Answer:
-7.34 kilo Joules is the change in enthaply when 20.0 grams of nitrogen triiodide decomposes.
Explanation:
Mass of nitrogen triiodide = 20.0 g
Moles of nitrogen triiodide =
According to reaction, 2 moles of nitrogen triiodide gives 290.0 kilo Joules of heat on decomposition ,then 0.05063 moles of nitrogen triiodide will give :
-7.34 kilo Joules is the change in enthaply when 20.0 grams of nitrogen triiodide decomposes.
Answer:
Only changes in temperature will influence the equilibrium constant . The system will shift in response to certain external shocks. At the new equilibrium
will still be equal to
, but the final concentrations will be different.
The question is asking for sources of the shocks that will influence the value of . For most reversible reactions:
For some reversible reactions that involve gases:
Catalysts do not influence the value of . See explanation.
Explanation:
.
Similar to the rate constant, the equilibrium constant depends only on:
The reversible reaction is in a dynamic equilibrium when the rate of the forward reaction is equal to the rate of the backward reaction. Reactants are constantly converted to products; products are constantly converted back to reactants. However, at equilibrium the two processes balance each other. The concentration of each species will stay the same.
Factors that alter the rate of one reaction more than the other will disrupt the equilibrium. These factors shall change the rate of successful collisions and hence the reaction rate.
For reactions that involve gases,
However, there are cases where the number of gases particles on the reactant side and the product side are equal. Rates of the forward and backward reaction will change by the same extent. In such cases, there will not be a change in the final concentrations. Similarly, catalysts change the two rates by the same extent and will not change the final concentrations. Adding noble gases will also change the pressure. However, concentrations stay the same and the equilibrium position will not change.