**Topic: Reaction of Carbon Dioxide with Lithium Hydroxide on Spacecraft**1. In a spacecraft, the carbon dioxide exhaled by astronauts can be removed by its reaction with lithium hydroxide, LiOH, according to the following chemical equation: \[ \text{CO}_2 (g) + 2\text{LiOH} (s) \rightarrow \text{Li}_2\text{CO}_3 (s) + \text{H}_2\text{O} (l) \] If 20.0 moles of CO₂ is exhaled, the average amount exhaled by a person each day, how much (in grams) Li₂CO₃(s) is produced?This problem involves stoichiometry to determine the mass of lithium carbonate (Li₂CO₃) produced from a known quantity of carbon dioxide. Given the balanced chemical equation, you can calculate the mass of Li₂CO₃ by first determining the moles of Li₂CO₃ formed from 20 moles of CO₂ and then using the molar mass of Li₂CO₃ for the final conversion to grams.

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1. In a spacecraft, the carbon dioxide exhaled by astronauts can be removed by its reaction with lithium hydroxide, LiOH, according to the following chemical equation. CO2(g) + 2LİOH(s) → Li¿CO3(s) + H2O(1) If 20.0 moles of CO2 is exhaled, the average amount exhaled by a person each day, how much (in grams) Li2CO:(s) is produced?

1. In a spacecraft, the carbon dioxide exhaled by astronauts can be removed by its reaction with lithium hydroxide, LiOH, according to the following chemical equation. CO2(g) + 2LİOH(s) → Li¿CO3(s) + H2O(1) If 20.0 moles of CO2 is exhaled, the average amount exhaled by a person each day, how much (in grams) Li2CO:(s) is produced?

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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