A Sample of Nitrogen Gas: Temperature and Volume Relationship
A sample of nitrogen occupies 3.50 liters under a pressure of 900. torr at 25.0 oC. At what temperature will it occupy 7.0 liters at the same pressure?
C. 323 °C
To solve this problem, we can use the combined gas law equation, which relates the initial and final volumes, pressures, and temperatures of a gas sample. The equation is:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Where:
P1 = Initial pressure
V1 = Initial volume
T1 = Initial temperature
P2 = Final pressure
V2 = Final volume
T2 = Final temperature
Given:
P1 = 900 torr
V1 = 3.50 liters
T1 = 25.0 °C
P2 = 900 torr
V2 = 7.0 liters
Converting the temperatures to Kelvin scale:
T1 = 25.0 °C + 273.15 = 298.15 K
Rearranging the equation to solve for T2:
T2 = (P2 * V2 * T1) / (P1 * V1)
Substituting the given values:
T2 = (900 torr * 7.0 liters * 298.15 K) / (900 torr * 3.50 liters)
T2 = 2 * 298.15 K
T2 = 596.3 K
Converting the temperature back to Celsius:
T2 = 596.3 K - 273.15 = 323.15 °C
Therefore, the temperature at which the nitrogen will occupy 7.0 liters at the same pressure is approximately 323 °C.
The temperature required for the nitrogen to occupy 7.0 liters at the same pressure is approximately 323 °C.
What is the temperature at which the nitrogen will occupy 7.0 liters at the same pressure? The temperature required for the nitrogen to occupy 7.0 liters at the same pressure is approximately 323 °C.