I don't understand.. 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.

Given data mass of potassium chlorate (KClO3) decompose = 15.0 g Chemical reaction : KClO3 (s) →…

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. KCI(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. KCI(s) +. O2(g) (unbalanced) Balance the equation, and determine the

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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I don't understand..

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) →
KC(s) +
O2(g) (unbalanced) Balance the equation, and determine the
mass of oxygen that should be formed if 15.0 g of potassium chlorate decomposes.

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