According to Le Chatelier principle, a system at equilibrium when disturbed by an external agency will proceed in a direction in such a way to negate the disturbance to re-establish the equilibrium.
1. b. Left
Reaction will proceed in the direction in which I2 is produced, which is to the left.
2. A. Right
The excess H2 has to be consumed to attain equilibrium. So if reaction goes to right H2 will be consumed.
3. B. Left
Excess HI will be consumed if the reaction moves to the left.
4. B. Left
5. C. Neither
Increase in total pressure at constant volume will have no effect on the equilibrium.
6. B. Left
The reaction will move towards the direction in which heat is produced. Since heat is being produced when reaction goes to left it will be favored if temperature is decreased.
458kJ(heat) + H2(g) + 1260) $2H14) 1. If the concentration of I, decreases, the reaction favored...
1) The reaction below is exothermic 2SO2 (g) + O2(g) ⇌ 2SO3(g) + heat Le Châtelier's Principle predicts that _______ will result in an increase in the number of moles of SO3 (g) in the reaction container. Which direction will the reaction shift: ? left or right A) increasing the volume of the container B) increasing the amount of SO2 C) removing some oxygen D) increasing the temperature E) decreasing the pressure 2) Consider the following reaction at equilibrium: 2SO2 (g) + O2 (g) ⇌ 2SO3 (g) + heat ΔH...
5. Consider the reaction: N: (g) + 3 H2(g) = 2 NH, (g) + heat Determine the effects of the following stresses on the equilibrium. State whether the equilibrium will shift to the left, to the right or not at all. a. Increase [N:] b. Decrease [NH] c. Decrease [H:] d. Increase temperature e. Decrease total pressure f. Decrease volume g. Add helium in a container with fixed volume h. Add helium in a container with variable volume
QUESTION 1 The reaction 3 H2(g)+ N2g)2 NH3(g) is slightly reactant-favored at a certain temperature. Starting from the reaction at equilibrium concentration of reactants and products, which of the following actions will increase the concentration of NH3 that can be obtained.? Increase concentration of hydrogen gas. Decrease concentration of hydrogen gas. Increase concentration of nitrogen gas. Decrease concentration of nitrogen gas. Increase the pressure. Decrease the pressure.
35) Given the equilibrium reaction at constant pressure: 2HBr(g) + 72.7 kJ = H2(g) + Br2(g) When the temperature is increased, the equilibrium will shift to the A) left, and the concentration of HBr(g) will decrease B) right, and the concentration of HBr(g) will decrease C) right, and the concentration of HBr(g) will increase D) left, and the concentration of HBr(g) will increase
M. Given the system at euo N04g)+58.1 kJ+2 NOg) 14. Given the reaction at equilibrium: what will be the result ofan increase in temperature | at constant pressure? |NaCo) + hola) +21.6 kcal ++ NO(g) A) The equilibrium wil shift to the left, and the The equilibrium will shift to the right if the A) temperature increases B) temperature decreases C) pressure increases D) pressure decreases concentration of NO2(g) will decrease. B) The equilibrium will shift to the left, and...
For the reaction CHs (a) 3 H2 (a) <=---> CgH,2 (a) + heat Determine which of the following will shift the equilibrium to the left a) adding a catalyst b) decreasing the temperature c) increasing the pressure by decreasing the volume of the container d) increasing the concentration of H2 e) increasing the concentration of CeHe f) decreasing the concentration of C H12 g) more than one correct response h) no correct response O0000O
1. At a given temperature the Kp = 4.76x10-4 for the reaction: H2(g) + 12(g) = 2 HI(g) Calculate the equilibrium partial pressure of Hl if the original reaction mixture contains H2 gas at 0.752 atm, 12 gas at 0.752 atm and Hl gas at 0.134 atm. a) 0.321 atm b) 0.810 atm c) 0.0177 atm d) 0.015 atm e) 0.192 atm
Consider the equilibrium CH,(g) + H2O(g) + 206 kJ=CO(g) + 3 H2(g). Which of the following disturbances will NOT cause the system to shift to the right to reestablish equilibrium? Select one: a. The partial pressure of CH4 increases. b. The partial pressure of CO decreases. c. The volume decreases. d. The temperature increases. e. All of these will cause the system to shift to the right
Under what conditions will the following reaction be the most product-favored? N2O(g) + NO2(g) <==> 3 NO(g) ; H = + 156 kJ A. low pressure, low temperature B. high pressure, low temperature C. high pressure, high temperature D. low pressure, high temperature
29. Consider the following equilibrium CO2(g)+ H2()Co(g) + H20(g); Ke 1.6 at 1260 K Suppose 0.019 mol CO2 and 0.030 mol H2 are placed in a 3.00-L vessel at 1260 K. What is pressure of CO(g)? (R 0.0821 L atm/K mol) a. 4 atm b. 0.35 atm c. 1.6 atm d. 0.66 atm e. 1 atm