Boyle's Rule: If the temperature and volume of the ideal gas remain constant in a closed system, the absolute pressure that a given mass of the gas exerts is inversely proportional to the space it takes up.
P1V1 = P2V2
447 × 86.4 = 1240 × V2
V2 = 447 × 86.4 / 1240
V2 = 31.146 mL
At constant temperature (T) and molecular weight (M), volume (V) decreases as pressure (P) increases (n)
PV = nRT
V = nRT/P
V = 4.55 × 0.082 × 285 / 7.32
Where R = ideal gas constant = 0.082 (L) (atm) (mole) -1(K) -1
V is equal to 14.53 L or 14530 cm3.
Charles's Rule: When pressure is held constant, a given mass of gas has a straight relationship between its volume and absolute temperature.
V1T2 = V2T1
1 × 263 = V2 × 310
V2 = 1 × 310 / 263
V2 = 1. 179 L
Volume (V) increases at constant pressure (P) and mole as temperature (T) rises (n)
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