We’re being asked to identify the correct statement for the given reaction:
6 A(s) + 7 B(g) ⇌ 5 C(g) + 8 D(l) ΔH = –3226.6 kJ/mol
According to Le Chatelier’s Principle, if a system (chemical reaction) is at equilibrium and we disturb it, then the system will readjust to maintain its equilibrium state.
Since the reaction is exothermic, ΔH = (–), heat is given off as a product:
6 A(s) + 7 B(g) ⇌ 5 C(g) + 8 D(l) + heat
Now, let’s look at each given statement.
Consider the following reaction at equilibrium
6A (s) + 7B (g) ⇌ 5C (g) + 8D (l) ΔH = -3226.6 kJ/mol
Which one of the following statements is correct?
A. Increasing the temperature would shift the reaction right.
B. Increasing the temperature would decrease the value of K.
C. Increasing the total pressure on the system would cause the reaction to shift left.
D. Adding a catalyst would favor the forward reaction, causing the reaction to shift right.
E. Adding some A would cause the reaction to shift right.
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Le Chatelier's Principle concept. You can view video lessons to learn Le Chatelier's Principle . Or if you need more Le Chatelier's Principle practice, you can also practice Le Chatelier's Principle practice problems.
How long does this problem take to solve?
Our expert Chemistry tutor, Sabrina took 5 minutes and 5 seconds to solve this problem. You can follow their steps in the video explanation above.