Question

A gas with a pressure of 3.6atm and a volume of 24L is held at 12∘C. If the volume increases to 35L and the temperature increases to 52∘C, what will be the new pressure in atmospheres? Round to the nearest tenth of an atmosphere.

Answer 1

Using the combined gas law, the new pressure of the gas when the volume increases to 35L and the temperature increases to 52°C is calculated to be approximately 2.6 atm, after converting temperatures to Kelvin and solving for P2.

To find the new pressure, we can use the combined gas law equation. The new pressure is approximately 0.4 atm.

Step-by-step explanation:

To find the new pressure, we can use the combined gas law equation, which states that:

P1V1/T1 = P2V2/T2

P1 = 3.6 atm (initial pressure)

V1 = 24 L (initial volume)

T1 = 12°C + 273 = 285 K (initial temperature in Kelvin)

V2 = 35 L (final volume)

T2 = 52°C + 273 = 325 K (final temperature in Kelvin)

Let's plug these values into the equation:

(3.6 atm)(24 L)/(285 K) = (P2)(35 L)/(325 K)

Simplifying the equation:

3.6(24) = P2(35)(285/325)

86.4 = 220.5P2

Dividing both sides by 220.5:

P2 = 86.4/220.5

P2 = 0.392 atm

The new pressure is approximately 0.4 atm.