Question

At 142◦C, the pressure of a sample of nitrogen is 1.92 atm. What will the pressure be at 218◦C, assuming constant volume?

Answer in units of atm

Answer 1

please help ):

Answer 2

Use ideal gas law, which says:\[\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}\]Where P-pressure; V-volume, T-temperature
Since V1=V2, you can simplify this expression to:\[\frac{P_1}{T_1}=\frac{P_2}{T_2}\]
So, first convert temperatures from Celsius to Kelvin
\[\ T_1= 142 + 273.15 = 415.15 K\]\[\ T_2= 218 + 273.15 = 491.15 K\]\[\ P_1= 1.92\ atm\]
Solve the above expression for P2 and plug in the values.

Answer 3

so it's 391489.7712

Answer 4

Well, no. You can tell that this is wrong just by looking at the number you got, that's a pretty big pressure :D.What expression did you get for P2?