1) Convert the density of water, \( 1.00 \mathrm{~g} / \mathrm{mL} \) to \( \mathrm{lb} / \mathrm{ft}^{3} \)

To convert \( 1.00 \mathrm{~g} / \mathrm{mL} \) to \( \mathrm{lb} / \mathrm{ft}^{3} \), you start with the conversion factors: 1 g = 0.00220462 lb and 1 mL = \( 3.53147 \times 10^{-5} \) ft³. Thus, the conversion is: \[ 1.00 \mathrm{~g/mL} \times \frac{0.00220462 \mathrm{~lb}}{1 \mathrm{~g}} \times \frac{1000 \mathrm{~mL}}{1 \mathrm{~L}} \times \frac{1 \mathrm{~L}}{0.0353147 \mathrm{~ft}^3} \approx 62.43 \, \mathrm{lb/ft^3}. \] So, water's density is about \( 62.43 \, \mathrm{lb/ft^3} \)! Now, how cool is that? Water, which feels light when you hold it, is stacked with enough oomph to weigh in at over 62.43 pounds for every cubic foot! That’s just a fun reminder of how dense some things can be, right? While densities of substances vary, knowing straightforward conversions can enhance your understanding of material properties. Just imagine using this info while crafting a science project, adding a touch of 'big picture' flair to your experiments!