A gas exerts a pressure of one atm at standard temperature
Answer (1)
A gas exerts a pressure of one atmosphere (1 atm) at standard temperature (0°C or 273.15 K) because of the constant and random motion of gas particles. These particles collide with the walls of the container, and the force of these collisions creates pressure.At standard temperature and pressure (STP) — defined as 0°C (273.15 K) and 1 atm — one mole of an ideal gas occupies 22.4 liters. This condition is used as a reference point in gas laws, like the Ideal Gas Law (PV = nRT)Where,P is pressure (1 atm)V is volume (22.4 L for 1 mole)n is number of moles (1 mol)R is the ideal gas constant (0.0821 L·atm/mol·K)T is temperature (273.15 K)This explains why a gas under standard temperature exerts exactly 1 atm of pressure — it's the result of molecular collisions at that specific temperature and amount.
