At 119 degrees C, the pressure of a sample of nitrogen is 1.94 atm. What will the pressure be at 282 degrees C, assuming constant volume?
Answer in units of atm
P1/T1 = P2/T2
Do I have to change celcius to K?
Yes.
To find the pressure at 282 degrees C, assuming constant volume, you can use the combined gas law equation. The combined gas law relates the initial and final states of a gas when any two of the following variables are held constant: pressure (P), volume (V), and temperature (T). The equation is as follows:
(P1 * V1) / T1 = (P2 * V2) / T2
In this case, we are assuming constant volume (V1 = V2). We are given that P1 = 1.94 atm and T1 = 119 °C (or 119 + 273.15 = 392.15 K). We are asked to find P2 at T2 = 282 °C (or 282 + 273.15 = 555.15 K).
Plugging in the values into the equation:
(1.94 atm * V1) / 392.15 K = (P2 * V1) / 555.15 K
Since V1 cancels out, we can simplify the equation to:
1.94 / 392.15 = P2 / 555.15
Now, we can solve for P2 by multiplying both sides of the equation by 555.15:
P2 = (1.94 / 392.15) * 555.15
Calculating this expression will give you the pressure, P2, at 282 degrees C assuming constant volume.