What is the effect of the following on the volume of 1 mol of an ideal gas? The temperature changes from 305 K to 32°C and the pressure changes from 2 atm to 101 kPa.

A. Volume increases by 200%

B. Volume decreases to 50% of its original value

C. Volume decreases by 100%

D. Volume increases by 100%

E. Volume does not change

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%.