A gas occupies 275 ml at 0°C and 610 Torr. What
final temperature would be required to increase the
pressure to 760 Torr, the volume being held constant?
Yes
To find the final temperature required to increase the pressure of the gas while keeping the volume constant, we can use the combined gas law equation:
(P1 * V1) / T1 = (P2 * V2) / T2
Where:
P1 = initial pressure
V1 = initial volume
T1 = initial temperature
P2 = final pressure
V2 = final volume (held constant)
T2 = final temperature (to be determined)
In this case, the initial pressure (P1) is 610 Torr, the initial volume (V1) is 275 mL, the final pressure (P2) is 760 Torr, and the final volume (V2) is equal to the initial volume.
First, we need to convert the temperatures to Kelvin, as the combined gas law requires temperature values in Kelvin. To convert from Celsius to Kelvin, you simply add 273.15 to the Celsius temperature. So, in this case, the initial temperature (T1) is 0°C + 273.15 = 273.15 K.
Now we can plug in the given values into the combined gas law equation:
(610 Torr * 275 mL) / 273.15 K = (760 Torr * 275 mL) / T2
Next, we can rearrange the equation to solve for T2:
T2 = (760 Torr * 275 mL * 273.15 K) / (610 Torr * 275 mL)
Calculating the values:
T2 = (760 Torr * 275 mL * 273.15 K) / (610 Torr * 275 mL)
T2 = (760 * 273.15) / 610
T2 = 339.95 K
Therefore, the final temperature required to increase the pressure to 760 Torr while keeping the volume constant is approximately 339.95 K.