How Many Moles of H2 Gas Will Be Produced from CaH2 and H2O?

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SUMMARY

The reaction between calcium hydride (CaH2) and water (H2O) produces calcium hydroxide (Ca(OH)2) and hydrogen gas (H2). The balanced chemical equation is CaH2 + 2H2O -> Ca(OH)2 + H2. Given 0.80 moles of CaH2 and 1.29 moles of H2O, the limiting reactant must be identified to determine the amount of H2 produced. Since the stoichiometric ratio requires 2 moles of H2O for every mole of CaH2, the limiting reactant is CaH2, resulting in the production of 0.40 moles of H2 gas.

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Homework Statement


The reaction of calcium hydride and water produces calcium hydroxide and hydrogen as products. How many moles of H2 gas will be formed in the reaction between 0.80 mol CaH2 solid and 1.29 mol H2O liquid? (Two Significant Digits):



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The Attempt at a Solution


Well the balanced equation for this reaction I believe is CaH2 + 2H2O -> Ca(OH)2 + H2. Therefore the molar ration is about 2:1 so if 1.29 mol is reacts than 0.645 will be formed? But I'm always wrong? Any help is appreciated.
 
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You need 2 moles of water to 1 mole of CaH2. What ratio of reactants do you have? How does 1.29:0.80 compare with 2:1 ? Now, which is the limiting reactant? This is then what you use to determine the amount of hydrogen produced.
 

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