1) Balance the reactions for the three theoretical decomposition reactions. A. sodium bicarbonate (s) → sodium hydroxide (s) + carbon dioxide (g) NaHCO3(s) → NaOH(s) + 2NaHCO3(s) B. sodium bicarbonate (s) → sodium oxide (s) + carbon dioxide (g) + water (g) CO₂(g) Na₂O(s) + CO₂(g) + NaHCO3(s) → Na₂CO3(s) + _H₂O(g) C. sodium bicarbonate (s)→ sodium carbonate (s) + carbon dioxide (g) + water (g) CO₂(g) + H₂O(g) (Reaction A) decrease (Reaction B) (Reaction C)
1) Balance the reactions for the three theoretical decomposition reactions. A. sodium bicarbonate (s) → sodium hydroxide (s) + carbon dioxide (g) NaHCO3(s) → NaOH(s) + 2NaHCO3(s) B. sodium bicarbonate (s) → sodium oxide (s) + carbon dioxide (g) + water (g) CO₂(g) Na₂O(s) + CO₂(g) + NaHCO3(s) → Na₂CO3(s) + _H₂O(g) C. sodium bicarbonate (s)→ sodium carbonate (s) + carbon dioxide (g) + water (g) CO₂(g) + H₂O(g) (Reaction A) decrease (Reaction B) (Reaction C)
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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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
Transcribed Image Text:HERO'S
cord all masses to the maximum number of
sig figs
Mass of beaker
1.
2.
3.
4.
Mass of beaker + NaHCO3
Initial mass of NaHCO3
Unlicensed printer. License is needed
Mass of beaker plus products after
heating.
5. Mass of product (actual yield)
Run 1
200°C
PostLab Questions
1) Balance the reactions for the three theoretical decomposition reactions.
A. sodium bicarbonate (s) → sodium hydroxide (s) + carbon dioxide (g)
NaHCO3(s) → NaOH(s) + CO₂(g)
NaHCO3(s) →
B. sodium bicarbonate (s) → sodium oxide (s) + carbon dioxide (g) + water (g)
2NaHCO3(s) → Na₂O(s) 2 CO₂(g) + H₂O(g)
109.600g
116.2369
6.636 g
113.77ад
113.7799-109-600g 109.540g-10$.2249
=140179g
= 4.316g
Na₂CO3(s) +
Run 2
400°C
C. sodium bicarbonate (s)→ sodium carbonate (s) + carbon dioxide (g) + water (g)
CO₂(g) + H₂O(g)
in
105. 224 д
112.155g
6.9319
109.540g
F
The reaction
after heat
and before
decrease
(Reaction A)
ef
(Reaction B)
(Reaction C)
Transcribed Image Text:Unlicensed printer. License is needed
Using the mass of sodium bicarbonate used for runs 1 and 2, calculate the theoretical yield of solid products
om each of the possible decomposition reactions, then calculate the percent yield by dividing your actual yield by the
theoretical yield you calculate for each reaction.
Reaction A
Run 1: Initial grams of NaHCO3 =
NaHCO3(s)
Run 2: Initial grams of NaHCO3 =
NaHCO3(s)
Reaction B
Run 1: Initial grams of NaHCO3 =
Percent yield =
NaOH(s) + __CO₂(g)
actual yield
theoretical yield
_Na₂O(s)
x 100
Theoretical yield (grams) of NaOH:
Percent yield (Run 1) =
Theoretical yield (grams) of NaOH:
Percent yield (Run 2) =
_H₂O(g)
_CO₂(g) +
Theoretical yield (grams) of Na₂0:
Percent yield (Run 1) =
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