(a)
Interpretation:
The equilibrium constant expression for the heterogenous reaction system
Concept Introduction:
Equilibrium constant: At equilibrium the ratio of products to reactants (each raised to the power corresponding to its
For a general reaction,
The concentration of solids and pure liquids do not change, so their concentration terms are not included in the equilibrium constant expression.
(b)
Interpretation:
The equilibrium constant expression for the heterogenous reaction system
Concept Introduction:
Refer part (a) for concept.
(c)
Interpretation:
The equilibrium constant expression for the heterogenous reaction system
Concept Introduction:
Refer part (a) for concept.
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Chapter 12 Solutions
OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)
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- 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_forwardConsider 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 the equilibrium constant expression for each of the following reactions in terms of concentrations. (a) CO2(g) + C(s) 2 CO(g) (b) [Cu(NH3)4)2+(aq) Cu2+(aq) + 4 NH3(aq) (c) CH3CO2H(aq) + H2O() CH3CO2(aq) + H3O+(aq)arrow_forward
- Write the equilibrium constant expression for each of the following reactions in terms of concentrations. (a) CO2(g) + C(s) 2 CO(g) (b) [Cu(NH3)4)2+(aq) Cu2+(aq) + 4 NH3(aq) (c) CH3CO2H(aq) + H2O() CH3CO2(aq) + H3O+(aq)arrow_forwardWrite the equilibrium constant expression for this reaction: C,H1,04(aq)+2 OH (aq) → 2 CH,CO0 (aq)+C,H,O2(aq) oloarrow_forwardWhat is the equilibrium constant expression for the reaction 4NO(g) + 6H2O(g) ⇌ 4NH3(g) + 5O2(g)?arrow_forward
- Consider the reaction: 2 CO(g) + O₂(g) 2 CO₂(g). The reaction is allowed to reach equilibrium in a sealed vessel. According to Le Chatelier's principle, what will happen to the equilibrium, if the volume of the vessel is decreased while the temperature is kept constant? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will be unchanged, but the reaction will shift to the right. (D) The equilibrium constant will increase and the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.arrow_forwardThe equilibrium constant for the reaction2 NO(g) + Br2(g) ⇌ 2 NOBr(g)is Kc = 1.3 x 10-2 at 1000 K. (a) At this temperature doesthe equilibrium favor NO and Br2, or does it favor NOBr?(b) Calculate Kc for 2 NOBr(g)⇌ 2 NO(g) + Br2(g).(c) Calculate Kc for NOBr(g)⇌ NO(g) + 1/2 Br2(g).arrow_forwardWrite equilibrium constant expression for the following:Fe2O3 (s) + 3 H2 (l) ⇌ 2 Fe (s) + 3 H2O (g)arrow_forward
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