13.The rate of a chemical reaction normally as reactant concentration increases.
14. Why does a higher concentration make a reaction faster?
15. What units represent a reaction rate?
16.If a reaction has an equilibrium constant (Keq) just greater than 1, how do we interpret that information?
17.A catalyst works by
18.If sulfur dioxide and oxygen can be made into sulfur trioxide, what is the reverse reaction?
19. What are 3 ways to increase rate of reaction?
20. Identify A, B, C, D and E!
13. Generally, the rate of a chemical reaction increases as reactant concentration increases.
14. A higher concentration of reactants increases the frequency of collisions between particles, leading to a higher chance of effective collisions. This increases the rate of reaction.
15. The units representing a reaction rate vary depending on the specific reaction being studied. Some common units include mol/L/s, M/s, or s^-1.
16. If a reaction has an equilibrium constant (Keq) just greater than 1, it suggests that the concentration of products is slightly greater than the concentration of reactants at equilibrium. This indicates that the reaction favors the formation of products.
17. A catalyst works by providing an alternative pathway with lower activation energy for the reaction to occur. It increases the rate of reaction by speeding up the rate-determining step.
18. The reverse reaction of sulfur dioxide and oxygen forming sulfur trioxide would be the decomposition of sulfur trioxide to sulfur dioxide and oxygen.
19. Three ways to increase the rate of a reaction are: increasing reactant concentration, increasing temperature, and using a catalyst.
20. Without specific context, it is unclear what A, B, C, D, and E refer to. Please provide more information or a specific question for clarification.