If the pressure of an ideal gas is doubled from 1.0 atm to 2.0 atm and its tempe
ID: 529689 • Letter: I
Question
If the pressure of an ideal gas is doubled from 1.0 atm to 2.0 atm and its temperature is halved from 80.0 degree C to 40.0 degree C, the volume of the gas A. will double its original value. B. will be half its original value. C. will increase by a factor of 0.56. D. will decrease by a factor of 0.56 Which of the following gases would have the greatest kinetic energy at 300 K? A. N_2 B. NH_3 C. Ar D. All of them would have the same kinetic energy. The volume of a gas must always decrease when A. temperature increases and pressure increases. B. temperature increases and pressure decreases. C. temperature decreases and pressure increases. D. temperature decreases and pressure decreases.Explanation / Answer
Ans 3. D. will decrease by a factor of 0.56
According to the ideal gas law ,
pV = nRT
p1 V1 / T1 = p2 V2/ T2
(p1 T2) / (T1 p2) = V2 / V1
putting the values mentioned in the question , convert the temperatures into kelvin
(1 x 313) / (353 x 2) = V2 / V1
V2 = 0.44 V1
V1 - V2 = V1 - 0.44V1 = 0.56
So V2 has decreased by factor of 0.56