For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium constant if the temperature is increased?
Practice Questions
1 question
Q1
For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium constant if the temperature is increased?
Increases
Decreases
Remains the same
Depends on the pressure
For exothermic reactions, increasing the temperature shifts the equilibrium to the left, thus decreasing the equilibrium constant.
Questions & Step-by-step Solutions
1 item
Q
Q: For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium constant if the temperature is increased?
Solution: For exothermic reactions, increasing the temperature shifts the equilibrium to the left, thus decreasing the equilibrium constant.
Steps: 4
Step 1: Identify the type of reaction. The given reaction is N2(g) + 3H2(g) ⇌ 2NH3(g). This reaction is exothermic, meaning it releases heat.
Step 2: Understand what happens when temperature increases. For exothermic reactions, increasing the temperature adds heat to the system.
Step 3: Apply Le Chatelier's Principle. According to this principle, if you add heat to an exothermic reaction, the equilibrium will shift to the left to absorb the extra heat.
Step 4: Determine the effect on the equilibrium constant. When the equilibrium shifts to the left, the concentration of reactants increases and the concentration of products decreases, which results in a decrease in the equilibrium constant.
