(a)
Interpretation:
The equilibrium constant
Concept introduction:
Equilibrium constant
In gas phase reactions, partial pressure is used to write equilibrium equation than molar concentration. Equilibrium constant
Consider the reaction where A reacts to give B.
On rearranging,
Where,
The pressure of each species of ideal gas and its molar concentration are directly proportional to each other.
In same way
Where,
R is gas constant
T is absolute temperature
(b)
Interpretation:
At equilibrium, partial pressure of all gas in reaction has to be calculated. Also concentration of hydrogen gas in
Concept introduction:
Calculation of equilibrium partial pressure from initial partial pressure:
- The balanced equation for given reaction has to be written.
- Set up an equilibrium table to calculate x value
- The value of x is solved by substituting partial pressures of chemical species in equilibrium constant expression.
- The partial pressure of chemical species at equilibrium is calculated from value of x
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General Chemistry: Atoms First
- Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.arrow_forwardAt 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_forwardAt a temperature of 60 C, the vapor pressure of water is 0.196 atm. What is the value of the equilibrium constant KP for the transformation at 60 C? H2O(l)H2O(g)arrow_forward
- The decomposition of PCl5(g) to form PCl3(g) and Cl2(g) has Kc = 33.3 at a high temperature. If the initial concentration of PCl5 is 0.1000 M, what are the equilibrium concentrations of the reactants and products?arrow_forwardIodine chloride decomposes at high temperatures to iodine and chlorine gases. 2ICl(g)I2(g)+Cl2(g)Equilibrium is established at a certain temperature when the partial pressures of ICl, I2, and Cl2 are (in atm) 0.43, 0.16, and 0.27, respectively. (a) Calculate K. (b) If enough iodine condenses to decrease its partial pressure to 0.10 atm, in which direction will the reaction proceed? What is the partial pressure of iodine when equilibrium is reestablished?arrow_forwardYou place 0.600 mol of nitrogen, N2, and 1.800 mol of hydrogen, H2, into a reaction vessel at 450C and 10.0 atm. The reaction is N2(g)+3H2(g)2NH3(g) What is the composition of the equilibrium mixture if you obtain 0.048 mol of ammonia, NH3, from it?arrow_forward
- Write 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_forward12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.arrow_forwardWhat is the pressure of BrCl in an equilibrium mixture of Cl2, Br2, and BrCl if the pressure of CI2 in the mixture is 0.115 atm and the pressure of Br2 in the mixture is 0.450 atm? Cl2(g)+Br2(g)2BrCl(g)KP=4.7102arrow_forward
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