The whole ‘breaking the surface tension’ is a myth. You would splat no matter how many bullets you had. Unless you have a grenade launcher capable of creating vast amounts of gas bubbles in water under you. With a large enough gun, the recoil might slow you enough to save you.

The salt water has a much lower cohesion than plain water so it’s attractive forces are less than plain water. The surface tension does increase when the salt is added to the water so that means that the penny drop experiment is mostly affected by the water’s cohesive forces.

Falling into water from about 245 ft. will be fatal for most people. The fatal results can vary from person to person and there are known cases of people dying from heights less than 200 ft.

Water has a high surface tension (72 dynes/cm). It can be lowered into the range of 32–35 dynes/cm with traditional water-soluble fatty surfactants. Oil has a surface tension of 30–35 dynes/cm, meaning that oil-soluble fatty surfactants do not provide the desired surface tension reduction for oils.

Surfactants are molecules, such as soaps and detergents, that reduce the surface tension of polar liquids like water. Capillary action is the phenomenon in which liquids rise up into a narrow tube called a capillary.

Hexane

Oil/brine interfacial tensions are usually somewhat higher than the corresponding oil/(pure) water values. Typical values for both range from 18 mN/m to 32 mN/m. Surface and interfacial tensions tend to decrease with temperature and increase with weathering.

Surface tension depends mainly upon the forces of attraction between the particles within the given liquid and also upon the gas, solid, or liquid in contact with it. In comparison, organic liquids, such as benzene and alcohols, have lower surface tensions, whereas mercury has a higher surface tension.

Surface tension is caused by attraction between liquid molecules. Different compounds have different levels of attraction. Water and Ethanol are held together by hydrogen bonds, the strongest of all intermolecular forces. Thus water and ethanol have strong surface tension.

As the fluid crosses the critical point, there is no clear transition between liquid and gas, and the meniscus (the layer separating the liquid and gas phases) disappears. So a supercritical fluid is pretty much a liquid with gas-like properties, like no surface tension. You can check for yourself!

Surface tension of a liquid is zero at critical point. The surface tension of a liquid decreases with increase of temperature and becomes zero at its critical temperature (where the surface of separation between liquid and its vapour dispapears).

Surface Tensions of Liquids Figure 2-5 demonstrates the surface tension of water from 0°C to its critical value of 374.2°C In general, the surface tension of a liquid in equilibrium with its own vapor decreases with temperature and becomes zero at the critical point.

It’s not a simple case of just getting rid of water’s surface tension. No surface tension/ energy would imply no intermolecular interactions and from there all non ideal models of the world fly out the window. There would be no phase transformations; everything would be an ideal gas, absent of molecular interactions.

The surface tension of liquids and the influence of surfactants on the surface tension depend on the temperature. Additionally, the dynamic of surfactant molecules increases due due higher thermal energy. In general, the surface tension decreases with increasing temperature.

Because of the relatively high attraction of water molecules to each other through a web of hydrogen bonds, water has a higher surface tension (72.8 millinewtons (mN) per meter at 20 °C) than most other liquids. Surface tension is an important factor in the phenomenon of capillarity.

According to the kinetic theory of gases, viscosity should be proportional to the square root of the absolute temperature, in practice, it increases more rapidly. With high temperatures, viscosity increases in gases and decreases in liquids, the drag force will do the same.

The viscosity of a liquid usually depends on its temperature. Viscosity generally decreases as the temperature increases. Viscosity generally increases as the temperature decreases. The viscosity of a liquid is related to the ease with which the molecules can move with respect to one another.

Viscosity is normally independent of pressure, but liquids under extreme pressure often experience an increase in viscosity. Since liquids are normally incompressible, an increase in pressure doesn’t really bring the molecules significantly closer together.

The shear viscosity of the liquids that are used as lubricants increases with increasing pressure and decreases with increasing temperature and, at sufficiently large stress (rate), decreases with increasing shear stress (shear rate). …

For the same pressure, the flow diminishes when the fluid viscosity increases. For a given flow, an increase of viscosity can present a reduction in the factor K of the measurer. When the compressibility has a considerable value, it is important to measure the pressure to allow the correction of the measured flow.