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![6.56 Use each expression for the equilibrium constant to write a
chemical equation.
88.D
[AB,]²
[A,][B,]²
[A,B,]
illupe 1ot a6. K= w
a. K =
e erl)
wollot
[A]°[B]³
%3B](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2c2b8110-d0c1-40b5-bcf7-745424b5efc2%2Ffc4519c2-788a-446b-9e24-688726e9210a%2Fh12h3i_processed.jpeg&w=3840&q=75)
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- Use the reaction below to answer the following questions. 2NO2 (??) ⇌ N2O4 (??) a.What is the expression for the equilibrium constant, Keq, for the reaction? b.If there are 0.400 moles of N2O4 and 0.500 moles of NO2 in a 1.00 L flask at equilibrium at 20°C,what is the Keq?Car engines produce pollution through numerous reactions. One such reaction is theoxidation of nitrogen into nitrogen monoxide:N2 + O2 ⇌ NOa. 1.00 mol N2, 2.00 mol O2, and no moles of NO are initially mixed. Atequilibrium there are 1.80 mol of O2 remaining. How many moles of N2 andNO are present at equilibrium? b. Calculate Kc for this reaction.c. Is the forward reaction, reverse reaction, or neither favored?When 2.3 moles of HBrO2 is dissolved in 2 liters of solution it is found at equilibrium that [H3O+] = . 067, calculate ki for HBrO2
- Consider the following reaction:Glycogen(aq)(stored glucose) + H2O(l) -->blood glucose(aq) + heata. Is the reaction exothermic or endothermic as written?b. Provide an equilibrium expression (K) for the reaction.c. How will the equilibrium shift if blood glucose is removed from the reaction?d. How will the equilibrium shift if the temperature is raised?Does the equilibrium for this 1.reaction favor reactants or products? Support your answer using the Keq value. 2. What are the units of Keq? Fe3+(aq) + HSCN (aq) ↔ FeSCN2+(aq) + H+ (aq)For the following reactions at equilibrium, identify which between the reactants and products is dominant. (ONLY 1 AND 2)
- SiO2(s) + 4HF(g) SiF4(g) + 2H2O (g) What happens, in the system at eq≡m, to: ___ mass of SiO2 if HF is added? two ways to make [SiF4] increase? _________________A sample of PCl5 was placed in a vessel with an original concentration of 0.40 mol/L. After the PCl5 has decomposed and equilibrium has been established, 25% of the PCl5 remains. PCl5(g) ---> PCl3(g) + Cl2(g) Equilibrium concentrations of PCl5, PCl3, and Cl2?1.. This question is given in the photo 2..The Haber process is used to produce ammonia for fertilizers: N2(g)+3H2(g)→2NH3(g) The reaction is performed at 300 Kand 500 Kand found to have equilibrium constants of 3.9×105and 1.2×10−1, respectively. Calculate ΔHand ΔSfor the reaction.
- If this reaction releases heat, what direction will the equilibrium shift when: 1. the amount of N_2N2 is decreased? 2. the heat of the system is increased? 3. an inert gas with pressure 3.00 atm is placed in the system? 4. the volume of the system is reduced? 5. a catalyst in the reaction is placed?Ammonia can be oxidized in oxygen as shown: 4 NH3(g) + 3 O2(g) <=> 2 N2(g) + 6 H2O(g). When 0.732 mol of NH3 and 0.666 mol of O2 are placed in a 1.00 L container at a certain temperature, the equilibrium {N2} is 0.1775. Calculate the value of Kc for the reaction. Give your answer to 4 decimal places.What effect will increasing the temperature have on the system at equilibrium? C3H8(g) + 5 O2(g) ⟷ 3 CO2(g) + 4 H2O(l) ΔHo = -2220 kJ The value of K will increase, and the reaction will shift toward the reactants. The value of K will increase, and the reaction will shift toward the products. The value of K will decrease, and the reaction will shift toward the products. The value of K will decrease, and the reaction will shift toward the reactants.
