🤓 Based on our data, we think this question is relevant for Professor Selampinar's class at UCONN.
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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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.
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Based on our data, we think this problem is relevant for Professor Selampinar's class at UCONN.
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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.