A 1.78 l container of oxygen gas at 28.5°C is deceited to 46.1°C assuming what the volume of the container can vary what is the new volume of gas

Answer 1

To solve this problem, we can use the combined gas law equation:

(P1 * V1) / T1 = (P2 * V2) / T2

Where:
P1 = initial pressure (assuming constant)
V1 = initial volume
T1 = initial temperature
P2 = final pressure (assuming constant)
V2 = final volume (unknown)
T2 = final temperature

First, we need to convert the temperatures to Kelvin:
Initial temperature (28.5°C) = 28.5 + 273.15 = 301.65 K
Final temperature (46.1°C) = 46.1 + 273.15 = 319.25 K

Now we can plug in the values we know:
(1.78 * V1) / 301.65 = (1.78 * V2) / 319.25

Now, we can solve for V2:
V2 = (V1 * T2 * 301.65) / (T1 * 319.25)
V2 = (1.78 * 319.25 * 301.65) / (1.78 * 301.65)
V2 = 319.25

Therefore, the new volume of the oxygen gas in the container at 46.1°C is 1.78 liters.