Use Charles's Law: V1 / T1 = V2 / T2
Constant pressure must be kept.
Absolute temp. must be used.
T1 = 0 + 273 = 273 degr.K
T2 = 200 + 273 = 473 degr.K
25 L / 273 K = V2 / 473 K
V2 = 25 x 473 / 273 = 43.315 L (final volume).
25 ml. The volume would not change. Now pressure on the other hand...
48.5 L (:
17 l
gas
17.....you said it in the question.
25 ml. The volume would not change. Now pressure on the other hand...
48.5 L (:
A fixed quantity of gas at a constant pressure exhibits a temperature of 27 degrees Celsius and occupies a volume of 10.0 L. Use Charles's law to calculate: the temperature of the gas in degrees Celsius in atmospheres if the volume is increased to 16.0 L
58 F
17 l
If the concentration of alcohol and water solution is 25 percent alcohol by volume, the volume of alcohol in a 200 solution is 50.
Hydrogen is a gas at 25 degrees Celsius.
gas
5.62 atm
Nitrogen would be a gas at 25 degrees Celsius.
17.....you said it in the question.
50.0 grams of what gas? This is the ideal gas law. Pressure * Volume = moles gas * the R constant * temperature in Kelvin PV = nRT