(a)
Interpretation:
The concentration of all species after the attainment of equilibrium in the following reaction has to be determined.
Concept Introduction:
The condition of equilibrium is a state of balance of processes that runs in opposite directions. At equilibrium, the formation of product from reactant balances the formation of reactant from product. Also, the change in concentration of reaction and product seems to be negligible at equilibrium state.
The general equilibrium reaction is as follows:
Here,
(a)
Answer to Problem 14.87QE
The concentration of
Explanation of Solution
The given reaction occurs as follows:
The concentration of
The ICE table for the above reaction is as follows:
The concentration of
The concentration of
The equilibrium concentration of
Therefore the equilibrium concentration of
The equilibrium concentration of
Therefore the equilibrium concentration of
(b)
Interpretation:
The value of
Concept Introduction:
The general equilibrium reaction is as follows:
Here,
The expression of the equilibrium constant for the above reaction is as follows:
Here,
(b)
Answer to Problem 14.87QE
The value of
Explanation of Solution
The given reaction occurs as follows:
The expression of
Substitute
(c)
Interpretation:
The value of
Concept Introduction:
The relation of equilibrium constant
Here,
The formula to calculate the value of
The value of
(c)
Answer to Problem 14.87QE
The value of
Explanation of Solution
The given reaction occurs as follows:
Substitute 3 for the total number of moles of gas on product side and 2 for the total number of moles of gas on reactant side in equation (3).
The formula to convert degree Celsius to Kelvin is as follows:
Substitute
Substitute 1 for
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Chapter 14 Solutions
Chemistry: Principles and Practice
- At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?arrow_forwardKc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?arrow_forwardFor the reaction N2(g)+3H2(g)2NH3(g) show that Kc = Kp(RT)2 Do not use the formula Kp = Kc(RT)5n given in the text. Start from the fact that Pi = [i]RT, where Pi is the partial pressure of substance i and [i] is its molar concentration. Substitute into Kc.arrow_forward
- Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium constant, Kc, is 0.60 for PCl5(g) PCl3(g) + Cl2(g) Calculate the concentrations of all species after equilibrium has been reached.arrow_forwardWrite an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a productarrow_forwardWrite the equilibrium constant expression for each reaction in terms of activities, simplifying where appropriate. a C(s)+O2(g)CO2(g) b P4(s)+5O2(g)P4O10(s) c 2HNO2(g)+3Cl2(g)2NCl3(g)+H2(g)+2O2(g)arrow_forward
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