Interpretation:
From the given options, the equilibrium constant expression for the reaction has to be chosen.
Concept Introduction:
Law of
The equilibrium constant is the product of molar concentrations of the product which is raised to its
Equilibrium Constant:
Consider a reaction,
Forward
Backward reaction rate
At equilibrium, the rate of forward reaction = rate of backward reaction
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General, Organic, and Biological Chemistry
- Consider the following hypothetical reactions. The equilibrium constants K given for each reaction are defined in terms of a concentration unit of molecules per liter. A(g)B(g)K=2X(g)2Y(g)K=62C(g)D(g)K=1 Assume that the reactions have reached equilibrium. Match each of these reactions with one of the containers I to IV (each of which has a volume of 1 L). Identify the color of each molecule (for example, is A red or blue?).arrow_forwardTest Yourself 4: For the reaction: CH3CH3(g) + 2H2O(g) + Ni(s) AH= +300 kJ/mol. 2CO(g) + 5H2(g) + Ni(s), (a) Write the equilibrium constant expression in Kp and Kc. (b) Will an increase in the reaction temperature of the system favor the formation of the products? (c) What is the effect on the rate of the reaction when the Ni is removed? (d) If the reaction was done in a 1000 mL flask, what would be the effect on the equilibrium if the volume of the flask is decreased to 500 mL?arrow_forwardProblem 6 Na₂(g) 2Na(g) constants. (1) NaCl(g) Na(g) + Cl(g) (2) Reaction 1 starts with No moles of Na₂ and zero moles of Na. Reaction 2 starts with No moles of NaCl and zero moles of Na and Cl. i) Using the extent of reaction, derive the corresponding expressions for the equilibrium ii) If both reactions take place at constant pressure as well as temperature, which extent of reaction 1 or 2 is greater and why?arrow_forward
- Exercise The chemicals A and B reacts to produce C and D A + B C+D The equilibrium constant (K) has a value of 0.30, Calculate the concentrations of A, B, C and D at equilibrium if [A]; = 0.2 M and [B]; = 0.5 M. Hints: 1. Building the ICE table produce the following quadratic equation (0.7x² +0.21x-0.3=0) 2. Solving quadratic equation (ax² + bx +c= 0) is carried out by: • Factoring by inspection Completing the square • Using the quadratic formula X -b± √b² - 4ac 2aarrow_forwardExercise 1. Write the equililuium constant expression, Kc, for the following reactions. Indicate also if the equilibrium is homogeneous or heterogeneous. 1. 3 NO) EN2Otq! + NCz) ECS + 4 Hag 2. CHafei + 2 H Sigi 3. Ni(CO ENig+ 4 CO 4. HFagi + F(an! 5. 2 Ago + Zn*taq) 2 Ag (aa + Zn(s) 6. 2 C2HG + 2 H2Ota) :2 C2Hgi + Ozig) CHAISI 7. C + 2 Hzig) 8. 4 HCkog) Ozie 2 H2O + 2 Claisarrow_forwardWhich of the following is the correct equilibrium constant expression for the reaction 3C(g)A(g)+2B(g) a. [A] [2B]/[3C] b. [3C]/[A] [2B] c. [A] [B]/[C] d. no correct responsearrow_forward
- 16. Heat + A + B ↔ C + DTo increase the amount of "D" present at equilibrium in the reaction vessel, you could a. add some "C" to the vessel b. cool the reaction vessel c. heat the reaction vessel d. remove some "B" from the vessel e. no correct responsearrow_forwardFill in the left side of this equilibrium constant equation for the reaction of carbonic acid (H,CO,) with water. D= K, Explanation Check 2022 McGraw Hill LLC. All R 80 F OL DCE Cloudy DELLarrow_forwardExercises 6-A. Consider the following equilibria in aqueous solution: (1) Ag* + Cl¯ = A£CI(aq) (2) AgCl(aq) + ci¯ = AgCl (3) AgCl(s) = Ag* + Cl¯ K = 2.0 × 10³ K = 9.3 × 10' K = 1.8 × 10-1o (a) Calculate the numerical value of the equilibrium constant for the reaction AGCI(s) = AgCl(aq). (b) Calculate the concentration of AgCl(aq) in eqilibrium with excess undissolved solid AgCl. (c) Find the numerical value of K for the reaction AgCl A£CI(s) + Cl¯.arrow_forward
- Write the concentration equilibrium constant expression for this reaction. CH;CO,C,H;(aq)+H,0(1)→CH;CO,H(aq)+C,H;OH(aq) Explanation Check 02022 McGraw Hl LLC All Rights Reserved K P Type here to search 99+ PUNZ AW CAOg 27 CaSZenBook F3 F4 F7 F8 F9 F1 %23 %24 3 7. E R T Y. U D H. K olo Carrow_forwardQuestion 5 ✓ Saved What is the concentration in molarity of magnesium ion in a saturated solution of magnesium phosphate? 1.88 x 10-5 M 1.33 x 10-6 M 3.06 x 10-¹2 M 1.91 x 10-8 M 3.12 x 10-24 M Question 6 Saved What is the equilibrium constant of the following reaction at 25°C? BaCrO4(s)= Ba²+(aq) + CrO42-(aq) 8.55 x 109 1.17 x 10-10 8.55 x 10-5 1.0 x 10-7 1.17 x 104arrow_forwardK = 9 K = 3 At equilibrium? At equilibrium? no yes O yes no X%3D2 At equiibrum7 At equilibr Jm7 yes ves no Explanation Check 1Larrow_forward
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