ΔH is positive for the equilibrium N2 (g) + O2 (g) ↔ 2 NO (g). If we lower the temperature,
(A) the equilibrium shifts to the left (more N2 + O2 gases formed)
(B) the equilibrium shifts to the right (more NO gas formed)
(C) Equilibrium does not shift because there are the same number of molecules on left side as on the right
(D) Equilibrium does not shift because temperature does not affect the reaction rates
why?
ΔH is positive for the equilibrium N2 (g) + O2 (g) ↔ 2 NO (g). If...
The reaction 2SO2 (g) + O2 (g) ↔ 2SO3 (g) is exothermic and at equilibrium. Which of the following action will shift equilibrium left? A Lower environment temperature B Add O2 to the system C Add a catalyst to slow down the reaction D Add Ne gas to the equilibrium E Increase the volume of the reaction chamber
N2(g) + O2(g) equilibrium reaction arrow 2 NO(g); Kc = 5.6 ✕ 10−4 at 2098 K (a) What is the value of Kc for the reaction 2 NO(g) equilibrium reaction arrow N2(g) + O2(g) at the same temperature? (b) What is the value of Kc for the reaction 1/2 N2(g) + 1/2 O2(g) equilibrium reaction arrow NO(g) at the same temperature? (c) Does the equilibrium in (a) favor the reactant or the products? reactant products (d) Does the equilibrium in...
1.For the reaction at equilibrium 2 SO3↔ 2 SO2 + O2 (∆Horxn= 198 kJ/mol), if we increase the reaction temperature, the equilibrium will (1 point ) * No shift None of the above Question lacks sufficient information Shift to the right 2. For the equilibrium reaction 2 SO2(g) + O2(g) ↔ 2 SO3(g), ∆Horxn = -198 kJ/mol. Which one of these factors would cause the equilibrium constant to increase? (1 point ) * Add a catalyst Decrease the temperature None...
For the following exothermic reaction 3H2(g) + N2(g) ↔ 2NH3(g) + heat. In which direction does equilibrium shift if the temperature of the reaction vessel is raised. Select one: a. Reaction shifts towards products. b. There is no effect. c. reaction shifts towards reactants
The system, CO(g) + O2(g) 2 CO2(g), is exothermic and at equilibrium at a temperature. Predict how Kp changes and direction of the shift if the temperature is increased. Kp increases, and it shifts to the right. Kp increases, and it shifts to the left. Kp decreases, and it shifts to the left. Kp doe not change, and it does not shift to either direction. Kp decreases, and it shifts to the right.
Part A N2(g)+3Br2(g)⇌2NBr3(g) K=[NBr3]2[N2][Br2]3 K=[N2][Br2]3[NBr3]2 K=[NBr3][N2][Br2] K=[NBr3]2[N2][Br2]3 Part B C(s)+O2(g)⇌CO2(g) K=[CO2][O2] K=[O2][CO2] K=[CO2][O2] K=[CO2][O2][C] When heated, carbon reacts with water to produce carbon monoxide and hydrogen. C(s)+H2O(g)+heat⇌CO(g)+H2(g) Part C What effect does each of the following changes have on the equilibrium? Drag the appropriate stresses to their respective bins. add H2O, Add heat, lower temperature, remove CO Categories: Equilibrium shifts to products, Equilibrium shifts to reactants, Equilibrium doesn't shift
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...
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. The reaction below is not at equilibria and Q = 1.7. The equilibrium constant is K = 0.230. 2SO3(g) ⇌ 2SO2(g) + O2(g)...
Determine the value of K for the balanced reaction, 2 NOCl(g) ↔ N2(g) + O2(g) + Cl2(g) at 279 K 2 N2(g) + 2 O2(g) ↔ 4 NO(g); K = 6.503×10-62 NO + 1/2 Cl2(g) ↔ NOCl(g); K = 4.122×104
Nitrogen and oxygen react at high temperatures. N2(g) + O2(g) equilibrium reaction arrow 2 NO(g) ΔH = 182.6 kJ (a) Write the expression for the equilibrium constant (Kc) for this reversible reaction. (Concentration equilibrium expressions take the general form: Kc = [C]c / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.)