Multiple Choice
A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H2(g) + N2(g) ⇄ 2NH3(g)
A) There will be no effect.
B) More ammonia will be produced at the expense of hydrogen and nitrogen.
C) Hydrogen and nitrogen will be produced at the expense of ammonia.
D) The equilibrium constant will increase.
E) The equilibrium constant will decrease.
Correct Answer:
Verified
Correct Answer:
Verified
Q28: Write the mass-action expression, Q<sub>c</sub>, for the
Q29: SO<sub>2</sub> reacts with O<sub>2</sub> to produce SO<sub>3</sub>.
Q30: Ammonium iodide dissociates reversibly to ammonia and
Q31: A good catalyst for a reaction will
Q32: Magnesium carbonate dissociates to magnesium oxide and
Q34: The following reaction is at equilibrium in
Q35: Hydrogen sulfide will react with water as
Q36: The equilibrium constant K<sub>c</sub> for the reaction
Q37: Write the mass-action expression, Q<sub>c</sub>, for the
Q38: Ethane can be formed by reacting acetylene