If 200 ml of gas held at a constant pressure has a starting temperature of 300 degrees K, and it expands to fill a 300 ml space, what would be the new temp? (I got 454.54)
Thanks!
Use PV=nRT
P,n,R are constant, so V is proportional to T.
T=300*300/200=?
To solve this problem, we can use the ideal gas law equation, which states that the product of pressure (P), volume (V), and temperature (T) for a gas is constant.
The equation is given as:
P1V1 / T1 = P2V2 / T2
Where:
P1 = initial pressure,
V1 = initial volume,
T1 = initial temperature,
P2 = final pressure,
V2 = final volume, and
T2 = final temperature.
In this case, we are given:
P1 = constant pressure (which is not mentioned),
V1 = 200 ml,
T1 = 300 K,
V2 = 300 ml,
T2 = ?
Since the pressure is constant, we can eliminate it from the equation, leaving us with:
V1 / T1 = V2 / T2
Now, we can plug in the given values:
200 ml / 300 K = 300 ml / T2
Next, we can cross-multiply the equation:
200 ml * T2 = 300 ml * 300 K
Simplifying,
200 T2 = 90000
Finally, solving for T2 by dividing both sides by 200:
T2 = 90000 / 200 = 450 K
Therefore, the new temperature (T2) would be 450 Kelvin (K), not 454.54 K.