Gay lussac law graph

Learn how pressure and temperature are proportional in a confined gas system at constant volume and mass. See the graphical representation of the law and solve problems using the formula. Learn about the law of Gay-Lussac, which relates the pressure and temperature of a gas at constant volume and mass.

See the equation, graph, and applications of this ideal gas law in chemistry and everyday life. What is Gay-Lussac’s Law? Gay-Lussac’s law is a gas law which states that the pressure exerted by a gas (of a given mass and kept at a constant volume) varies directly with the absolute temperature of the gas. Gay-Lussac's Law states that the pressure of a given mass of gas varies directly with the absolute temperature of the gas, when the volume is kept constant.

Gay-Lussac's Law is very similar to Charles's Law, with the only difference being the type of container. Gay-Lussac's is defined as the pressure of a given mass of gas varies directly with the absolute temperature of the gas when the volume is kept constant. Mathematically, it can be written as P/T=k. It is a special case of the ideal gas law. Reset password New user? Sign up. Existing user? Log in.

Already have an account? Log in here. An ideal gas is a theoretical gas composed of many randomly moving point particles that do not interact except when they collide elastically. The ideal gas law is the equation of state of an ideal gas. This implies that the gas molecules have negligible volume compared to the volume of container in which they are placed. They therefore possess kinetic energy, which is energy of motion.

Thus they can move independent of each other. They only interact with each other through elastic collisions. The last postulate of the kinetic molecular theory states that the average kinetic energy of a gas particle depends only on the temperature of the gas. Thus, the average kinetic energy of the gas particles increases as the gas becomes warmer. Because the mass of these particles is constant, their kinetic energy can only increase if the average velocity of the particles increases.

The faster these particles are moving when they hit the wall, the greater the force they exert on the wall. Since the force per collision becomes larger as the temperature increases, the pressure of the gas must increase as well. In this, volume and number of moles of gas is taken constant. If temperature is represented in kelvin then the graph between pressure and temperature will be a straight line passing through origin.

If temperature is represented in celsius then the graph between pressure and temperature will be a straight line but will not pass through origin. On extrapolating, the graph will hit Gases can be compressed because most of the volume of a gas is empty space.

gay lussac's law real life example

If we compress a gas without changing its temperature, the average kinetic energy of the gas particles stays the same. There is no change in the speed with which the particles move, but the container is smaller. Thus, the particles travel from one end of the container to the other in a shorter period of time. This means that they hit the walls more often.

Any increase in the frequency of collisions with the walls must lead to an increase in the pressure of the gas. Thus, the pressure of a gas becomes larger as the volume of the gas becomes smaller. If temperature and amount of gas is fixed then pressure is inversely proportional to volume occupied by the gas.

If temperature and number of moles of gas are fixed then the graph between pressure P and volume V will be a rectangular hyperbola. On increasing volume of gas pressure decrease and vice-versa. Such a process is also called as Isothermal Process. The average kinetic energy of the particles in a gas is proportional to the temperature of the gas.