Can you explain 2.Small amounts of oxygen gas can be produced for laboratory use by heating potassiumchlorate, which causes it to decompose by the following reaction:KCIO;(s) →KC(s) +O2(g) (unbalanced) Balance the equation, and determine themass of oxygen that should be formed if 15.0 g of potassium chlorate decomposes.

The amount of the reactant or products used in a reaction can be calculated from the balanced…

2.Small amounts of oxygen gas can be produced for laboratory use by heating potassium chlorate, which causes it to decompose by the following reaction: KCIO;(s) → mass of oxygen that should be formed if 15.0 g of potassium chlorate decomposes. KCl(s) + O2(g) (unbalanced) Balance the equation, and determine the

2.Small amounts of oxygen gas can be produced for laboratory use by heating potassium chlorate, which causes it to decompose by the following reaction: KCIO;(s) → mass of oxygen that should be formed if 15.0 g of potassium chlorate decomposes. KCl(s) + O2(g) (unbalanced) Balance the equation, and determine the

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter3: Mass Relations In Chemistry; Stoichiometry

Section: Chapter Questions

Problem 67QAP: When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and...

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