A chemist produces 460 ml of nitrogen gas at -43 degrees celsius and constant pressure. To what celsius temperature must the nitrogen be warmed in order for it to have a volume of 600 ml?
the volume is directly related to the ABSOLUTE temperature (ºK)
ºK = ºC + 273
600 / 460 = ? / 230
To determine the required Celsius temperature, we will use the combined gas law equation, which states that the initial pressure times the initial volume divided by the initial temperature is equal to the final pressure times the final volume divided by the final temperature.
The equation can be represented as:
(P1 * V1 / T1) = (P2 * V2 / T2)
Let's assign the given values to the variables:
V1 = 460 ml (initial volume)
T1 = -43 degrees Celsius (initial temperature)
V2 = 600 ml (final volume)
P1 = P2 (constant pressure, hence pressure can be canceled out in the equation)
Now, substituting the values into the equation:
(460 ml / -43°C) = (600 ml / T2)
To solve for T2, cross-multiply and solve for T2:
460 ml * T2 = 600 ml * -43°C
T2 = (600 ml * -43°C) / 460 ml
T2 = -56.09°C
Therefore, the nitrogen gas must be warmed to approximately -56.09 degrees Celsius to reach a volume of 600 ml.