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17 Nov 2019
The chemical equilibrium being studied is H_2 + l_2 = 2HI In the beginning, only 0.05 mole of each H_2 and I_2 are present. When the system reaches equilibrium, the motor quantities are as follows: H_2 and I_2 = 0.02 mole each, HI = 0.06 moles. The reaction is taking place m a 2.0_container at 300 K. Assume all reactants and products behave as ideal gases. From this data, find extent of reaction, equilibrium constant K, delta G and delta Go Find K for this reaction at 500K, if delta Hf for HI = 26.5 Kj/mol At which pressure would liquid H_2 O have an activity of 1.03 at 298 k? Molar volume of water = 18.07 cm^3
The chemical equilibrium being studied is H_2 + l_2 = 2HI In the beginning, only 0.05 mole of each H_2 and I_2 are present. When the system reaches equilibrium, the motor quantities are as follows: H_2 and I_2 = 0.02 mole each, HI = 0.06 moles. The reaction is taking place m a 2.0_container at 300 K. Assume all reactants and products behave as ideal gases. From this data, find extent of reaction, equilibrium constant K, delta G and delta Go Find K for this reaction at 500K, if delta Hf for HI = 26.5 Kj/mol At which pressure would liquid H_2 O have an activity of 1.03 at 298 k? Molar volume of water = 18.07 cm^3
Nelly StrackeLv2
20 Jun 2019