Percobaan Laju Reaksi | Lab Kimia | UPT Laboratorium Terpadu UHO

Summary

In this chemistry experiment, students explore the effects of concentration, temperature, and catalysis on reaction rates using sodium thiosulfate and hydrochloric acid. The procedure involves two main phases: first, measuring the impact of varying concentrations on the reaction rate, and second, assessing how temperature influences the reaction. By observing the disappearance of a marked 'X' beneath the reaction mixture, students gain insights into the dynamics of chemical reactions. This engaging experiment aims to enhance understanding of fundamental concepts in reaction kinetics.

Takeaways

• 🎓 The experiment aims to demonstrate the effects of concentration, temperature, and catalysis on reaction rates.
• 🧪 Students are expected to explain how these factors influence reaction rates and identify observable changes in the mixtures.
• 🔬 Essential equipment includes 100 ml beakers, measuring pipets, stopwatches, thermometers, hot plates, marked paper, and clamps.
• 💧 The chemicals used in the experiment are Na2S2O3 solutions (0.5 M, 0.2 M), HCl (1 M, 2 M), and distilled water.
• ⚗️ The first stage of the experiment investigates the effect of concentration on reaction rates.
• ⏱️ For the first stage, students mix 6 ml of Na2S2O3 (0.2 M) with 9 ml of HCl (1 M) and time how long it takes for a marked 'X' to disappear.
• 🔄 The procedure is repeated using different concentrations of Na2S2O3 and HCl solutions.
• 🔥 The second stage examines how temperature affects reaction rates by heating the Na2S2O3 solution to 40°C.
• 📋 Students repeat the marking and timing process for different concentrations at the elevated temperature.
• ✨ The experiment is designed to provide practical understanding and insights into reaction kinetics.

Q & A

What is the main objective of the reaction rate experiment?

The main objective is for students to explain the influence of concentration, temperature, and catalysis on the reaction rate and to identify changes in the mixture as evidence of the reaction.

What equipment is used in this experiment?

The equipment used includes a 100 ml beaker, measuring pipette, stopwatch, thermometer, hot plate, marked X paper, and a test tube clamp.

What are the substances used in the experiment?

The substances used include Na2S2O3 in different molarities (0.5 M, 0.2 M), HCl in different molarities (1 M, 2 M), and aquades (distilled water).

Describe the first phase of the experiment.

In the first phase, the effect of concentration on the reaction rate is tested by mixing 6 ml of 0.2 M Na2S2O3 with 9 ml of 1 M HCl, observing the time taken for a marked X paper beneath the beaker to disappear.

How does temperature affect the reaction rate according to the experiment?

The second phase tests the effect of temperature by heating the 0.2 M Na2S2O3 solution to 40 degrees Celsius before mixing it with 9 ml of 1 M HCl and measuring the time for the marked X to disappear.

What observations should be recorded during the experiment?

Students should record the time taken for the marked X to disappear in each trial as an indication of the reaction rate.

What variations are tested in the concentrations of the reactants?

The experiment tests different combinations: 0.2 M Na2S2O3 with 2 M HCl, and 0.5 M Na2S2O3 with 2 M HCl to observe the effect on reaction rates.

What is the importance of using marked paper in the experiment?

The marked paper serves as a visual indicator to measure the time taken for the reaction to occur, providing a clear endpoint for the observations.

Why is it important for students to understand reaction rates?

Understanding reaction rates is crucial for grasping concepts in chemistry related to kinetics, which can influence how reactions are conducted in real-world applications.

What conclusion can be drawn from the experiment regarding reaction rates?

The experiment concludes that reaction rates can be significantly influenced by factors such as concentration and temperature, which are critical for understanding chemical reactions.