Answer to Question #156795 in General Chemistry for Kimberli

Question

1. Based on the ​nature of the reactants​ in each of the equations below, which reaction at 25°C will occur at the fastest rate?

(1) C(s) + O​2​ (g) → CO​2​ (g)

(2) NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)

(3) CH​3O​ H(l) + CH​3C​ OOH(l) → CH​3C​ OOCH​3(​ aq) + H​2O​ (l) (4) CaCO​3(​ s) → CaO(s) + CO​2​(g)

2. In an experiment involving a reaction, it was found that an increase in temperature increased the rate of the reaction. Explain this result in terms of collision theory.

3. Which event must ​always ​occur for a chemical reaction to take place?

(1) formation of a precipitate

(2) formation of a gas

(3) effective collisions between reacting particles

(4) addition of a catalyst to the reaction system

Given the equation for a reaction at equilibrium:

2SO2 (g) + O2 (g) —> 2SO3 (g) + Energy

4. Explain, in terms of collisions between molecules

why increasing the concentration of O​2 (​ g) produces a ​decrease i​ n the concentration of SO​2​ (g).

Answer 1

1) 1,2

2) With an increase in temperature, there is an increase in energy that can be converted into activation energy in a collision, and that will increase the reaction rate. ... Increasing the concentration of a reactant increases the frequency of collisions between reactants and will, therefore, increase the reaction rate.

3) 1,2.

4) An increase in the concentration of a product will lead to a decrease in the amounts of all products and an increase in the amounts of all reactants. In both cases, there will be a net increase in the total amount of the added component, but the increase will be less than the amount added.