### Standard Temperature and Pressure(STP)

In chemistry, STP stands for “Standard Temperature and Pressure.” It is a set of standard conditions used for comparing and measuring the properties of gases. STP provides a consistent reference point for gas-related calculations. The standard conditions for STP are:

**Temperature:**0 degrees Celsius (0°C) or 273.15 Kelvin (K).**Pressure:**1 atmosphere (atm) or 101.3 kilopascals (kPa).

In chemistry, a modification to the definition of standard temperature and pressure (STP) was introduced by IUPAC in 1982:

Before 1982, STP was delineated as a temperature of 273.15 K (equivalent to 0 °C or 32 °F) and an absolute pressure precisely equal to 1 atmosphere (101.325 kilopascals).

Since 1982, the revised definition of STP designates a temperature of 273.15 K (0 °C or 32 °F) and an absolute pressure that precisely amounts to 105 pascals (100 kilopascals or 1 bar).

Therefore, the standard temperature is 0 degrees Celsius which is equal to 32 degrees Fahrenheit or 273.15 Kelvin. Essentially, this aligns with the freezing point of pure water at sea level when subjected to air at standard pressure. However, it’s worth noting that the National Institute of Standards and Technology offers an alternative definition for STP, indicating an absolute pressure of 1 atmosphere (101.325 kilopascals, 14.696 pounds per square inch) and a temperature of 20 degrees Celsius (293.15 Kelvin, 68 degrees Fahrenheit).

### Importance of Standard Temperature Pressure

First and foremost, STP offers a consistent and universally accepted benchmark for the measurement and comparison of gas properties. It defines standard conditions at which gases are studied, simplifying calculations and ensuring that scientific data from different sources can be directly compared. This standardization is particularly valuable in chemistry and physics, where gas behaviour is a fundamental aspect of research and experimentation.

Furthermore, STP is integral to the ideal gas law (PV = nRT), which relates the pressure (P), volume (V), number of moles (n), and temperature (T) of a gas. Under STP conditions, the values of P, V, n, and T are well-defined, making calculations straightforward and consistent.

In addition to its role in scientific research, STP has practical applications in various industries. It is essential in the calibration of instruments used to measure gas properties and plays a key role in the design and operation of equipment in fields such as chemical engineering, where precise knowledge of gas properties is crucial.

### Volume of Gases at STP

Gas volume depends on pressure and temperature. Under STP conditions, 1 mole of gas occupies 22.4 litres, termed the molar volume. The ideal gas law, PV = nRT (n = moles, R = gas constant), can be used to calculate this volume at STP as 22.4 L.

### Difference between STP and NTP?

**STP (Standard Temperature and Pressure):** STP, or Standard Temperature and Pressure, serves as a well-defined reference point in the fields of chemistry and physics. It specifies a temperature of 0 degrees Celsius (273.15 Kelvin) and a pressure of 1 atmosphere, equivalent to 101.3 kilopascals. STP is extensively used to establish uniform conditions for the measurement and comparison of gas properties, particularly in the ideal gas law (PV = nRT). Under STP, 1 mole of any ideal gas consistently occupies a volume of approximately 22.4 litres. This precise definition and widespread adoption make STP an essential concept for scientific research and calculations.

**NTP (Normal Temperature and Pressure):** NTP, or Normal Temperature and Pressure, is another set of standardized conditions, although it is less rigorously defined and not as widely accepted as STP. NTP specifies a temperature of 20 degrees Celsius (293.15 Kelvin), but its pressure is not precisely standardized and may vary depending on the source. While NTP is cited as being at 1 atmosphere (101.3 kilopascals) in some contexts, this pressure specification can be inconsistent.

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