g. For the gas-phase equilibrium described above (see problemi (0) quilibrium described above (see problemlol) an...
True or False, explain why please. 3 q. For the gas-phase equilibrium described above (see probleml (o)), an increase in pressure will force the reaction to the right. This results in fewer total molecules and a lower pressure overall. r. For the gas-phase equilibrium described below, an increase in pressure will force the equilibrium to the left. 2HI() Hz(9) + 1 (8) S. The equilibrium constant helps us to predict the direction and completeness of an equilibrium reaction. t. If...
True or False t. For an exothermic reaction, the equilibrium constant, Kc, becomes smaller as the temperature increases and larger as the temperature decreases. u. The gas-phase equilibrium shown below is used to produce ammonia, NH3, for commercial applications. The NH3 yield can be increased by decreasing the temperature, increasing the pressure, and removing some NH; from the mixture. N2(g) + 3H2(g) - 2NH3() AH = -94 kJ. v. For the gas-phase equilibrium described above (see problemlu), an increase in...
The reaction by which bromoform (CHBr3) transfers between an aqueous and a gas phase is described by the equation: CHBr3(aq) ⇔ CHBr3(g) Equilibrium constants of the reaction were determined experimentally at three temperatures and are tabulated below. Temperature, C 4 20 30 K 0.0071 0.0170 0.2800 Use the equilibrium data provided in the table to estimate the standard enthalpy of the reaction and the equilibrium constant at 15°C.
All questions are true or false A catalyst changes both the equilibrium constant and the rate of a chemical equilibrium. j. Ifthe temperature of a chemical equilibrium is increased, the reaction will shift in a direction that will lead to the consumption of some of the extra heat. An increase in temperature favors an endothermic reaction over an exothermic reaction. k. nundifis Is ined If a chemical equilibrium is exothermic in the forward direction, it is also exothermic in the...
Question 5 0/1 point The equilibrium constant for the gas phase reaction N2 (g) + 3H2(g) + 2NH3 (B) is Keq - 4,34 x 10-3 at 300 °C. At equilibrium, Question 5 The equilibrium constant for the gas phase reaction N2 (8) + 3H2 (g) – 2N63 (g) is keq = 4.34 x 10-3 at 300 °C. At equilibrium, products predominate only reactants are present roughly equal amounts of products and reactants are present only products are present reactants predominate
2) Write the equilibrium constant expressions for each of the following reactions. (For gas-phase reactions, write the Ke expression.) a) 2 NO(g) + O2(g) = 2 NO2(g) b) 4 Ag(s) + O2(g) + 2 Ag2O(S) c) CaCO3(s) + CO2(aq) + H2O(l) = Ca2+(aq) + 2 HCO3(aq) 3) a) Write the K, expressions for reactions a and b in problem 2. b) If the value of K for reaction a in problem 2 is 2.8 x 1011 at 200°C, what is...
For each of the following reactions: (a) Write the Equilibrium expression (b) Calculate the Equilibrium Constant, Kc (c) Determine the DIRECTION of the reaction (d) Determine if the reaction is in Equilibrium (e) Determine the effect of INCREASING the temperature (f) Determine the effect of increasing the concentration of ONE of the reactants. (g) Determine the effect of increasing the volume of the container. (h) Determine the effect of increasing the Pressure in the container. Reaction 1: N204(g) 2NO2(g) Reaction...
1) 2) 3) 4) The equilibrium constant for the gas phase reaction 2803 (g) = 2802 (g) + O2 (g) is Keg = 7.1 x 102 at 999 K. At equilibrium,_ O only reactants are present O roughly equal amounts of products and reactants are present products predominate only products are present reactants predominate QUESTION 20 The rate law of a reaction is rate = k[X]-. The units of the rate constant are O mol L-15-2 OL mol-15-1 O mol2...
1. Write the equilibrium constant expressions (Kc) for the following reactions: (a) CO (g) + H2O (g) ⮂ CO2 (g) + H2 (g) (b) CH4 (g) + 2H2S (g) ⭢ CS2 (g) + 4H2 (g) (c) COCl2 (g) ⮂ Cl2 (g) + CO (g) (d) 2HI (g) ⮂ H2 (g) + I2 (g) (e) PCl3 + Cl2 (g) ⮂ PCl5 (g) (f) 2H2 (g) + O2 (g) ⮂ ...
please explain, thanks 1a. The equilibrium for the formation of HOCl in the gas phase from chlorine dioxide (C120) is given below. What are the expected equilibrium pressures if a cylinder has initial pressures as follows: PC120 = PH20 = 0.45 atm; Phoci = 0.65 atm ? (10 points) Cl20 (g) + H2O (g) = 2 HOCl2 (g) Kp=0.085 at 395 °C 1b. Does the total pressure in the cylinder increase, decrease or remain the same as the reactions goes...