Final answer:
To calculate the volume of hydrogen produced from a reaction between methane and water, one must use stoichiometry based on a provided balanced chemical equation and identify the limiting reagent. The volume of hydrogen can then be found using the ideal gas law, but without specific conditions or the balanced equation, the question cannot be answered accurately.
Step-by-step explanation:
The question is asking to determine the volume of hydrogen gas that can be produced from the reaction between methane (CH4) and water, as well as to identify the limiting reagent in the reaction using the provided masses of the reactants. To solve this, we'll need to use stoichiometry based on a balanced chemical equation. However, the chemical equation for the reaction has not been provided.
Usually, methane reacts with water in a steam reforming process to produce hydrogen and carbon monoxide:
CH4(g) + H2O(g) → CO(g) + 3H2(g)
We would first calculate the number of moles of both CH4 and H2O using their given masses and respective molar masses. Then, we would determine the mole ratio between the reactants from the balanced equation to find the limiting reagent. After identifying the limiting reagent, we can calculate the volume of hydrogen produced using the ideal gas law, provided that temperature and pressure conditions are specified or assuming standard temperature and pressure (STP).
However, sufficient information to provide a detailed response is not available, as the temperature and pressure conditions or the balanced chemical equation in the context of this reaction have not been given. Hence, any further calculation would be speculative without that information.