We can use the ideal gas law to determine the volume of H2 produced by the reaction.
We first need to determine the moles of H2 produced from 15.0 g H2O. The molar mass of H2O is 2(1.01 g/mol H) + 16.00 g/mol O = 18.02 g/mol. From the given chemical equation, 4 moles of H2O form 4 moles of H2.
Cavendish prepared hydrogen in 1766 by the novel method of passing steam through a red-hot gun barrel:
4 H2O (g) + 3 Fe(s) ⟶ Fe3O4 (s) + 4 H2 (g)
(a) Outline the steps necessary to answer the following question: What volume of H2 at a pressure of 745 torr and a temperature of 20 °C can be prepared from the reaction of 15.0 g of H2O?
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