modern vacuum techniques make it possible to reach a pressure of 1.00 * 10 ^ -10 mm Hg in a laboratory system. what volume in mi

Result: 1.68 L of liquid nitrogen is generated during the gas liquefaction process.

Clarification:

This process involves transforming gaseous nitrogen into its liquid form.

The two states possess distinct densities, thus occupying varying volumes; however, the mass remains constant.

Step 1: Calculate the mass of nitrogen gas

Let’s determine the mass of nitrogen gas associated with 297 L.

The density formula is:

With a density of nitrogen gas at 4.566 g/L and a volume of 297 L, we can compute the mass of nitrogen gas as follows:

Using these values yields:

The mass of nitrogen gas calculates to be 1356 g.

Step 2: Derive the volume of liquid nitrogen from the mass obtained

The mass for liquid nitrogen remains the same.

With the density of liquid nitrogen at 809 g/L, we can substitute this into our formula to find the volume of liquid.

Therefore, the volume of liquid nitrogen is 1.68 L.

Answer:

In blood: Dispersed phase: blood cells; Dispersed medium: liquid plasma

In fruit jelly: Dispersed phase: fruit juice; Dispersed medium: pectin

Explanation:

The dispersed phase refers to the phase where colloidal particles are dispersed within another phase, known as the dispersion medium.

In blood, the tiny cells act as colloidal particles, forming the dispersed phase within the liquid medium identified as plasma.

Conversely, in fruit jelly, the fruit juice constitutes the dispersed phase while the solid pectin serves as the dispersed medium.

Answer:

                    Benzoyl Chloride

Explanation:

                     Friedel-Craft Acylation is a reaction used to incorporate electrophiles (especially carbonyl groups) into the double bonds of aromatic compounds.

This scenario involves synthesizing benzophenone using benzene and benzoyl chloride.

Mechanism:

Step 1: Initially, benzoyl chloride reacts with a Lewis acid to create an electrophile known as oxo(phenyl)methylium.

Step 2: The second stage involves benzene participating in an electrophilic substitution reaction, where the electrophile is added.

Step 3: Finally, the aromatic nature of benzene is restored by releasing a proton.