some oxygen occupies 500.0 ml when its temperature is 40.0 C . if you wished to decrease the volume by 100.0 ml, to what temperture celsius would you need to lower the gas?
not sure how to set this up right..keep thinking i need to subtract 100.0 from 500.0 first,then set it up....
To solve this problem, you can use the combined gas law, which relates the initial and final conditions of temperature and volume for a given amount of gas. The combined gas law formula is:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Where:
P1 and P2 are the initial and final pressures (which we can assume to be constant since no pressure is given in the question)
V1 and V2 are the initial and final volumes
T1 and T2 are the initial and final temperatures
In this case, we know the initial temperature is 40.0 °C and the initial volume is 500.0 mL. Since we want to decrease the volume by 100.0 mL, the final volume will be V2 = 500.0 mL - 100.0 mL = 400.0 mL.
Now we need to solve for T2, the final temperature. Rearrange the equation to solve for T2:
T2 = (P2 * V2 * T1) / (P1 * V1)
Since the pressure is not given, we can cancel it out in the equation. Now, plug in the values:
T2 = (V2 * T1) / V1
T2 = (400.0 mL * 40.0 °C) / 500.0 mL
Convert the volumes to the same unit, for example, milliliters (mL).
T2 = (400.0 * 40.0) / 500.0
T2 = 32.0 °C
Therefore, you would need to lower the temperature to 32.0 °C in order to decrease the volume of the oxygen to 400.0 mL.