1.5L of gas is initially at 37 degrees * C. The volume of the gas is increased to 42L. What is the final temperature of the gas if the pressure remains constant?

8680K or 8407°C

Explanation:

Initial volume V1 = 1.5L

Initial temperature T1 = 37+273 = 310K

Final volume V2 = 42L

Final temperature T2=?

From Charles law:

V1/T1 = V2/T2

Therefore T2 = V1*T1/V1 = 42*310/1.5=8680K or 8407°C

The final temperature is 8680 K or 8407 °C

Explanation:

Step 1: Data given

Initial volume of the gas = 1.5 L

Initial temperature of the gas = 37.0 °C = 310 K

Final volume of the gas = 42 L

Step 2: Calculate final temperature

V1/T1 = V2/T2

⇒with V1 = the initial volume of the gas = 1.5 L

⇒with T1 = the initial temperature = 310 K

⇒with V2 = the final volume of the gas = 42 L

⇒with T2 = the final temperature of the gas = ?

1.5 L / 310 K = 42 L / T2

0.0048387 = 42L / T2

T2 = 42 / 0.0048387

T2 = 8680 K

The final temperature is 8680 K or 8407 °C