states how reacting particles (atoms, ions, or molecules) must interact to start a chemical reaction. Calorimetry Law of Conservation of Mass Collision Theory Le Chatelier's Principle

Sketch a qualitative reaction energy diagram for a chemical reaction with and without a catalyst. Assume the uncatalyzed reaction is endothermic. Note: Because the sketches are only qualitative, the energies in them don't have to be exact. They only have to have the right relationship to each other. For example, if one energy is less than another, that fact should be clear in your sketch. energy Uncatalyzed reaction reactants reaction coordinate products energy Catalyzed reaction reactants reaction coordinate X products 5

What is the usefulness of catalysts?

What is the rate of a chemical reaction? The speed at which a reaction proceeds. The energy required for a reaction to occur. The amount of product formed in a reaction. O The amount of reactant consumed in a reaction.

Increasing the pressure on the following reaction will increase which of the chemicals present in the reaction?      PCl5 (g)  double arrows  PCl3 (g)  +  Cl2 (g)     PCl5       PCl3     Cl2     None of these

How do you label an energy diagram of a chemical reaction?   What is a catalyst and how does it increase chemical reaction rates?

Which among the following is needed by reacting molecules to overcome in order for products to be formed? Choose from the choices below:       Kinetic energy       Potential energy       Activation energy       Heats of reaction mixture

True or false? For chemical reactions that occurs in multiple steps, the fastest step in the reaction mechanism requires the most amount of energy to proceed.

Balance the following reaction and write the reaction rate. __CH3NH2(g) + __O2 --> __CO2(g) + __H2O(g) + __N2(g)

Restate the collision theory in your own words. Apply the concepts of collision theory to determine if the rate of reaction between zinc metal and hydrochloric acid will either increase or decrease under the following conditions: Decreasing the temperature of the hydrochloric acid Increasing the concentration of the hydrochloric acid Adding a catalyst to the reaction