Introductory Chemistry: A Foundation
9th Edition
ISBN: 9781337399425
Author: Steven S. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Chapter 12, Problem 7CR
Interpretation Introduction
Interpretation:
The enthalpy change for the reaction is to be calculated by using Hess’ law.
Concept Introduction:
Hess’s Law or the law of constant heat of summation states that “the total enthalpy of the multistep reaction is the sum of the enthalpy of each step involved in it.”
Enthalpy gives the information regarding changes in heat or energy during the formation of reactant into products.
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Students have asked these similar questions
At 25 °C, the following reactions have the
equilibrium constants noted to the right of their
equations.
2CO(g) + O₂(g) ⇒ 2CO₂(g) Kç= 3.3 × 10⁹1
2H₂(g) + O₂(g) → 2H₂O(g) Kc= 9.1 × 108⁰
Use these data to calculate Kc for the reaction
H₂O(g) + CO(g) ⇒ CO₂(g) + H₂(g)
Kc=
i
Part 1
A student carried out an investigation to observe the effect of changing
concentration of sulfuric acid on the breakdown of calcium carbonate
(marble) chips. They changed the concentration of the acid between
each test but kept the size of the marble chips constant. The full equation
for the reaction and a graph of the overall results can be seen below.
CaCO3(s) + H₂SO4(aq) → CaSO4(aq) + CO2(g) + H₂O (1)
a)
b)
Rate of Reaction
*
Concentration of Acid (mol dm³)
Explain, using collision theory, why the student obtained
these results, and state what they could conclude about the
effect of changing concentration of acid on the rate of reaction
between calcium carbonate and sulfuric acid.
If the student had ground up the calcium carbonate chips into
a powder and run the tests again, what would you expect to
happen to the rate of reaction? Briefly explain why by
applying collision theory.
Part 2
The student ran the same experiment, but this time changed the
temperature, increasing it…
The equilibrium constant for the reaction PCI5(g) → PCI3 (g) + Cl₂(g) is 1.00 x 106 at 637 K and 9.10 x10² at
800 K. Use the van't Hoff equation to determine the standard enthalpy of reaction.
Units need to be in kJ/mol. Report values to 3 sig figs. Use gas constant value of 8.3145 J/molk.
Chapter 12 Solutions
Introductory Chemistry: A Foundation
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