Kimia Dasar 2 : Kinetika dan Kesetimbangan Kimia

Summary

This script details an online practical session on chemical kinetics and equilibrium, covering various experiments. It begins by explaining the effects of diffusion using KMnO4 in water, comparing stirred and unstirred conditions. Next, the impact of catalysts on reaction rates is explored with hydrogen peroxide and FeCl3. The third experiment focuses on determining the reaction order of magnesium with HCl. Finally, the script examines the effect of temperature on gas equilibrium using copper wire and nitric acid under cold and warm conditions. Throughout, key observations and conclusions highlight the influence of these factors on chemical reactions.

Takeaways

• 😀 The experiment is focused on chemical kinetics and chemical equilibrium, where the impact of diffusion, mixing, temperature, and catalysts are studied.
• 😀 The first part of the experiment involves observing the effects of diffusion, using KMnO4 mixed with aquades. One sample is agitated, while the other is left still to compare diffusion rates.
• 😀 The experiment reveals that the sample with agitation diffuses faster than the one left undisturbed.
• 😀 In the second experiment, oxalic acid (H2C2O4) is mixed with sulfuric acid (H2SO4), and then KMnO4 is added to both mixtures to observe the difference in diffusion rates under stirring versus still conditions.
• 😀 In the third part, the influence of catalysts on the reaction rate is tested by adding FeCl3 and another catalyst to H2O2 solutions and observing how quickly oxygen is released.
• 😀 The presence of a catalyst speeds up the oxidation reaction of H2O2, showing the role of catalysts in increasing reaction rates.
• 😀 A reaction between magnesium (Mg) and hydrochloric acid (HCl) is studied to determine the reaction order. Different concentrations of HCl are used to observe how they affect the reaction rate.
• 😀 As the concentration of HCl increases, the reaction rate also increases, which helps determine the order of the magnesium-HCl reaction.
• 😀 The final part of the experiment focuses on the effect of temperature on a gas-phase equilibrium reaction involving copper and nitric acid, observing the differences in the reaction when cold and hot.
• 😀 In the cold experiment, the gas produced is brown and decreases over time, while in the hot experiment, the resulting color is green, indicating the influence of temperature on equilibrium.

Q & A

What is the primary focus of the chemistry practicum described in the script?

The practicum focuses on chemical kinetics and equilibrium, specifically studying the effects of diffusion, the influence of catalysts, the reaction order, and temperature on chemical reactions.

What is observed in the first part of the experiment related to diffusion?

In the first part, the experiment involves mixing KMnO4 (potassium permanganate) with water (aquades). One mixture is stirred, and the other is left undisturbed. The time it takes for the KMnO4 to diffuse and spread uniformly in water is measured.

What was concluded about the effect of stirring on diffusion?

It was observed that the solution that was stirred had a faster diffusion rate compared to the one that was left undisturbed.

What substances were mixed in the second part of the experiment related to diffusion?

In the second part, oxalic acid (H2C2O4) and sulfuric acid (H2SO4) were mixed, and KMnO4 was added to both mixtures. One was stirred, and the other was left undisturbed to observe the difference in diffusion rates.

How did the reaction behave in the experiment with oxalic acid and KMnO4?

The solution that was stirred showed a faster diffusion rate, while the one left undisturbed showed slower diffusion with remaining visible KMnO4.

What is the objective of studying catalysts in the practicum?

The objective is to observe how catalysts, specifically FeCl3 and HCl, affect the rate of a reaction involving hydrogen peroxide (H2O2).

What happens when a catalyst is added to the reaction between H2O2 and FeCl3?

When the catalyst is added, the reaction speeds up, as indicated by the rapid formation of bubbles due to the release of oxygen gas.

What reaction was studied in the section about determining reaction order?

The reaction studied was the interaction between magnesium (Mg) and hydrochloric acid (HCl). The goal was to determine the reaction order by varying the concentration of HCl and measuring the time it takes for the magnesium strip to completely react.

What effect did varying the concentration of HCl have on the reaction rate?

As the concentration of HCl increased from 0.6 M to 3 M, the rate of reaction also increased, leading to a faster consumption of the magnesium strip.

How did temperature affect the chemical equilibrium in the gas experiment?

In the gas experiment, temperature changes were shown to affect the equilibrium, with the reaction producing brown gas at higher temperatures and green at lower temperatures. The experiment also highlighted how gas production and dissolution occurred differently at cold and warm temperatures.