Assuming you start with 1.25 g of pure aluminum, calculate the following: 1) The amount of potassium hydroxide, KOH, in grams, needed to react with all of the 1.25 g of Al. The reaction is: 2 A1 (s) + 2КОН (аq) + 6 Н20 (1) 2 K (аq) + 2 AI(ОН)4 (аq) + 3 Н2 (в) g 2) The amount of KOH needed, in grams, in reaction 1 if you want to have 10% excess KOH. g 3) The amount of water, in milliliters, that will react with the Al and KOH in reaction 1. ml

Assuming you start with 1.25 g of pure aluminum, calculate the following: 1) The amount of potassium hydroxide, KOH, in grams, needed to react with all of the 1.25 g of Al. The reaction is: 2 A1 (s) + 2КОН (аq) + 6 Н20 (1) 2 K (аq) + 2 AI(ОН)4 (аq) + 3 Н2 (в) g 2) The amount of KOH needed, in grams, in reaction 1 if you want to have 10% excess KOH. g 3) The amount of water, in milliliters, that will react with the Al and KOH in reaction 1. ml

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter5: Stoichiometry

Section: Chapter Questions

Problem 103E: Silicon is produced for the chemical and electronics industries by the following reactions. Give the...

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The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.
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