Which statements explains the energy requirements of chemical reactions?

A) The rate of reaction increases with both increasing temperature and activation energy.

B) The rate of reaction increases with increasing temperature and decreasing activation energy.

C) The rate of reaction increases with decreasing temperature and increasing activation energy.

D) The rate of reaction increases with both decreasing temperature and activation energy.

Which of the following describes the reaction in the energy diagram below?

True or False. Although a catalyst does take part in the reaction, it is not consumed since it reacts in one step and is then regenerated in the next step.

Describe what happens to the rate of the reaction of H₂ and Cl₂ in a cylinder with a movable piston when a catalyst is added. 

H₂ (g) + Cl₂ (g) → 2 HCl (g)

The following reaction was studied in an experiment: Ag⁺(aq) + Cl⁻(aq) → AgCl(s), and the data are listed below. Calculate the average rate of the reaction for the time interval 120s to 180s.

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?

Estimate the instantaneous rate of formation of O₂ at 70 s for the reaction based on the given graph.

2 N₂O₅ → 4 NO₂ + O₂

How does the rate constant change with increasing activation energy?

The rate constant values for a hypothetical reaction are 1.250×10⁻⁴ s⁻¹ and 8.764×10⁻³ s⁻¹ at 345 K and 360 K, respectively. Calculate the value of activation energy.

The decomposition of nitramide (O₂NNH₂) is being studied where the concentration–time data for nitramide (O₂NNH₂) and H⁺ were gathered. Nitramide decomposes into nitrous oxide (N₂O) gas and water. What is the balanced reaction equation?

Identify the rate law for the theoretical three-step mechanism below: 

A₂ ↔ A Fast 

A + CB → C + BA Slow

A + BA → BA₂ Fast 

The following data were gathered for the reaction

CD → C + D

Time(s)   [CD] (M)

0             1.00

10            0.833

20           0.714

30           0.625

40           0.555

50           0.505

60           0.455

Determine the following:

a. Order of the reaction

b. Rate constant of the reaction

c. Concentration of CD at 80 s

The components of a reaction after 0 mins and 20 mins are shown below.

After 7 half-life periods, what fraction of reactant is still present if the reaction is first-order?

A hypothetical reversible reaction M → N is represented by the following five figures. Blue spheres represent M while yellow spheres represent N. The progress of the reaction is depicted by the figures from left to right. Does the reaction reach equilibrium in any of the figures? If so, which figure(s) show the system in equilibrium?

The equilibrium constant for the following decomposition reaction at 75.0 °C is 2.73. 

NH₃BF₃(s) ⇌ NH₃(g) + BF₃(g)

What is the minimum amount of NH₃BF₃(s) in grams that has to be added to a 0.350 L flask in order to reach equilibrium?

Calculate K_c for each reaction. b. CH₄(g) + H₂O(g) ⇌ CO(g) + 3 H₂(g), K_p = 2.5 x 10³ (at 1200 K)

At 298 K, the K_c for the reaction 2 H₂S(g) ⇋ 2 H₂(g) + S₂(g) is 1.67×10⁻⁷. What is the K_c for the reaction H₂S(g) ⇋ H₂(g) + 1/2 S₂(g) at the same temperature?

Consider the hypothetical reaction P₂ + Q₂ ⇌ 2 PQ. Provided in the table below are the rate constants of the forward and reverse reactions at different temperatures.

Determine if the reaction is endothermic or exothermic and justify your answer.

A reaction vessel at 27 °C contains a mixture of SO₂ (P = 3.00 atm) and O₂ (P = 1.00 atm). When a catalyst is added, this reaction takes place: 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g). At equilibrium, the total pressure is 3.75 atm. Find the value of K_c.

Consider the reaction for the dissolution of Barium carbonate:

BaCO₃(s) ⇌ Ba²⁺(aq) + CO₃^2-(aq) K_c = 8.10 x 10^-8 at 25°C

Identify if additional solid barium carbonate is dissolved if it was added to a solution 2.0-L solution that already contains 15.02 g BaCO₃.