(a)
Interpretation:
The value of
Concept Introduction:
Relations between equilibrium constants:
Chemical equation | Equilibrium constant |
(a)
Answer to Problem 5H.2E
The value of
Explanation of Solution
The given reaction is as follows,
By multiplying
Therefore, the value of
(b)
Interpretation:
The value of
Concept Introduction:
Refer to part (a).
(b)
Answer to Problem 5H.2E
The value of
Explanation of Solution
The given reaction is as follows,
The reverse reaction of the above reaction can be written as follows,
By multiplying
Therefore, the value of
(c)
Interpretation:
The value of
Concept Introduction:
Refer to part (a).
(c)
Answer to Problem 5H.2E
The value of
Explanation of Solution
The given reaction is as follows,
By multiplying
Therefore, the value of
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Chapter 5 Solutions
Chemical Principles: The Quest for Insight
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- Consider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the concentration of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N2(g)? (3) adding water? (4) expanding the container? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?arrow_forwardWrite equilibrium constant expressions for the following reactions. For gases, use either pressures or concentrations. (a) 2 H2O2(g) 2 H2O(g) + O2(g) (b) CO(g) + O2g CO2(g) (c) C(s) + CO2(g) 2 CO(g) (d) NiO(s) + CO(g) Ni(s) + CO2(g)arrow_forwardBecause calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?arrow_forward
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