Question

The compound 1 -iodododecane is a nonvolatile liquid with a density of \(1.20 \mathrm{~g} / \mathrm{mL}\). The density of mercury is \(13.6 \mathrm{~g} / \mathrm{mL}\). What do you predict for the height of a barometer column based on 1 -iodododecane, when the atmospheric pressure is 749 torr?

Short answer

The height of a barometer column based on 1-iodododecane when the atmospheric pressure is 749 torr can be predicted to be approximately 67.0 millimeters.

Step-by-step solution

Convert the atmospheric pressure to pascals

Since we are given the atmospheric pressure in torr, we need to convert it to pascals (Pa) to keep our units consistent. We know that 1 torr = 133.322 Pa. So we can convert 749 torr to pascals as follows: \(pressure_{atmosphere\_Pa} = pressure_{atmosphere\_torr} \times 133.322\) \(pressure_{atmosphere\_Pa} = 749 \times 133.322 = 99884.778\,Pa\)

Calculate the height of the barometer column

Now, we can use the formula mentioned in the analysis to calculate the height of the 1-iodododecane column. \(height = \frac{density_{substance} \times atmospheric\_pressure}{density_{mercury} \times pressure_{substance}}\) \(height = \frac{1.20 \, g/mL \times 99884.778\, Pa}{13.6 \, g/mL \times 99884.778\, Pa}\) Since the pressure of 1-iodododecane is equal to the atmospheric pressure, we can cancel out the pressure values in the equation: \(height = \frac{1.20 \, g/mL}{13.6 \, g/mL}\)

Solve for the height of the barometer column

Now, we simply solve for the height of the 1-iodododecane column: \(height = \frac{1.20}{13.6}\) \(height = 0.0882\) Since the result is in a dimensionless format, we need to multiply it by the height of the mercury column at standard atmospheric pressure (760 mmHg) to get the height of the 1-iodododecane column in millimeters: \(height_{iodododecane} = height \times 760\, mmHg\) \(height_{iodododecane} = 0.0882 \times 760\) \(height_{iodododecane} = 67.032\,mm\) We can approximate the height of the 1-iodododecane column to be approximately 67.0 millimeters when the atmospheric pressure is 749 torr.

Key concepts

Atmospheric Pressure Conversion

Atmospheric pressure is often measured in different units around the world. Two common ones are torr and pascals (Pa). Converting one unit to another ensures accuracy in calculations. To change atmospheric pressure from torr to pascals, we use the conversion factor where 1 torr equals 133.322 pascals.
A practical example is provided in the exercise. Here, 749 torr is converted using the formula:

• Multiply 749 by 133.322.
• Resulting in 99884.778 pascals.

This conversion is crucial because working with consistent units simplifies following calculations and ensures precise results.

Density Comparison

Density plays a key role in understanding the behavior of substances in varying pressures. It is the mass per unit volume, often expressed in grams per milliliter (g/mL).
In the exercise, the densities of two different liquids are compared:

• 1-Iodododecane has a density of 1.20 g/mL.
• Mercury has a higher density of 13.6 g/mL.

This comparison is pivotal for calculating the height of a barometer column. Liquids with lower density will have taller columns for the same pressure compared to those with higher density. Understanding these differences allows accurate predictions about liquid behavior under specific atmospheric conditions.

Pascals and Torr

Pascals (Pa) and torr are units of pressure, and understanding their relationship is essential for scientific calculations. Pascals are the SI unit used globally for scientific work, whereas torr often appear in meteorology and some other fields.
To compare them, remember:

• 1 torr = 133.322 pascals.

When dealing with barometer problems, as in the exercise, it's crucial to convert torr to pascals. This allows you to use formulas that are typically set in pascals, ensuring consistency and accuracy. Using consistent pressure units simplifies calculations and minimizes errors.

Nonvolatile Liquids

Nonvolatile liquids, such as the 1-iodododecane mentioned in the exercise, do not easily vaporize at room temperature. This characteristic makes them ideal for certain scientific applications, including barometry.
Key points about nonvolatile liquids include:

• They maintain their volume under varying atmospheric conditions.
• They provide a stable medium for accurate pressure measurements.

In the context of the exercise, using a nonvolatile liquid ensures that the pressure and density remain constant. This is crucial for predicting the height of the barometer column accurately, as fluctuations due to vaporization can skew results.