The gas would occupy approximately 10.235 liters at 31.0°C and 140 atm.
We can use Charles's Law to solve this problem.
Charles's Law states that the volume of a gas is directly proportional to its temperature at constant pressure.
In other words, as the temperature of a gas increases, its volume also increases, and vice versa.
Here is the formula for Charles's Law:
V₁ / T₁ = V₂ / T₂
where:
V₁ is the initial volume of the gas
T₁ is the initial temperature of the gas (in Kelvin)
V₂ is the final volume of the gas
T₂ is the final temperature of the gas (in Kelvin)
We are given the following information:
V₁ = 10 liters (assuming this is the initial volume)
T₁ = 24.0°C + 273.15 K = 297.15 K
T₂ = 31.0°C + 273.15 K = 304.15 K
P = 140 atm (we are told that the pressure is constant)
We can rearrange the formula to solve for V₂:
V₂ = V₁ * T₂ / T₁
Now we can plug in the values:
V₂ = 10 liters * 304.15 K / 297.15 K
V₂ ≈ 10.235 liters
Therefore, the gas would occupy approximately 10.235 liters at 31.0°C and 140 atm.