The volume of a gas at 85.0 kPa is 400.0 mL. If the pressure is increased to 177 kPa, what will be the new vol

Question

A gas at 85°C occupies a volume of 0.67 L. At what Celsius temperature will the volume increase to 1.02 L?
? °C

Answer 1

PV=nRT, so
P1V1=P2V2 <-- solve this for V2

Answer 2

Using the equation:
PV = nRT
Where :
P = pressure
V = volume
n = equals the number of mols in the gas
R = Rydhberg's constant
T = temperature of the substance

Because no other variables than the pressure and the volume are given, we assume all other variables to be constant, leaving P to be multiplied by V (as can easily be seen).
In the two situations presented in the question (the lower pressure and the higher pressure), there are different values given, therefore:

Initial pressure and volume = P1 (85.0 kPa) and V1 (400.0 mL)
Final pressure and volume = P2 (177 kPa) and V2 (?)

If you equate these, you can easily find the answer:
P1*V1 = P2*V2
(85)(400) = (177)V2
V2 = 192.09... mL

Therefore, the new volume is 192.1 mL

I hope this helped ^^;

Answer 3

V = 85*400/177 = 192.09 ml

Answer 4

The volumne shouldn't change if you are using the same container. Otherwise you have no Control in your experiment. You can't change 2 variables.