Given the following equilibrium system, what will occur if the system is subjected to an increase in temperature?
[tex]CuCl_4^{2-}(a q) g r e e n \rightleftharpoons Cu^{2+}+(a q) b l u e+4 Cl^{1-}(a q)+e n e r g y[/tex]
A. Keq will decrease
B. the solution will turn more blue
C. the solution will shift right
D. nothing will change
Answer (1)
The reaction is endothermic, meaning it absorbs energy.
Increasing the temperature shifts the equilibrium to the right, favoring the forward reaction.
The solution turns more blue as more C u 2 + is produced.
The equilibrium shifts right.
Explanation
Understanding the Problem The given equilibrium system is:
C u C l 4 2 − ( a q ) g ree n ⇌ C u 2 + ( a q ) b l u e + 4 C l 1 − ( a q ) + e n er g y
When the system is subjected to an increase in temperature, we need to determine what will happen to the equilibrium.
Applying Le Chatelier's Principle The reaction is endothermic because energy is released (or written as a product) in the forward direction. According to Le Chatelier's principle, if the temperature is increased, the equilibrium will shift in the direction that absorbs heat.
Determining the Direction of the Shift Since the forward reaction absorbs heat, the equilibrium will shift to the right. This means that more C u 2 + and C l 1 − will be produced.
Determining the Effect on the Color of the Solution Since the forward reaction produces C u 2 + ( a q ) which is blue, the solution will turn more blue.
Determining the Effect on Keq Since the forward reaction is favored by an increase in temperature, the equilibrium constant Keq will increase.
Final Answer Based on the analysis, the correct answers are:
The solution will turn more blue.
The solution will shift right.
Examples
Consider a chemical reaction in a lab where you want to produce more of a specific product. If the reaction is endothermic (absorbs heat), increasing the temperature can shift the equilibrium towards the product side, increasing the yield. This principle is used in various industrial processes to optimize reaction conditions and maximize product formation. For example, in the Haber-Bosch process for ammonia synthesis, carefully controlling the temperature and pressure is crucial to achieving a high yield of ammonia.
