I have 130 liters of gas in a piston at a temperature of 250 degree Celsius. If i cool the gas until the volume decreases to 85 liters what will temperature of the gas be?

V1/T1=V2/T2

1.130L = 85L 2. 250*85/130=L 3. 163.5 (1d.p) C and 436.6 K
/250 /T2

you check by 130 /250 to get 0.52. and with the other side 85/163.5 to also get 0.52. since they are both proportionate equations they should both equal one another. The answ also makes sense since if volume decreasing should also make temp decrease :D

what about the pressure?

PV = kT
I guess if you somehow keep the pressure constant, then V/T is constant, so you want T such that
85/T = 130/(250+273.15)
T = 342°K = 69°C

Well, well, well, looks like we've got ourselves a cooling conundrum! Let's see... If the volume decreases from 130 liters to 85 liters, that's quite the squeeze! Now, I don't want to be accused of being "cold-hearted," but it seems like we need to apply some good old-fashioned gas laws here.

We can use Charles's Law to crack this puzzle. Charles's Law states that for a fixed amount of gas at a constant pressure, the volume of the gas is directly proportional to its temperature in Kelvin. So, let's convert that sneaky Celsius temperature to Kelvin first!

To convert Celsius to Kelvin, simply add 273.15 to the temperature. So, 250 degrees Celsius would be (250 + 273.15) = 523.15 Kelvin. Now that we've got the Kelvin temperature, we can set up the equation:

Initial volume / Initial temperature = Final volume / Final temperature

Plugging in the values we have:

130 L / 523.15 K = 85 L / Final temperature

Now, all we need to do is isolate that "Final temperature" so we can give it a warm welcome. By rearranging the equation, we have:

Final temperature = (85 L x 523.15 K) / 130 L

And after some quick calculations, we find that the final temperature will be approximately 341.96 Kelvin.

So, to answer your question, if you cool the gas until the volume decreases to 85 liters, the temperature of the gas will be around 341.96 Kelvin. Just remember to keep things cool and not let your excitement reach boiling point!

To find the final temperature of the gas after cooling, we can use the combined gas law equation, which states that the initial pressure multiplied by the initial volume divided by the initial temperature is equal to the final pressure multiplied by the final volume divided by the final temperature.

The equation can be written as:
(P1 * V1) / T1 = (P2 * V2) / T2

Let's assign some variables to the given values:
P1 = initial pressure of the gas (unknown)
V1 = initial volume of the gas (130 liters)
T1 = initial temperature of the gas (250 degrees Celsius)
P2 = final pressure of the gas (unknown)
V2 = final volume of the gas (85 liters)
T2 = final temperature of the gas (unknown)

Since the pressure remains constant in this scenario, we can simplify the equation:

(V1 / T1) = (V2 / T2)

Now we can substitute the known values into the equation and solve for T2:

(130 / 250) = (85 / T2)

Cross-multiplying, we get:

130 * T2 = 85 * 250

130 * T2 = 21250

Dividing both sides by 130:

T2 = 21250 / 130

T2 ≈ 163.46

Therefore, after cooling the gas, the approximate final temperature will be about 163.46 degrees Celsius.

To find the temperature of the gas after cooling, we can use the ideal gas law equation. The ideal gas law states that the product of pressure (P), volume (V), and temperature (T) for a given amount of gas is always constant.

The equation for the ideal gas law is:
PV = nRT

Where:
P = pressure of the gas
V = volume of the gas
n = number of moles of gas
R = ideal gas constant
T = temperature of the gas

In this case, we are given the initial volume (V1 = 130 liters), the initial temperature (T1 = 250 degrees Celsius), and the final volume (V2 = 85 liters). We need to find the final temperature (T2).

First, let's convert the initial temperature from Celsius to Kelvin since temperature should be in Kelvin for the ideal gas law equation.

To convert from Celsius to Kelvin, we use the formula:
T(K) = T(°C) + 273.15

So, the initial temperature in Kelvin (T1) is:
T1 = 250 + 273.15
T1 = 523.15 K

Next, rearrange the ideal gas law equation to solve for T2:
T2 = (P2 * V2) / (n * R)

Since the pressure (P) and the number of moles of gas (n) are not given, we can assume that they remain constant. Therefore, we can cancel them out in the equation. This leaves us with:
T2 = (V2 * T1) / V1

Plugging in the values we have:
T2 = (85 * 523.15) / 130
T2 ≈ 341.646 K

Finally, let's convert the temperature from Kelvin back to degrees Celsius:
T(°C) = T(K) - 273.15
T2 ≈ 341.646 - 273.15
T2 ≈ 68.5 °C

So, the temperature of the gas after cooling to 85 liters will be approximately 68.5 degrees Celsius.