A 5.00 L sample of gas at 1.00 atm and 20 degrees Celsius is compressed to 2.00 L at 2.00 atm. What is the temperature of the gas?

234.4 K

Explanation:

Using the combined gas law equation as follows;

P1V1/T1 = P2V2/T2

Where;

P1 = initial pressure (atm)

P2 = final pressure (atm)

V1 = initial volume (L)

V2 = final volume (L)

T1 = initial temperature (K)

T2 = final temperature (K)

According to the provided information,

P1 = 1.00atm

P2 = 2.00 atm

V1 = 5.00L

V2 = 2.00L

T1 = 20°C = 20 + 273 = 293K

T2 = ?

Using P1V1/T1 = P2V2/T2

1 × 5/293 = 2 × 2/T2

5/293 = 4/T2

Cross multiply

293 × 4 = 5 × T2

1172 = 5 T2

T2 = 1172 ÷ 5

T2 = 234.4 K

the answer is a and have a great day