Question

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

Answer 1

Using the Combined Gas Law, the new pressure of the gas when the volume increases to 35 L and the temperature to 52 °C is approximately 2.6 atm, rounded to the nearest tenth.

Step-by-step explanation:

To calculate the new pressure of the gas after its volume and temperature change, we can use the Combined Gas Law which is formulated as (P1 × V1) / T1 = (P2 × V2) / T2, where P stands for pressure, V for volume, and T for temperature in Kelvin. The initial and final conditions are given for pressure (P1 and P2), volume (V1 and V2), and temperature (T1 and T2).

First, we need to convert the temperatures from Celsius to Kelvin: T1 = 12 °C = 285.15 K and T2 = 52 °C = 325.15 K. Now we can plug the values into the Combined Gas Law equation:

(3.6 atm × 24 L) / 285.15 K = (P2 × 35 L) / 325.15 K

By solving for P2, we get:

P2 = (3.6 atm × 24 L × 325.15 K) / (285.15 K × 35 L)

After calculating, we find that P2 ≈ 2.6 atm when rounded to the nearest tenth.