How would each of the following change the rate of the reaction shown here? 2SO₂(g) + O₂(g) → 2SO₃(g)
a. adding more SO₂(g)

Question

How would each of the following change the rate of the reaction shown here? 2SO₂(g) + O₂(g) → 2SO₃(g)

a. adding more SO₂(g)

Accepted Answer

Welcome back, everyone consider the following reaction where two moles of selenium dioxide gas reacts with one mole of oxygen gas to form two moles of selenium trioxide gas, determine the effect on the reaction rate if two moles of selenium dioxide are added. So, selenium dioxide is our first reactant listed out. And if we are adding two moles of selenium dioxide, then therefore, we are increasing our concentration of selenium dioxide in the reaction, which will correspond to an increase in the number of collisions and they should have one. So in the number of collisions between our reactants, selenium dioxide and oxygen in the same volume of space. And so therefore, that would correspond to an increase in our reaction rate of our entire reaction. So our reaction would happen faster. And this would make sense because if we recall collision theory, which states that our reaction will occur when our reactants collide with sufficient energy. And that is in reference to our activation energy, which is represented as sub not only is our reaction occurrence dependent upon the activation energy, but also depends on the proper orientation of our reactant molecules. So we'll say and proper orientation. So overall, we can summarize that according to collision theory, an increase in our concentration of reactants will correspond to an increase in the number of collisions of our reactants in a in the same volume of space per unit of time, which correlates to an increase in our reaction rate. And again, the activation energy relates to the energy needed for our reactant molecules to have a successful collision with one another for the reaction to occur to form our product. In this case, our selenium trioxide gas. So with all of this outlined in summary, our final answer is going to be that if we increase our concentration of our reactant selenium dioxide, we have an increase in our reaction rate. So our increased reaction rate is our final answer. I hope this made sense and let us know if you have any questions.

How would each of the following change the rate of the reaction shown here? 2SO₂(g) + O₂(g) → 2SO₃(g)
a. adding more SO₂(g)

Verified video answer for a similar problem:

Key Concepts

Reaction Rate

Le Chatelier's Principle

Concentration Effects

How would each of the following change the rate of the reaction shown here? 2SO2(g) + O2(g) → 2SO3(g)a. adding more SO2(g)

Verified video answer for a similar problem:

Key Concepts

Reaction Rate

Le Chatelier's Principle

Concentration Effects

How would each of the following change the rate of the reaction shown here? 2SO₂(g) + O₂(g) → 2SO₃(g)
a. adding more SO₂(g)