The balanced equation for the reaction of sodium sulfide with hydrogen bromide is as follows. 

2 HBr(aq) + Na₂S(aq) → H₂S(g) + 2 NaBr(aq)

What is the value of Δ[H₂S]/Δt if Δ[HBr]/Δt = 2.8×10^—3 M/s during the same time period?

Consider the following gas-phase reaction:

C₂H₁₁N (g) → 2 CH₄ (g) + NH₃ (g)

In relation to the rate at which the products form, what is the rate at which the reactant disappears?

Consider the formation of NO₃ in the following reaction: N₂(g) + 3 O₂(g) → 2 NO₃(g). What is the relationship between the rate of consumption of N₂ and O₂?

Calculate the average rate of appearance of SO₂ across the following time intervals all centered on t = 175 min. Identify the best estimate for the instantaneous rate of appearance of SO₂ at t = 175 min and explain why.

(i) 50 to 300 min

(ii) 150 to 200 min

(iii) 100 to 250 min

(iv) 0 to 350 min

Using the given kinetic data below for the reaction B → C + D, approximate the instantaneous rate at t = 40 s.

A particular reaction has an activation energy equal to 80 kJ/mol at 500 K. Find the fraction of the molecules in a gas that will collide with an energy equal to or greater than the activation energy at 500 K. If the activation energy at the same temperature is 160 kJ/mol, determine the value of this fraction.

Which of the following reactions will be the fastest? Assume that the collision factors for the reactions are equal.

Reaction rates can be explained using collision theory. Which statement(s) explain(s) why decreasing the temperature would decrease the reaction rate according to collision theory.

I. Decreasing the temperature increases the activation energy of the reaction.

II. Decreasing the temperature decreases the activation energy of the reaction.

III. Decreasing the temperature increases the amount of molecules with sufficient energy.

IV. Decreasing the temperature decreases the amount of molecules with sufficient energy.

V. Decreasing the temperature increases the amount of collisions with correct orientation.

VI. Decreasing the temperature decreases the amount of collisions with correct orientation.

Consider the following first-order reaction:

2 N₂O₅(g) → 2 N₂O₄(g) + O₂(g)

If the reaction has an activation energy of 103 kJ/mol and an Arrhenius constant of 2.01×10¹³ s^–1, calculate the rate constant of the reaction at 650 K.

A catalyst increases a chemical reaction's rate by lowering its activation energy. A particular chemical reaction has an activation energy of 125 kJ/mol at 45 °C. The activation energy is lowered by 55 kJ/mol when a catalyst is added to the reaction. Calculate the factor by which the rate of the reaction is increased. Assume that the frequency factor remains the same.

Calculate the fraction of xenon (Xe) atoms having an energy of 6.40 kJ/mol or greater at a temperature of 150 °C?