Question

question 1 (1 point)
which factor will not affect the rate of the following reaction?
na(s) + agno3(aq) --> nano3(aq) + ag(s)
the addition of a catalyst
an increase in pressure
an increase in the concentration of agno3(aq)
an increase in temperature
all of these factors will have a strong effect on the rate of the reaction
question 2 (1 point)
why does the rate of reaction increase with increasing temperature?
the activation energy decreases as the temperature increases.
changing the temperature usually alters the reaction mechanism, similar to the effect of a catalyst.
the change in temperature reduces the overall potential energy change between reactants and products.
a greater proportion of all the molecules possess kinetic energy that is equal to or greater than the activation energy.
hotter molecules stick together better.
question 3 (1 point)
potential energy diagram

Explanation:

• For Question 1:
• Catalysts lower activation energy and increase reaction rate.
• Increasing the concentration of \(AgNO_3(aq)\) (a reactant) increases the rate (more reactant particles to collide).
• Increasing temperature gives particles more kinetic energy, increasing collision frequency and energy (more effective collisions), so rate increases.
• The reaction has no gaseous reactants/products. Pressure affects gas - phase reactions (by changing gas concentration). Since there are no gases here, an increase in pressure has no effect on the rate.
• For Question 2:
• Activation energy (\(E_a\)) is a characteristic of the reaction and catalyst (if present), not temperature. So, the statement about \(E_a\) decreasing with temperature is wrong.
• Temperature change doesn't usually alter the reaction mechanism (catalysts do that by providing an alternative pathway).
• The overall potential energy change (\(\Delta H\)) between reactants and products is fixed for a reaction and not affected by temperature in terms of rate (it affects equilibrium position in some cases, but not the rate explanation here).
• According to the Maxwell - Boltzmann distribution, as temperature increases, a greater proportion of molecules have kinetic energy (\(KE\)) equal to or greater than \(E_a\). So, more molecules can overcome the activation energy barrier and react, increasing the rate.
• The statement “Hotter molecules stick together better” is not a valid scientific explanation for rate increase with temperature in terms of reaction kinetics.

Answer:

Question 1: B. an increase in pressure
Question 2: D. A greater proportion of all the molecules possess kinetic energy that is equal to or greater than the activation energy.