Skip to main content
Ch.15 - Chemical Equilibrium
Chapter 15, Problem 69b

(b) If the temperature is raised by 100 K, does the equilibrium constant for this reaction increase or decrease?

Verified Solution

Video duration:
3m
This video solution was recommended by our tutors as helpful for the problem above.
Was this helpful?

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 system will adjust to counteract the change and restore a new equilibrium. This principle helps predict how changes in temperature, pressure, or concentration will affect the position of equilibrium in a chemical reaction.
Recommended video:
Guided course
07:32
Le Chatelier's Principle

Temperature and Equilibrium Constant

The equilibrium constant (K) of a reaction is temperature-dependent. For exothermic reactions, increasing the temperature typically decreases K, while for endothermic reactions, increasing the temperature usually increases K. Understanding the nature of the reaction (exothermic or endothermic) is crucial to predicting how K will change with temperature.
Recommended video:
Guided course
02:33
Magnitude of Equilibrium Constant

Exothermic and Endothermic Reactions

Exothermic reactions release heat, resulting in a negative change in enthalpy (Ξ”H < 0), while endothermic reactions absorb heat, leading to a positive change in enthalpy (Ξ”H > 0). The classification of a reaction as exothermic or endothermic is essential for determining how the equilibrium constant will respond to temperature changes.
Recommended video:
Guided course
02:30
Endothermic & Exothermic Reactions
Related Practice
Textbook Question

Methanol (CH3OH) can be made by the reaction of CO with H2: CO(𝑔) + 2 H2(𝑔) β‡Œ CH3OH(𝑔) (c) To maximize the equilibrium yield of methanol, would you use a high or low pressure?

435
views
Textbook Question

Ozone, O3, decomposes to molecular oxygen in the stratosphere according to the reaction 2 O3(𝑔) ⟢ 3 O2(𝑔). Would increasing the pressure by decreasing the size of the reaction vessel favor the formation of ozone or of oxygen?

Textbook Question

(a) Is the dissociation of fluorine molecules into atomic fluorine, F2(𝑔) β‡Œ 2 β€Šβ€ŠF(𝑔), an exothermic or endothermic process?

711
views
Textbook Question

When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2: SO2Cl2(𝑔) β‡Œ SO2(𝑔) + Cl2(𝑔) (a) Calculate 𝐾𝑐 for this reaction at this temperature.

1261
views
1
rank
Textbook Question

When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2: SO2Cl2(𝑔) β‡Œ SO2(𝑔) + Cl2(𝑔) (c) According to Le ChΓ’telier's principle, would the percent of SO2Cl2 that decomposes increase, decrease or stay the same if the mixture were transferred to a 15.00-L vessel?

557
views
Textbook Question

A sample of nitrosyl bromide (NOBr) decomposes according to the equation 2 NOBr(𝑔) β‡Œ 2 NO(𝑔) + Br2(𝑔) An equilibrium mixture in a 5.00-L vessel at 100Β°C contains 3.22 g of NOBr, 2.46 g of NO, and 6.55 g of Br2. (b) What is the total pressure exerted by the mixture of gases?