Calculate temperature when 0.50L sample or gas at 1.0 atm and 25degrees C is compressed to 0.05L of gas at 5.0 atm.

v1=0.50L. use the combined gas law = (P1)(V1)/(T1)=P2(V2)/(T2)

p1=1.0atm
t1=25C+273=298K. ANSWER IS =149K
v2=0.05L
p2=5.0
t2=???

Use the Combined Gas Law:

P1V1 / T1 = P2V2 / T2
P1 = 1.0 atm, V1 = 0.50L, T1 = 25+273=298K
P2 = ?____, V2 = ?____ (both given)
Solve for T2 to get the temperature in degrees Kelvin

1490

149.0

Well, if you're compressing a gas like that, it sounds like you're really squeezing the poor thing! I hope you're not trying to make it feel claustrophobic.

But let's get down to the numbers. We can use the ideal gas law to solve this. The equation is P1V1/T1 = P2V2/T2, where P1, V1, and T1 are the initial pressure, volume, and temperature, and P2, V2, and T2 are the final pressure, volume, and temperature.

Plugging in the values we know, we get:

(1.0 atm)(0.50 L)/(25°C) = (5.0 atm)(0.05 L)/(T2)

Now we just need to solve for T2.

Cross-multiplying, we have:

(1.0 atm)(0.50 L)(T2) = (5.0 atm)(0.05 L)(25°C)

Dividing both sides by (1.0 atm)(0.50 L), we get:

T2 = (5.0 atm)(0.05 L)(25°C)/ (1.0 atm)(0.50 L)

Calculating this out, we find that T2 is equal to 250°C.

So after being compressed, our gas is really feeling the heat at 250°C. It's like a sauna in there!

To calculate the temperature when a gas sample is compressed, we can use the ideal gas law equation:

PV = nRT

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

In this case, we are given:

Initial conditions:
P1 = 1.0 atm
V1 = 0.50 L
T1 = 25 degrees C

Final conditions:
P2 = 5.0 atm
V2 = 0.05 L

To solve for the temperature, we need to find the number of moles of gas. We can use the ideal gas law equation again to solve for n:

n = (P1 * V1) / (R * T1)

Next, we can use the number of moles to calculate the final temperature:

T2 = (P2 * V2) / (n * R)

First, let's convert the initial temperature from Celsius to Kelvin:

T1 = 25 + 273.15 = 298.15 K

The ideal gas constant (R) is 0.0821 L·atm/(mol·K).

Now, let's calculate the number of moles of gas:

n = (1.0 atm * 0.5 L) / (0.0821 L·atm/(mol·K) * 298.15 K) = 0.02013 mol

Finally, we can calculate the final temperature:

T2 = (5.0 atm * 0.05 L) / (0.02013 mol * 0.0821 L·atm/(mol·K)) = 616.57 K

Therefore, the temperature when the gas sample is compressed to 0.05L at 5.0 atm is approximately 616.57 Kelvin.