The pressure exerted on a surface depends on:

Temperature, pressure, volume and the amount of a gas influence its pressure.

Pressure is affected by volume, temperature, and the number of moles present. P is pressure; V is volume; n is number of moles; R is a constant; T is temperature (in Kelvin!) Area and force are the two factors on which pressure depend.

• The thrust.
• The area on which the thrust is applied.
• Larger the area on which a thrust acts, less is the pressure exerted by it.
• Larger the thrust acting on an area more is the pressure exerted on it.

Boyle’s Law explains the relationship between volume and pressure. According to Boyle’s Law, the volume of a fixed amount of gas decreases as its pressure increases. If the volume increases, its pressure decreases.

For a fixed mass of an ideal gas kept at a fixed temperature, pressure and volume are inversely proportional. Or Boyle’s law is a gas law, stating that the pressure and volume of a gas have an inverse relationship. If volume increases, then pressure decreases and vice versa, when the temperature is held constant.

The volume of a gas is directly proportional to its absolute temperature. More specifically, for a fixed mass of gas at a constant pressure, the volume (V) is directly proportional to the absolute temperature (T). This is Charles’ Law. The volume is directly to the absolute temperature.

Gas laws are important because they can be used to determine the parameters of a mass of gas using theoretical means.

Gas laws, laws that relate the pressure, volume, and temperature of a gas. These two laws can be combined to form the ideal gas law, a single generalization of the behaviour of gases known as an equation of state, PV = nRT, where n is the number of gram-moles of a gas and R is called the universal gas constant.

What are some examples of the gas laws in action in everyday life? Charles’s Law: Doubling the temperature of a gas doubles its volume, as long as the pressure of the gas and the amount of gas isn’t changed. A football inflated inside and then taken outdoors on a winter day shrinks slightly.

Solids and liquids have intermolecular attraction between them, which provide their characteristic shape and properties, therefore the ideal gas laws do not apply solids and liquids.

The ideal gas law can be used in stoichiometry problems in which chemical reactions involve gases. Standard temperature and pressure (STP) are a useful set of benchmark conditions to compare other properties of gases. At STP, gases have a volume of 22.4 L per mole.

Explanation: Cars have tires. These tires (in British English tyres) have to have air pressure. Inflatable beds can be given as another example as well as baloons.

Boyle’s law can be used to describe the effects of altitude on gases in closed cavities within the body, and to calculate the total intra-thoracic gas volume by body plethysmography. Using Boyle’s law, P1V1 = P2V2, we can calculate the change in volume at different altitudes.

Here is a list of 10 gases and their uses:

• Oxygen (O2): medical use, welding.
• Nitrogen (N2): fire suppression, provides an inert atmosphere.
• Helium (He): balloons, medical equipment.
• Argon (Ar): welding, provides an inert atmosphere for materials.
• Carbon dioxide (CO2): carbonated soft drinks.
• Acetylene (C2H2): welding.

Water, ethane, butane, propane, pentanes, hydrogen sulphide, carbon dioxide, water vapor, and occasionally helium and nitrogen may be present in a natural gas well.

Natural Gas in Our Daily Lives

• Electricity.
• Home Heating.
• Transportation.
• Manufacturing.
• Products.

The commercial sector uses natural gas to heat buildings and water, to operate refrigeration and cooling equipment, to cook, to dry clothes, and to provide outdoor lighting. Some consumers in the commercial sector also use natural gas as a fuel in combined heat and power systems.

natural gas