An experiment requires 13.0 g of cyclohexane, which has a density of 0.7781 g/mL at 25° C. What volume of cyclohexane should be used?

Question

Express your answer using three significant figures.

Answer 1

To find the volume of cyclohexane needed, we can use the formula for density:

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

Rearranging this formula to solve for volume gives:

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

We are given:

• Mass of cyclohexane = 13.0 g
• Density of cyclohexane = 0.7781 g/mL

Now, we can calculate the volume:

$$\text{Volume}=\frac{13.0,\text{g}}{0.7781,\text{g/mL}}\approx 16.7,\text{mL}$$

Now, rounding to three significant figures, the volume of cyclohexane that should be used is:

$$\boxed{{\displaystyle 16.7,\text{mL}}}$$