A quantity of gas has a volume of 0.20 cubic meter and an absolute temperature of 333 degrees kelvin. When the temperature of the gas is raised to 533 degrees kelvin, what is the new volume of the gas? (Assume that there's no change in pressure.)
assuming the gas is ideal, we can use the Charles' Law:
V1 / T1 = V2 / T2
where
V1 = initial volume of gas
T1 = initial temp of gas
V2 = final volume of gas
T2 = final temp of gas
substituting the values to the equation,
0.20 / 333 = V2 / 533
V2 = 0.20*533/333
V2 = 0.32 cubic meter
hope this helps~ :)
To solve this problem, we can use the combined gas law, which states that the product of the initial volume and initial temperature divided by the initial absolute temperature is equal to the product of the final volume and final temperature divided by the final absolute temperature.
Let's denote the initial volume as V1 (0.20 cubic meter), the initial temperature as T1 (333 degrees Kelvin), and the final temperature as T2 (533 degrees Kelvin).
Using the combined gas law, we can set up the equation:
(V1 * T1) / T1 = (V2 * T2) / T2
Simplifying the equation, we get:
V1 = V2 * (T1 / T2)
Now we can plug in the values:
0.20 = V2 * (333 / 533)
To find the value of V2, we isolate it:
V2 = 0.20 * (533 / 333)
Calculating this expression, we find:
V2 ≈ 0.32 cubic meters
Therefore, the new volume of the gas is approximately 0.32 cubic meters.
To solve this problem, we can use the combined gas law, which states:
(P1 × V1) / T1 = (P2 × V2) / T2
In this case, we can assume that the pressure (P) remains constant, so we can rearrange the equation to solve for the new volume (V2):
V2 = (T2 / T1) × V1
Given:
V1 = 0.20 cubic meters
T1 = 333 Kelvin
T2 = 533 Kelvin
Substituting the values into the equation, we have:
V2 = (533 / 333) × 0.20
Now, we can calculate the new volume of the gas:
V2 = 0.602 cubic meters
Therefore, the new volume of the gas when the temperature is raised to 533 degrees Kelvin (assuming no change in pressure) is approximately 0.602 cubic meters.