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Chapter 1: Problem 27

The density of \(\mathrm{CCl}_{4}\) (carbon tetrachloride) is 1.58 \(\mathrm{g} / \mathrm{mL} .\) What is the mass of 95.7 \(\mathrm{mL}\) of \(\mathrm{CCl}_{4} ?\)

Short Answer

Expert verified
The mass of 95.7 mL of \(\mathrm{CCl}_{4}\) is approximately 151.206 g.

Step by step solution

01

Identify the given values

The given values are the density of the \(\mathrm{CCl}_{4}\) which is 1.58 \(\mathrm{g} / \mathrm{mL}\), and the volume of the \(\mathrm{CCl}_{4}\) which is 95.7 \(\mathrm{mL}\).
02

Apply the mass formula

The mass formula is: \( \text{Mass} = \text{Density} \times \text{Volume} \) Substitute the given density and volume values into the formula: \( \text{Mass} = 1.58 \, \mathrm{g/mL} \times 95.7 \, \mathrm{mL} \)
03

Compute the mass

To get the mass in grams, perform the multiplication: \( \text{Mass} = 1.58 \, \mathrm{g/mL} \times 95.7 \, \mathrm{mL} = 151.206 \, \mathrm{g} \)
04

Round-off the final answer

Round off the final answer to three decimal places. This gives us 151.206 g.

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