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Problem: Metal hydrides react with water to form hydrogen gas and metal hydroxide. For example, SrH2 (s) + 2H2O (l) → Sr(OH)2 (s) + 2H2 (g) You wish to calculate the mass of hydrogen gas that can be prepared from 7.27 g of SrH  2  and 6.06 g of H2O. (a) How many moles of H2 can be produced from the given mass of SrH 2? (b) How many moles of H2 can be produced from the given mass of H 2O?  (c) Which is the limiting reactant? (d) How many grams of H2 can be produced? 

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Problem Details

Metal hydrides react with water to form hydrogen gas and metal hydroxide. For example, 

SrH2 (s) + 2H2O (l) → Sr(OH)2 (s) + 2H2 (g) 

You wish to calculate the mass of hydrogen gas that can be prepared from 7.27 g of SrH  2  and 6.06 g of H2O. 

(a) How many moles of H2 can be produced from the given mass of SrH 2


(b) How many moles of H2 can be produced from the given mass of H 2O?  


(c) Which is the limiting reactant? 

(d) How many grams of H2 can be produced? 


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Our tutors have indicated that to solve this problem you will need to apply the Limiting Reagent concept. If you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.

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Based on our data, we think this problem is relevant for Professor Korzeniewski's class at TTU.