2ClF(g) + O2(g) ↔ Cl2O(g) + F2O(g) &DELTA;H = 167 kJ/molrxn During the reaction above, the product yield can be increased by increasing the temperature of the reaction. Why is this effective?

The reaction is endothermic; therefore adding heat will shift it to the right.

Increasing the temperature increases the speed of the molecules, meaning there will be more collisions between them.

The reactants are less massive than the products, and an increase in temperature will cause their kinetic energy to increase more than that of the products.

The increase in temperature allows for a higher percentage of molecular collisions to occur with the proper orientation to create the product.www.crackap.com

Chemistry

College Board

Exam No：AP Chemistry Problem Set 2 Year：2024 Question No：APChemistry2024AP0087

Answer:

Knowledge points:

6.1 Endothermic and Exothermic Processes

6.9 Hess’s Law

7.1 Introduction to Equilibrium

7.9 Introduction to Le Châtelier’s Principle

Solution:

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2ClF(g) + O2(g) ↔ Cl2O(g) + F2O(g) &amp;DELTA;H = 167 kJ/molrxn During the reaction above, the product yield can be increased by increasing the temperature of the reaction. Why is this effective?

Answer:

Knowledge points:

Solution:

Related Question

2ClF(g) + O2(g) ↔ Cl2O(g) + F2O(g) &DELTA;H = 167 kJ/molrxn During the reaction above, the product yield can be increased by increasing the temperature of the reaction. Why is this effective?