What happens to the pressure of a gas when the temperature is increased?
a
the kinetic energy decreases so the pressure decreases
b
the kinetic energy decreases so the pressure increases
c
the kinetic energy increases so the pressure increases
d
the kinetic energy increases so the pressure decreases
c
the kinetic energy increases so the pressure increases
The correct answer is c) The kinetic energy increases, so the pressure increases.
When the temperature of a gas increases, the average kinetic energy of its molecules increases. This means that the molecules move faster and collide with the walls of the container more frequently and with more force. As a result, the pressure of the gas increases.
When the temperature of a gas is increased, the kinetic energy of its particles increases. To understand how this affects the pressure of the gas, we can use the ideal gas law, which states that the pressure of a gas is directly proportional to its temperature.
The ideal gas law is given by the equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature.
From this equation, we can see that if we increase the temperature (T) while keeping the other variables constant, such as the volume (V) and the number of moles (n), the pressure (P) will also increase.
Therefore, the correct answer is:
c) The kinetic energy increases, so the pressure increases.