What is Le Chatelier\'s principle? How would increasing the H_2(g) concentration
ID: 992836 • Letter: W
Question
What is Le Chatelier's principle? How would increasing the H_2(g) concentration affect the following equilibrium? N_2(g) + 3H_2(0) 2NH_3(g) What does the double arrow appearing in the preceding equation indicate? Under certain conditions, hydrogen gas will combine with oxygen gas to produce gaseous water. The following equilibrium results. 2H_2(g) + O_2(g) 2H_2O(g) The forward reaction is exothermic. How would increasing the amount of H_2O(g) affect the equilibrium? How would an increase in temperature affect the equilibrium?Explanation / Answer
1. When any system at equilibrium is subjected to change in concentration, temperature, volume, or pressure, then the system readjusts itself to (partially) counteract the effect of the applied change and a new equilibrium is established.
2. By adding H2 we are increasing the concentration of reactant so the reaction will move in forward direction so that more NH3 is formed and equilibrium is gained back.
3. The reaction is in equilibrium. I.e, reaction will go to a certain extent till a centain amount of product with respect to reactant is formed and the reaction will neither go in forward or reverse direction unless external factor like pressure or temprature is changed.
4. (1) the reaction will go in reverse direction to produce H2 and O2
(2) Since the reaction is exothermic, we can think heat as product, so by increasing temp. the reaction will go in reverse direction
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