Textbook Question
Consider the reaction 4 NH3(π) + 5 O2(π) β 4 NO(π) + 6 H2O(π), Ξπ» = β904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (e) add a catalyst
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Ch.15 - Chemical Equilibrium
Chapter 15, Problem 64
For a certain gas-phase reaction, the fraction of products in an equilibrium mixture is increased by either increasing the temperature or by increasing the volume of the reaction vessel. Does the balanced chemical equation have more molecules on the reactant side or product side?
Verified step by step guidance1
Step 1: Understand Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
Step 2: Consider the effect of increasing temperature on the equilibrium. For an endothermic reaction, increasing temperature shifts the equilibrium towards the products, while for an exothermic reaction, it shifts towards the reactants.
Step 3: Analyze the effect of increasing the volume of the reaction vessel. According to Le Chatelier's Principle, increasing the volume decreases the pressure, and the equilibrium will shift towards the side with more moles of gas to increase the pressure.
Step 4: Since both increasing temperature and volume increase the fraction of products, the reaction is likely endothermic and has more moles of gas on the product side.
Step 5: Conclude that the balanced chemical equation has more molecules on the product side, as both changes favor the formation of products.
Related Practice
Textbook Question
Consider the reaction 4 NH3(π) + 5 O2(π) β 4 NO(π) + 6 H2O(π), Ξπ» = β904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (f) increase temperature.
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Open Question
How do the following changes affect the value of the equilibrium constant for a gas-phase exothermic reaction: (a) removal of a reactant, (b) removal of a product?
Textbook Question
Consider the following equilibrium between oxides of nitrogen 3 NO(g) β NO2(g) + N2O(g) (a) Use data in Appendix C to calculate ΞHΒ° for this reaction.
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Textbook Question
Methanol (CH3OH) can be made by the reaction of CO with H2: CO(π) + 2 H2(π) β CH3OH(π) (a) Use thermochemical data in Appendix C to calculate ΞHΒ° for this reaction.
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Textbook Question
Methanol (CH3OH) can be made by the reaction of CO with H2: CO(π) + 2 H2(π) β CH3OH(π) (b) To maximize the equilibrium yield of methanol, would you use a high or low temperature?
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