A TANK OF COMPRESSED CO2 HAS A TEMPERATURE OF 43.5C AND A VOLUME OF 42.5L THE CO2 IS COMPLETELY TRANSFERRED INTO A SMALLER TANK THAT HAS A VOLUME OF 25.0L WAHT IS THE TEMPERATURE OF THE SMALLER TANK IF THE PRESSURE REMAINS CONSTANT?
V1/T1 = V2/T2
Don't forget to change T to Kelvin.
To solve this problem, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
In this case, since the pressure remains constant, we can say P1 = P2. Therefore, the equation becomes:
V1/T1 = V2/T2
Now let's substitute the given values into the equation:
V1 = 42.5 L (initial volume)
T1 = 43.5°C (initial temperature)
V2 = 25.0 L (final volume)
T2 = ? (final temperature)
First, we need to convert the initial temperature from Celsius to Kelvin. To do this, we add 273.15 to the Celsius temperature:
T1 = 43.5°C + 273.15 = 316.65 K
Now, we can rearrange the equation and solve for T2:
(V1/T1) = (V2/T2)
(V1 * T2) = (V2 * T1)
T2 = (V2 * T1) / V1
T2 = (25.0 L * 316.65 K) / 42.5 L
T2 ≈ 186.7 K
Therefore, the temperature of the smaller tank, when the pressure remains constant, is approximately 186.7 Kelvin.