EBK CHEMISTRY: PRINCIPLES AND REACTIONS
8th Edition
ISBN: 9780100547964
Author: Hurley
Publisher: YUZU
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Textbook Question
Chapter 8, Problem 22QAP
Small amounts of oxygen gas can be prepared in the laboratory by decomposing potassium chlorate with heat. A by-product of the decomposition is potassium chloride. When one mole of potassium chlorate decomposes, 44.7 kJ are evolved.
(a) Write a balanced thermochemical equation for the decomposition of one mole of potassium chlorate.
(b) Is the reaction exothermic?
(c) Draw an energy diagram showing the path of this reaction. (Figure 8.6 is an example of such an energy diagram.)
(d) What is ΔH when 3.00 g of potassium chlorate decompose?
(e) How many grams of potassium chlorate need to be decomposed to liberate fifteen kilojoules of heat?
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Please help me to figure this out. I got 24 is that correct? Please step by step help.
The initial rates method can be used to
determine the rate law for a reaction.
using the data for the reaction below, what is
the rate law for reaction?
A+B-C
-
ALA]
At
(mot
Trial [A] (mol)
(MD
2
1
0.075
[B](
0.075
mo
LS
01350
2
0.075
0.090 0.1944
3
0.090 0.075
0.1350
Report value of k with two significant Figure
Compare trials 1 and 2 where [B] is
constant.
The rate law can be written as: rate
= k[A][B]".
rate2
0.090
= 9.
rate1
0.010
[A]m
6.0m
= 3m
[A] m
2.0m
Chapter 8 Solutions
EBK CHEMISTRY: PRINCIPLES AND REACTIONS
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