(a) Number of moles of O2
= \(\frac{Mass\,of\,O_2}{Molar\,mass\,of\,O_2}\) = \(\frac{4}{32}\) = 0.125
= \(\frac{Mass\,of\,H_2}{Molar\,mass\,of\,H_2}\) = \(\frac{2}{2}\) = 1
Total moles = 0.125 + 1 = 1.125
According to ideal gas equation, -
PV = nRT
[V = 1 L, n = 1.125 moles, T = 0 + 273 = 273 K, P =?]
\(\therefore\) P = \(\frac{nRT}{V}\)
= \(\frac{1.125\,moles\times0.0821\,L\,atm\,K^{-1}mol^{-1}\times273\,K}{1\,L}\)
= 25.215 atm
(b) At SATP, the molar volume of a gas is 24.789 L mol-1
(c) Gay Lussac's Law: According to this law, “At constant volume, pressure of a fixed amount of a gas varies directly with the temperature." Mathematically, P \(\propto\) T
Or \(\frac{P}{T}\) = = constant = K