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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FREE Expert Solution
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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?

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 Limiting Reagent concept. You can view video lessons to learn Limiting Reagent Or if you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems .

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Our tutors rated the difficulty of Metal hydrides react with water to form hydrogen gas and met... as medium difficulty.

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