Answer:
The volume increases by 100%.
Explanation:
Step 1: Data given
Number of moles ideal gas = 1 mol
Initial temperature = 305 K
Final temperature = 32°C + 273.15 = 305.15 K
Initial pressure = 2 atm
final pressure = 101 kPa = 0.996792 atm
R = gasconstant = doesn't change
V1 = initial volume
V2= the final volume
Step 2: Calculate volume of original gas
P*V = n*R*T
(P*V)/ T = constante
(P1 * V1) / T1 = (P2 * V2)/ T2
In this situation we have:
(2atm * V1)/ 305 = (0.996792 *V2) / 305.15
0.006557*V1 = 0.003266*V2
V2 = 2*V1
We see that the final volume is twice the initial volume. So the volume gets doubled. The volume increases by 100%.
Volume increases by 100% under the conditions mentioned in the question.
This is the gas in which all collisions between atoms or molecules are perfectly elastic and in which there are no intermolecular attractive forces
PV = nRT
(P1 V1) / T1 = (P2 V2)/ T2
(2atm × V1)/ 305 = (0.996792×V2) / 305.15
0.006557×V1 = 0.003266×V2
V2 = 2V1
Therefore we can conclude that the volume doubled and increased by 100%.
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