Consider the following equilibrium 2 NO(g) + Cl_2(g) 2 NOCl(g) Delta H degree_rx
ID: 522721 • Letter: C
Question
Consider the following equilibrium 2 NO(g) + Cl_2(g) 2 NOCl(g) Delta H degree_rxn = -77.0 Which of the following statements about this equilibrium is/are correct? (i) If the total is increased by reducing the volume of the container at constant temperature, then the equilibrium amount of NOCl in the mixture will increase. (ii) If the mixture is heated at constant pressure, the equilibrium will shift to the right. (iii) If the total pressure is doubled by reducing the volume of the container at constant T, the equilibrium partial pressures of all the gases in the mixture will double as well. A) (i) only B) (ii) only C) (i) and (ii) only D) (i) and (iii) only E) (i), (ii), and (iii)Explanation / Answer
Answer is A because it is true according to Le Chatelier's principle when the pressure of a reaction inceases which will try to decrease the pressure here to reduce the pressure equilibrium will shift towards right.