In this virtual lab, you'll learn how to calculate the empirical formula of magnesium chloride by reacting solid magnesium with hydrochloric acid. Through a sequence of steps, you'll create magnesium chloride, gaining hands-on experience with chemical reactions in a virtual environment. You will deduce the Empirical Formula of Magnesium based on the mole ratio of Magnesium and Chlorine.
Empirical Formula Understanding: Master the scientific method to identify the simplest ratio of magnesium to chlorine in a compound.
Scientific Method Application: Participate in a virtual experiment that involves mixing chemicals, observing their reactions, and interpreting the results.
Data Collection: Create a data table and record the collected data with the correct units.
Data Analysis & Calculations: Determine the mole ratio of magnesium to chlorine using your measurements to calculate the empirical formula of magnesium chloride.
Data Collection: Create a data table and record the collected data with the correct units.
Critical Thinking Development: Analyze the experiment's outcomes, especially unexpected ones, to understand the potential reasons behind them.
1. Completing the Pre-lab Activity:
a. Answer the pre-lab questions to prepare for the experiment.
b. Review your answers with your teacher to ensure you're ready to proceed.
2. Conducting the Experiment:
a. Begin the experiment by watching the instructional video provided in the FORMATIVE activity.
b. Carefully follow the step-by-step instructions, completing all sections as you go.
c. Accurately record all measurements and observations in FORMATIVE.
3. Completion and Submission: Once you've completed the experiment and answered all questions, review your work to ensure accuracy.
Submit your lab activity through FORMATIVE, making sure every section is thoroughly completed.
4. Reflection: Reflect on the experiment and your findings. Think about what you've learned regarding empirical formulas and any obstacles you encountered during the lab. This is a crucial step in deepening your understanding of the scientific process and its application.
The title of this lab is
What is the molecular formula (MF) of a compound whose empirical formula is X2Y, given that the empirical formula mass is 10.33 g/mol and the compound's molecular molar mass is 31 g/mol?
What is the mass of magnesium in this reaction?
Calculate the mass of chlorine.
Calculate and select the moles of magnesium and chlorine.
What is the Empirical Formula (EF) of Magnesium Chloride.
Magnesium Chloride has a Molar mass of 95.221 g/mol. Find the Molecular Formula of Magnesium Chloride.
Think about the experiment and what you discovered. Write a short paragraph about what you learned about empirical formulas and any problems you had during the lab.