Two moles of an ideal gas at 3.0 atm and 10 $\degree$C are heated up to 150 $\degree$C.If the volume is held constant during this heating,what is the final pressure?
A)4.5 atm
B)1.8 atm
C)0.14 atm
D)1.0 atm

Question

Two moles of an ideal gas at 3.0 atm and 10 $\degree$C are heated up to 150  $\degree$C.If the volume is held constant during this heating,what is the final pressure?
A)4.5 atm
B)1.8 atm
C)0.14 atm
D)1.0 atm

Quizplus · Accepted Answer

According to Gay-Lussac's Law, the pressure of an ideal gas held at constant volume is directly proportional to its temperature. Therefore, when the temperature is increased from 10°C to 150°C, the pressure will also increase proportionally. Using the formula P1/T1 = P2/T2, where P1 and T1 are the initial pressure and temperature, and P2 and T2 are the final pressure and temperature, we can solve for P2:

P1/T1 = P2/T2
(3.0 atm)/(283 K) = P2/(423 K)
P2 = (3.0 atm)(423 K)/(283 K) = 4.5 atm

Therefore, the final pressure is 4.5 atm, which corresponds to choice (A).

Two Moles of an Ideal Gas at 3 °\degree° C Are Heated Up to 150

Two Moles of an Ideal Gas at 3 $\degree$ C Are Heated Up to 150