assume the pressure is kept constant if the volume of a gas quadruples, how does the absolute temperature change?
note that volume is directly proportional to the temperature at a constant pressure, or:
V = kT or V/T = k *Ideal Gas*
therefore, if V quadruples, absolute Temp must quadruple also,,
so there,, :)
To determine how the absolute temperature changes when the volume of a gas quadruples, we need to use the ideal gas law equation.
The ideal gas law is given by the formula:
PV = nRT
Where:
P is the pressure of the gas
V is the volume of the gas
n is the number of moles of the gas
R is the ideal gas constant
T is the absolute temperature of the gas
Since the pressure is constant, we can rewrite the ideal gas law equation as:
V/T = constant
Now let's consider what happens when the volume quadruples (increases by a factor of 4). We can denote the initial volume as V1 and the final volume as V2, where V2 = 4V1.
Applying the constant relationship (V/T = constant), we can write:
V1/T1 = V2/T2
Substituting V2 = 4V1:
V1/T1 = 4V1/T2
Simplifying the equation:
T2 = 4T1
Therefore, when the volume of a gas quadruples (increases by a factor of 4) while keeping the pressure constant, the absolute temperature also quadruples (increases by a factor of 4).