Question

question 6 (1 point)
which statement about the factors that affect reaction rates is false?
decreasing the concentrations of the reacting particles decreases the chance of collision.
a collision with poor orientation requires a higher activation energy than a collision with optimum orientation.
increasing the pressure in a gaseous reaction increases the chance of collision.
a reaction occurs every time particles of the reactants collide.
increasing the temperature increases the reaction rate.

Explanation:

For a reaction to occur, particles must collide with sufficient energy (activation energy) and proper orientation. Not every collision meets these criteria.

• Decreasing reactant concentrations reduces collision chances as there are fewer particles.
• Higher pressure in gas reactions (for gaseous reactants) means more particles per unit volume, increasing collision probability.
• Poor - orientation collisions need more energy to react compared to optimal - orientation ones.
• Increasing temperature gives particles more kinetic energy (more particles have energy ≥ activation energy), increasing the reaction rate.

Answer:

A reaction occurs every time particles of the reactants collide.