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Predict the effect of each of the following on the indicated equilibrium system in terms of which reaction will be favored (forward, reverse, or neither)
H2(g)+Cl2(g)<=>2HCl(g) +184 kJ
A)addition of Cl2
B)removal of HCl
C)increased pressure
D)decreased temperature
E)removal of H2
F)decreased pressure
G)addition of a catalyst
H)increased temperature
I)decreased system volume

  • Chemistry -

    All of these are answered with a knowledge of Le Chatelier's Principle. You need to learn to do these yourself. Start by telling me what you don't understand about the principle and we can go from there. The first thing to remember is that whatever you do to a system in equilibrium, it will shift left or right to UNDO what you did. For example, a, the addition of Cl2. The system will shift to undo the addition. What exactly does that mean? It means that the system will shift to the right because reacting Cl2 with H2 is the only way to get rid of the Cl2 that has been added. Removing H2 will shift it to the left because forming more H2 is the way to add H2 to undo removing it.

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