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Be sure to answer all parts. 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 5.64 g of SrH2 and 4.70 g of H2O. (a) How many moles of H2 can be produced from the given mass of SrH2?

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Answer:

Explanation:

SrHâ‚‚ + 2Hâ‚‚O = Sr(OH)â‚‚ + 2Hâ‚‚

90gm     36gm                  2 moles

5.64 g        4.7 g

water required for 5.64 g of SrHâ‚‚ = (36/ 90) x 5.64 g

= 2.256 g

water is in excess . Hence limiting reagent is SrHâ‚‚

90g SrH₂  makes 2 mole of water

5.64g SrHâ‚‚ makes water equal to mole = 2 x 5.64 / 90

= .125 mole .

mole of hydrogen formed = .125 .

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