Ideal Gas Law: Understanding the Relationship Between Pressure and Temperature
What is the ideal gas law?
The relationship between pressure and temperature is described by the Ideal Gas Law, which states:
PV = nRT
where P is pressure, V is volume, n is the number of moles of gas, R is the universal gas constant, and T is temperature.
From this equation, pressure and temperature are directly proportional only if the volume and the number of moles of gas are constant.
Ideal Gas Law Calculation:
Given:
Volume (V) = 6.23 L
The number of moles(n) = 0.25 mol
Universal gas constant (R) = 0.082
Temperature (T) = 35°C = 273+35=308 K
Substitute the values in the above equation:
P = 0.250 × 0.082 × 308.15 × 6.23
P = 1.015 atm
P = 101.325 kPa
Thus, The absolute pressure of the air in the balloon is 101.325 kilopascals.
The Ideal Gas Law is a fundamental principle in chemistry that describes the behavior of ideal gases. It helps us understand the relationship between pressure, volume, temperature, and the number of moles of a gas in a system.
When applying the Ideal Gas Law to a specific scenario, such as a balloon filled with air, we can calculate the absolute pressure of the gas inside the container by knowing the volume, number of moles, and temperature of the gas.
In this case, the calculation showed that the absolute pressure of the air in the balloon is 101.325 kilopascals. This value represents the force exerted by the gas molecules on the surface of the balloon per unit area.
Understanding the Ideal Gas Law is crucial in various fields, including chemistry, physics, and engineering. It helps scientists and researchers predict the behavior of gases under different conditions and enables them to make informed decisions based on scientific principles.