When the number of moles and absolute temperature both double, the pressure of the gas will be 4 times its original value. This result follows from the Ideal Gas Law. Hence, the correct answer is D: 4 times.
Effect of Doubling Moles and Temperature on Pressure
To determine how the pressure changes when the number of moles and the absolute temperature are both doubled, we can use the **Ideal Gas Law** equation: PV = nRT.
Here,
P is pressure
V is volume
n is the number of moles
R is the gas constant
T is absolute temperature
Initially, we have :P1V = n1RT1
After doubling the number of moles and the absolute temperature, the equation becomes:
P2V = (2n1)R(2T1)
Simplifying this, we get :P2V = 4n1RT1
To compare with the initial equation P1V = n1RT1, we see that P2 is 4 times P1. Therefore, the pressure will be 4 times its original value.
Thus, the correct answer is :D: 4 times
