the reaction of hydrogen and iodine to produce hydrogen iodide, H_2 (g) + I_2 (g) 2HI (g) is 54.3 at 430 degree C. Determine the initial and equilibrium concentration of HI if initial concentrations of H_2 and I_2 are both 0.10 M and their equilibrium concentrations are both 0.043 M at 430 degree C. [HI]_i = M [HI]_e = M
K_c for the reaction of hydrogen and iodine to produce hydrogen iodide, H_2(g)+I_2(g) doubleheadarrow 2HI(g) is 54.3 at 430 degree C. Determine the initial and equilibrium concentration of H_2and I_2 are both 0.11 M and their equilibrium concentrations are both 0.048 M at 430 degree
A student ran the following reaction in the laboratory at 677 K: 2HI(g) H_2(g) + I_2(g) When she introduced HI(g) at a pressure of 5.32 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of HI(g) to be 4.22 atm. Calculate the equilibrium constant, K_p, she obtained for this reaction. K_p =
IV Consider the reaction: H_2 (g) + I_2 (g) = 2 HI(g) A reaction mixture in a 4.25 L flask at a certain temperature initially contains 0.668 g H_2 (g) and 86.9 g of I_2 (g). At equilibrium, the flask contains 78.4 g HI. Calculate K_c degree for this reaction at this temperature.
A chemical engineer is studying the following reaction: H_2 (g) + I_2 (g) rightarrow 2 HI (g) At the temperature the engineer picks, the equilibrium constant K_p for this reaction is 0.11. The engineer charges ("fills") three reaction vessels with hydrogen and iodine, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions...
At 400 K, an equilibrium mixture of H_2, I_2, and HI consists of 0.068 mol H_2, 0.075 mol I_2, and 0.13 mol HI in a1.00-L flask. What is the value of K_p, for the flowing equilibrium? (R = 0.0821 L middot atm (K - mol)) 2HI_(g) Rightwardsharpoonoverleftwardsharpoon H_2 (g) + I_2 (g) A) 0.039 B) 3.4 C) 26 D) 0.29 E) 8.2 If K = 0.150 for A_2 + 2B Rightwardsharpoonoverleftwardsharpoon 2AB, what is the value of K for the...
The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g)+ HI(g) NH4I(s) at 400 °C is 4.65. (a) If the partial pressure of ammonia is PNH, 0.881 atm and solid ammonium iodide is present, what is the equilibrium partial pressure of hydrogen iodide at 400 °C? PHI atm (b) An excess of solid NH,I is added to a container filled with NH3 at 400 °C and a pressure of 1.17 atm. Calculate the pressures of NH(g) and HI(g)...
The equilibrium constant, K_c, for the following reaction is 55.6 at 698 K: H_2(g) + I_2(g) 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.351 moles of H_2 and 0.351 moles of I_2 are introduced into a 1.00 L vessel at 698 K. [H_2] = M [I_2] = M [HI] = M
Determining the Equilibrium Constant K_p: Methane (CH_4) reacts with hydrogen sulfide to yield H_2 and carbon disulfide, a solvent used in manufacturing rayon and cellophane: CH_4(g) + 2H_2S(g) Equilibrium CS_2(g) + 4 H_2(g) What is the value of K_p at 1000 K if the partial pressures in an equilibrium mixture at 1000 K are 0.20 atm of CH_4, 0.25 atm of H_2S, 0.52 atm of CS_2, and 0.10 atm of H_2?