For determining the correct significant figures (sig figs) for the density values in the right column, we need to consider the following rules of significant figures in multiplication and division:

1. Multiplication/Division Rule: The result should have the same number of significant figures as the number in the calculation with the fewest significant figures.

In this case, the formula for density is:

$\text{Density} = \frac{\text{Mass of Water}}{\text{Volume of Water}}$

Review of Significant Figures for Each Column:

• Mass of Water (g): The values are reported to 4 significant figures (e.g., 4.937g).
• Volume of Water (mL): The volume is fixed at 5.00 mL, which has 3 significant figures.

Since we are dividing the mass (4 sig figs) by the volume (3 sig figs), the result should be rounded to 3 significant figures (the fewest in the input values).

Correct Significant Figures for Density (g/mL):

• Trial 1: 0.9874 g/mL should be rounded to 0.987 g/mL.
• Trial 2: 0.7180 g/mL should be rounded to 0.718 g/mL.
• Trial 3: 0.7644 g/mL should be rounded to 0.764 g/mL.
• Trial 4: 0.7396 g/mL should be rounded to 0.740 g/mL.
• Trial 5: 0.7240 g/mL should be rounded to 0.724 g/mL.

Let me know if you'd like any further details on significant figures!

Here are 5 follow-up questions you might consider:

1. How are significant figures handled in addition or subtraction?
2. Why is the volume of water fixed at 3 significant figures?
3. How do significant figures affect precision in experimental data?
4. What is the difference between accuracy and precision in the context of this experiment?
5. How can you estimate uncertainty based on significant figures?

Tip: Always check the significant figures of your measuring instruments to ensure you're reporting values with the right precision.