Le Chatelier's Principle Hydrogen gas can be generated from propane by the following catalyzed reaction, performed in a closed container. C3H8(g) + 5O2(g) + heat → 3CO2(g) + 4H2O(g) Indicate the direction in which the equilibrium position would shift as a consequence of each of the following actions: - Heating the equilibrium mixture - Decreasing the size of the reaction container - Increasing the pressure in the container by adding an inert gas - Decreasing the relative concentration of H2 (by removal)
Added by Karen J.
Step 1
Heating the equilibrium mixture: Since the reaction is endothermic (requires heat), increasing the temperature will shift the equilibrium to the right to consume the added heat. So, the equilibrium will shift in the direction of the Show more…
Show all steps
Your feedback will help us improve your experience
Madhur L and 65 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Using the Le Chatelier's principle, answer the following questions: When some product is removed from an equilibrium mixture more reactants are formed At constant temperature, if the volume of a mixture of gases in equilibrium is reduced, the system shifts in the direction that reduces the total number of moles of gas
Adi S.
Le Chatelier's Principle (2 parts) Hydrogen gas can be generated from methane by the following catalyzed reaction, performed in a closed container: CH4(g) + H2O(g) + heat = CO(g) + 3H2(g) Indicate the direction in which the equilibrium position would shift as a consequence of each of the following actions: Left Right Right No Effect increasing the pressure in the container by adding an inert gas refrigerating the warm equilibrium mixture Increasing the size of the reaction container adding a catalyst to the mixture Ammonia gas can be synthesized by the following catalyzed reaction, performed in a closed container: N2(g) + 3H2(g) = 2NH3(g) + heat Indicate the direction in which the equilibrium position would shift as a consequence of each of the following actions: Right Left Right Right decreasing the relative concentration of NH3 (by removal) heating the equilibrium mixture adding N2 to the mixture increasing the pressure in the container by adding an inert gas
Susan H.
A chemical equilibrium between gaseous reactants and products is shown: N2(g) + 3H2(g) ⇌ 2NH3(g). How will the reaction be affected if the pressure on the system is increased? It will shift toward the reactant side as there is lower pressure on the reactant side. It will shift toward the product side as there is higher pressure on the product side. It will shift toward the reactant side as there are a greater number of moles of gas on the reactant side. It will shift toward the product side as there are fewer number of moles of gas on the product side.
Jennifer H.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD