I. Directions: Write the equilibrium constant expression, Kc, for the followingreactions. Indicate also if the equilibrium is homogeneous orheterogeneous.-Section Break(Next Page)-1. 3 NO N½O(g) + NO29)2. CHa) + 2 H2Sig)CSz@) + 4 Hzg)3. Ni(CO)ag)ENiw + 4 CO)4. HF(aq)*(aq)+ Flaq)5. 2 Aga + Zn²* (aq)2 Ag*taq) + ZnC2 C2H&g + Ozg)6. 2 C2HAlg) + 2 H2O(g)7. C + 2 H2ig)FCHaa)8. 4 HCl(ag) + Ozíg):2 H2OM + 2 Cl2)

Equilibrium constant reaction: As per our guidelines we have to answer first three questions only.

I. Directions: Write the equilibrium constant expression, Kc, for the following reactions. Indicate also if the equilibrium is homogeneous or heterogeneous. Section Break(Next Page)- 1. 3 NO EN2Og) + NO29) 2. CHag) + 2 H2Sa) 3. Ni(CO)a(g) CS2«@) + 4 Hzg) ENiw + 4 CO) 4. HF(aq) H'aq) + F"(aq) 2 Ag*tag) + Zn :2 C2H«g + Ozig) 5. 2 Agw + Zn²*(aq) 6. 2 C2H9) + 2 H2O(g) 7. Cu + 2 H2ig)

I. Directions: Write the equilibrium constant expression, Kc, for the following reactions. Indicate also if the equilibrium is homogeneous or heterogeneous. Section Break(Next Page)- 1. 3 NO EN2Og) + NO29) 2. CHag) + 2 H2Sa) 3. Ni(CO)a(g) CS2«@) + 4 Hzg) ENiw + 4 CO) 4. HF(aq) H'aq) + F"(aq) 2 Agtag) + Zn :2 C2H«g + Ozig) 5. 2 Agw + Zn²(aq) 6. 2 C2H9) + 2 H2O(g) 7. Cu + 2 H2ig)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 103QRT: In Table 12.1 (←Sec. 12-3a) the equilibrium constant for the reaction ⇋ is given as 4.2 × 1052. If...

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The following reaction has KP=4.50105 at 720 K. N2(g)+3H2(g)2NH3 If a reaction vessel is filled with each gas to the partial pressures listed, in which direction will it shift to reach equilibrium? P(NH3)=93atm,P(N2)=48atm, and P(H2)=52
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium. a. If the volume is increased by a factor of 10.0. will the mole percent of N2O5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer. b. Calculate the mole percent of N2O5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.
The equilibrium constant K for the reaction 2CI(g)CI2(g) was measured as a function of temperature (Kelvin). A graph of In (K) versus 1/T for this reaction gives a straight line with a slope of 1.352 104 K and a y-intercept of 14.5 1. Determine the values of H and S for this reaction. See Exercise 79.
A common type of reaction we will study is that having a very small K value (K 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be perfomed. However, the math involved when solving equilibrium problems for reactions having small K values (K 1) is simplified. What assumption is made when solving the equilibrium concentrations for reactions with small K values? Whenever assumptions are made, they must be checked for validity. In general, the 5% rule is used to check the validity of assuming x (or 2 x, 3x, and so on) is very small compared to some number. When x (or 2 x. 3x. and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?
In Table 12.1 (←Sec. 12-3a) the equilibrium constant for the reaction ⇋ is given as 4.2 × 1052. If this reaction is so product-favored, why can large piles of yellow sulfur exist in our environment (as they do in Louisiana and Texas)?
Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.
Consider the system A(g)+2B(g)+C(g)2D(g)at 25C. At zero time, only A, B, and C are present. The reaction reaches equilibrium 10 min after the reaction is initiated. Partial pressures of A, B, and D are written as PA, PB, and PD. Answer the questions below, using LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more information required). (a) PD at 11 min PD at 12 min. (b) PA at 5 min PA at 7 min. (c) K for the forward reaction K for the reverse reaction. (d) At equilibrium, K Q. (e) After the system is at equilibrium, more of gas B is added. After the system returns to equilibrium, K before the addition of B K after the addition of B. (f) The same reaction is initiated, this time with a catalyst K for the system without a catalyst the system with a catalyst. (g) K for the formation of one mole of D K for the formation of two moles of D. (h) The temperature of the system is increased to 35C. PB at equilibrium at 25C PB at equilibrium at 35C. (i) Ten more grams of C are added to the system. PB before the addition of C PB after the addition of C.
A student studies the equilibrium I2(g)2I(g)at a high temperature. She finds that the total pressure at equilibrium is 40% greater than it was originally, when only I2 was present. What is K for this reaction at that temperature?
7-29 The following reaction was allowed to reach equilibrium at 25°C. Under each component is its equilibrium concentration. Calculate the equilibrium constant, K, for this reaction.
Consider the decomposition of ammonium hydrogen sulfide: NH4HS(s)NH3(g)+H2S(g) In a sealed flask at 25C are 10.0 g of NH4HS, ammonia with a partial pressure of 0.692 atm, and H2S with a partial pressure of 0.0532 atm. When equilibrium is established, it is found that the partial pressure of ammonia has increased by 12.4%. Calculate K for the decomposition of NH4HS at 25C.
Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert between two isomeric forms, finally reaching an equilibrium between them. This is true for the simple sugar glucose, C6H12O6, which exists in solution in isomeric forms called alpha-glucose and beta-glucose. If a solution of glucose at a certain temperature is analyzed, and it is found that the concentration of alpha-glucose is twice the concentration of beta-glucose, what is the value of K for the interconversion reaction?