Coal, which is primarily carbon, can be converted to natural gas, primarily CH 4 , by the exothermic reaction: C(s) + 2 H 2 (g) ⇌ CH 4 (g) Which disturbance will favor CH 4 at equilibrium? a. adding more C to the reaction mixture b. adding more H 2 to the reaction mixture d. lowering the volume of the reaction mixture f. adding neon gas to the reaction mixture

Hi everyone here we have a question asking us which of the following will increase the formation of ammonia in the following eggs are thermic reaction at equilibrium Nitrogen gasses plus three hydrogen gasses, forms to ammonia gasses a increasing into in the reaction. This is increasing the reactant so that will increase the amount of ammonia be decreasing hydrogen in the reaction. That is decreasing a reactant so that will decrease the ammonia see decreasing into in the reactant and that is the same as above. It is decreasing the reactant will decrease the amount of ammonia Removing NH three as it forms in the reaction, decreasing the product shifts the reaction to the right so it will increase ammonia. So our answer here is a ND increasing into in the reaction and removing ammonia as it forms in the reaction. Thank you for watching. Bye.

Ch.16 - Chemical Equilibrium

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Tro 6th Edition

Ch.16 - Chemical Equilibrium

Problem 75b

Chapter 16, Problem 75b

Coal, which is primarily carbon, can be converted to natural gas, primarily CH₄, by the exothermic reaction: C(s) + 2 H₂(g) ⇌ CH₄(g) Which disturbance will favor CH₄ at equilibrium?
a. adding more C to the reaction mixture b. adding more H₂ to the reaction mixture d. lowering the volume of the reaction mixture f. adding neon gas to the reaction mixture

Verified step by step guidance

Identify the reaction and the type of reaction: The given reaction is C(s) + 2 H2(g) ⇌ CH4(g). This is a reversible reaction, and changes in conditions can shift the equilibrium position.

Understand Le Chatelier's Principle: This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.

Analyze the effect of adding more H2: Adding more H2 increases the concentration of one of the reactants in the reaction mixture.

Predict the shift in equilibrium: According to Le Chatelier's Principle, increasing the concentration of H2 will shift the equilibrium to the right, towards the formation of more products.

Conclude the effect on CH4 production: Therefore, adding more H2 to the reaction mixture will favor the production of CH4 at equilibrium.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. This principle helps predict how a system at equilibrium will respond to changes in concentration, pressure, or temperature, allowing us to determine which direction the reaction will favor.

Equilibrium Constant (K)

The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. For the reaction C(s) + 2 H2(g) ⇌ CH4(g), K can be calculated using the concentrations of CH4 and H2, providing insight into the extent of the reaction and the favorability of products versus reactants.

Exothermic Reactions

Exothermic reactions are chemical reactions that release energy, usually in the form of heat, to the surroundings. In the context of the given reaction, the conversion of carbon and hydrogen to methane (CH4) is exothermic, meaning that increasing the concentration of reactants like H2 can shift the equilibrium towards the production of more CH4, thereby favoring the formation of the product.

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Textbook Question

Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. b. PCl₃(g) + Cl₂(g) ⇌ PCl₅(g) (volume is increased)

Textbook Question

Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. c. CaCO₃(s) ⇌ CaO(s) + CO₂(g) (volume is increased)

Textbook Question

This reaction is endothermic. C(s) + CO₂(g) ⇌ 2 CO(g) Predict the effect (shift right, shift left, or no effect) of increasing and decreasing the reaction temperature. How does the value of the equilibrium constant depend on temperature?

Textbook Question

Coal, which is primarily carbon, can be converted to natural gas, primarily CH₄, by the exothermic reaction: C(s) + 2 H₂(g) ⇌ CH₄(g) Which disturbance will favor CH₄ at equilibrium? c. raising the temperature of the reaction mixture

Textbook Question

Coal can be used to generate hydrogen gas (a potential fuel) by the endothermic reaction: C(s) + H₂O(g) ⇌ CO(g) + H₂(g) If this reaction mixture is at equilibrium, predict whether each disturbance will result in the formation of additional hydrogen gas, the formation of less hydrogen gas, or have no effect on the quantity of hydrogen gas. e. adding a catalyst to the reaction mixture