Consider the gas-phase equilibrium system represented by the equation: 2H 20(g) 2 2H 2(g) + O 2(g) Given that the forward reaction (the conversion of "left-hand" species to "right-hand" species) is endothermic, which of the following changes will decrease the equilibrium amount of H2O? O adding He gas increasing the temperature at constant pressure O adding a solid phase calalyst decreasing the volume of the container (the total pressure increases) adding more oxygen O O

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Consider the gas-phase equilibrium system represented by the equation:
2H 20(g) 2 2H 2(g) + O 2(g)
Given that the forward reaction (the conversion of "left-hand" species to "right-hand" species) is endothermic, which of the following changes
will decrease the equilibrium amount of H2O?
adding He gas
increasing the temperature at constant pressure
adding a solid phase calalyst
decreasing the volume of the container (the total pressure increases)
adding more oxygen
Transcribed Image Text:Consider the gas-phase equilibrium system represented by the equation: 2H 20(g) 2 2H 2(g) + O 2(g) Given that the forward reaction (the conversion of "left-hand" species to "right-hand" species) is endothermic, which of the following changes will decrease the equilibrium amount of H2O? adding He gas increasing the temperature at constant pressure adding a solid phase calalyst decreasing the volume of the container (the total pressure increases) adding more oxygen
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