How would each of the following change the rate of the reaction shown here?
2 NO(g) + 2 H₂(g) → N₂(g) + 2 H₂O(g)
c. removing some H₂(g)

Verified step by step guidance

1. Identify the factors that influence the rate of a chemical reaction. These include concentration of reactants, temperature, presence of a catalyst, and surface area (if applicable). In this case, we are focusing on the concentration of H₂(g).
2. Understand the role of H₂(g) in the reaction. According to the balanced equation, H₂(g) is a reactant, and its concentration directly affects the reaction rate based on the collision theory. Fewer H₂ molecules mean fewer collisions with NO molecules.
3. Apply the concept of the rate law. The rate law for this reaction would depend on the concentrations of the reactants. If the reaction is second-order with respect to H₂(g), the rate would be proportional to [H₂]². Removing some H₂ would decrease its concentration, thereby reducing the reaction rate.
4. Consider the effect of removing H₂(g) on the equilibrium. While this question focuses on reaction rate, note that removing a reactant can also shift the equilibrium position of the reaction (Le Chatelier's Principle), but this is separate from the immediate rate change.
5. Conclude that removing some H₂(g) decreases the frequency of effective collisions between H₂ and NO molecules, leading to a slower reaction rate.

Key Concepts

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. In the context of a chemical reaction, if a reactant is removed, the equilibrium will shift to produce more of that reactant, thereby increasing the rate of the reaction until a new equilibrium is established.

Reaction Rate

The reaction rate refers to the speed at which reactants are converted into products in a chemical reaction. It can be influenced by various factors, including concentration, temperature, and the presence of catalysts. In this case, removing H₂(g) decreases its concentration, which can slow down the reaction rate as there are fewer reactant molecules available to collide and react.

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. Changes in concentration, such as removing H₂(g), can affect the position of equilibrium but do not change the value of K. Understanding K helps predict how the system will respond to changes in concentration.