Calcium hydride reacts with water to produce calcium hydroxide and hydrogen gas. CaH₂ (8) + 2 H₂O(l) Ca(OH)2 (s) + H₂(g) If 7.003 g CaH₂ is combined with 61.000 g H₂O, the reaction proceeds until all the CaH₂ is consumed. The hydrogen gas escapes to the environment, and the final weight of the flask is 67.332 g. The remaining water is evaporated, leaving 12.327 g Ca(OH)2. What mass of water is consumed in the reaction? g H₂O
Calcium hydride reacts with water to produce calcium hydroxide and hydrogen gas. CaH₂ (8) + 2 H₂O(l) Ca(OH)2 (s) + H₂(g) If 7.003 g CaH₂ is combined with 61.000 g H₂O, the reaction proceeds until all the CaH₂ is consumed. The hydrogen gas escapes to the environment, and the final weight of the flask is 67.332 g. The remaining water is evaporated, leaving 12.327 g Ca(OH)2. What mass of water is consumed in the reaction? g H₂O
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![**Chapter 4 - Stoichiometry: Quantitative Information About Chemical Reactions**
**Calcium hydride reacts with water to produce calcium hydroxide and hydrogen gas.**
The chemical equation for the reaction is:
\[ \text{CaH}_2(s) + 2 \text{H}_2\text{O}(l) \rightarrow \text{Ca(OH)}_2(s) + \text{H}_2(g) \]
When 7.003 g of CaH₂ is combined with 61.000 g of H₂O, the reaction proceeds until all the CaH₂ is consumed. The hydrogen gas escapes to the environment, and the final weight of the flask is 67.332 g. The remaining water is evaporated, leaving 12.327 g of Ca(OH)₂. What mass of water is consumed in the reaction?
Calculate the mass of H₂O:
\[ \text{g H}_2\text{O} \]
This exercise demonstrates the calculation of the mass of water consumed in the stoichiometric reaction between calcium hydride and water by analyzing the changes in mass before and after the reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff7ba9c54-af2b-48c5-8dd4-4f214c676725%2F5b739c9f-863c-4bd4-bf18-ebe2e2187612%2Fbx3nchc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chapter 4 - Stoichiometry: Quantitative Information About Chemical Reactions**
**Calcium hydride reacts with water to produce calcium hydroxide and hydrogen gas.**
The chemical equation for the reaction is:
\[ \text{CaH}_2(s) + 2 \text{H}_2\text{O}(l) \rightarrow \text{Ca(OH)}_2(s) + \text{H}_2(g) \]
When 7.003 g of CaH₂ is combined with 61.000 g of H₂O, the reaction proceeds until all the CaH₂ is consumed. The hydrogen gas escapes to the environment, and the final weight of the flask is 67.332 g. The remaining water is evaporated, leaving 12.327 g of Ca(OH)₂. What mass of water is consumed in the reaction?
Calculate the mass of H₂O:
\[ \text{g H}_2\text{O} \]
This exercise demonstrates the calculation of the mass of water consumed in the stoichiometric reaction between calcium hydride and water by analyzing the changes in mass before and after the reaction.
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