Assume tat you have a sample of a gas in a cylinder with a movable piston at constant pressure. Determine the volume of the gas if the absolute temperature is decreased by twenty-five percent.
THE VOLUME WOULDN'T HAVE ANY EFFECT ON THE TEMPERATURE. FOR A GAS IN A CLOSED CONTAINER, WITH THE PRESSURE CONSTANT THE TEMPERATURE DOESN'T CHANGE THE VOLUME. WHEN TEMPERATURE INCREASES, PRESSURE INCREASES. THEY ARE DIRECTLY PROPORTIONAL.
(V1/T1) = (V2/T2)
V1 = V
T1 = make up some number such as 300 Kelvin.
Solve for V2 when T2 = 25% less. So if T1 = 300K, then 25% less than that is 225 and solve for V1. I get something like.0.75V1 which means that V2 = just 3/4 of the old volume of V1.
To determine the volume of the gas when the absolute temperature is decreased by twenty-five percent, we can use Charles's Law, which states that the volume of a gas is directly proportional to its temperature at constant pressure.
Charles's Law can be expressed as follows:
V1 / T1 = V2 / T2
Where V1 and T1 are the initial volume and temperature of the gas, and V2 and T2 are the final volume and temperature of the gas.
In this case, we are given that the pressure is constant, so the equation simplifies to:
V1 / T1 = V2 / T2
Now let's plug in the values we have:
Let's assume the initial volume V1 and temperature T1. The final volume V2 can be calculated by decreasing the temperature T1 by twenty-five percent (which means the temperature becomes 75% of T1).
So, the equation becomes:
V1 / T1 = V2 / (0.75 * T1)
To solve for V2, we can rearrange the equation:
V2 = (V1 * 0.75 * T1) / T1
Simplifying further:
V2 = 0.75 * V1
This means the final volume (V2) is equal to 0.75 times the initial volume (V1).
Therefore, to determine the volume of the gas when the absolute temperature is decreased by twenty-five percent, multiply the initial volume of the gas by 0.75.