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(a) Find the pressure of 4 g of O2 and 2 g of H2 confined in a bulb of 1 liter at 0oC. (b) What is the molar volume of a gas at SATP conditions? (c) Define and explain Gay Lussac's law. |
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Answer» (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 |
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