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Heating a closed container increases the pressure inside it primarily due to the principles of gas behavior as described by the ideal gas law. When the temperature of a gas increases, the kinetic energy of the gas molecules also rises. As the molecules move faster, they collide with the walls of the container more frequently and with greater force. This increase in the frequency and intensity of collisions results in an increase in pressure within the closed system.

The relationship can be summarized with the formula from the ideal gas law, which states that the pressure of a gas is directly proportional to its temperature when volume is held constant. Therefore, if the temperature increases, the pressure must also increase, which directly supports why heating a closed container leads to an increase in pressure.