2. The reaction of calcium hydride with water can beused to prepare small quantities of hydrogen gas, asis done to fill weather-observation balloons.CaH2(s) + H2O(1) → Ca(OH)2(s) + H2(g) (not balanced)(a) How many grams of H2(g) result from the reactionof 134 g CaH2 with an excess of water?(b) How many grams of water are consumed in thereaction of 58.3 g CaH2?(c) What mass of CaH2(s), in g, must react with anexcess of water to produce 4.15 x 1024 molecules ofH2?

Answered: Image /qna-images/answer/c8702875-2523-49ed-91d5-bf35648cfcab.jpg

2. The reaction of calcium hydride with water can be used to prepare small quantities of hydrogen gas, as is done to fill weather-observation balloons. CaH2(s) + H2O(1) → Ca(OH)2(s) + H2(g) (not balanced) (a) How many grams of H2(q) result from the reaction of 134 g CaH2 with an excess of water? (b) How many grams of water are consumed in the reaction of 58.3 g CaH2? (c) What mass of CaH2(s), in g, must react with an excess of water to produce 4.15 x 1024 molecules of H2?

2. The reaction of calcium hydride with water can be used to prepare small quantities of hydrogen gas, as is done to fill weather-observation balloons. CaH2(s) + H2O(1) → Ca(OH)2(s) + H2(g) (not balanced) (a) How many grams of H2(q) result from the reaction of 134 g CaH2 with an excess of water? (b) How many grams of water are consumed in the reaction of 58.3 g CaH2? (c) What mass of CaH2(s), in g, must react with an excess of water to produce 4.15 x 1024 molecules of H2?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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