Final answer:
The provided student inquiries revolve around the calculation of molecular mass in chemistry, utilizing average atomic masses to determine the mass of a molecule, and conducting experiments with a focus on using averages and stratified sampling for data analysis.
Step-by-step explanation:
The questions presented pertain to the calculations of molecular mass, a fundamental concept in chemistry where the sum of the atomic masses of the atoms in a molecule is computed. Students are required to use the average atomic masses of individual elements to calculate the subtotal for each element, which then contributes to the total molecular mass of the compound. The process involves multiplying the quantity of each element present in the molecule by its respective average atomic mass. For example, if a molecule contains one carbon atom (C) with an atomic mass of 12.01 amu and three chlorine atoms (Cl) with an atomic mass of 35.45 amu each, the subtotals would be 12.01 amu for carbon and 106.35 amu for chlorine (35.45 amu multiplied by 3), leading to a molecular mass of 118.36 amu when summed. This approach is visually supported by diagrams that illustrate the structure of the mentioned molecules, such as a carbon backbone structure or simple diatomic molecules.
The instructional texts focus on data collection and analysis using average values, stratified sampling with random number generators, and adherence to statistical guidelines such as ensuring that each category in a study has an expected value of at least five. Students are tasked with conducting experiments, plotting graphs, and understanding the statistical requirements that underpin sound experimental practices. This includes recognizing the importance of averages in reducing variability for grouped data and applying this to scenarios such as changes in body composition or academic performance.