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- For the following combustion reactions, predict whether compression will favour the formation of products or reactants, or whether there will be no change in the equilibrium composition:(a) C4H8(g) + 6 O2(g) → 4 CO2(g) + 4 H2O(I)(b) C2H5OH(I) + 3(1)/(2) O2(g) → 2 CO2(g) + 3 H2O(I)(c) C6H12O11(s) + 3(1)/(2) O2(g) → 6 CO2(g) + 6 H2O(I)(d) 2 C6H5NH2(1) + 17(1)/(2) O2(g) → 12 CO2(g) + 7 H2O(I) +2 NO2(g)The reaction P4(g) 2 2 P2(g) is endothermic and begins to occur at moderate temperatures. (a) In which direction do you expect deviations to occur from Boyle's law, P ∞ 1/V (constant T), for gaseous P4? (b) In which direction do you expect deviations to occur from Charles's law, V « T (constant P), for gaseous P4?For the reaction 4HCl(g) +O2(g) == 2Cl2(g) + H2O (g), Keq =889 at 480 o If 0.03 mole HCl , 0,02 mole O2 , 0.08 mole Cl2 and 0.07 mole H2O were mixed in 1 liter container, in what direction will the reaction proceed. Support your answer.
- A gaseous mixture of CO and CO2 having total volume 150 mL is passed through a tube containing excess of red hot charcoal to cause the following reaction: CO(g) + C(s) - 2CO(g) The volume increases to 250 mL. Identify the correct statement. (a) Original mixture contains 50% by moles CO. (b) Original mixture contains 33.33% by moles CO. (c) Original mixture contains 33.33% by moles CO2. (d) Mole fraction of CO2 in the original mixture is 0.4.C6H12O6(aq) + 6O2(g) 6CO2(g) + 6H2O(l)ΔH = –2802.7 kJ mol –1a) Write an expression for the equilibrium constant for this reaction.b) At equilibrium, the concentration of the reactants and products are determined as [CO2] = 0.30 M, [O2] = 0.040 M and [C6H12O6] = 0.065 M. Determine the value of the equilibrium constant (Kc) and predict the whether the products or reactants will be favoured at equilibrium.c) Given that the concentrations of the reactants and products at a particular time are [CO2] = 0.65 M, [O2] = 0.020 M and [C6H12O6] = 0.055 M, determine the reaction quotient (Qc). Compare the Kc and Qc values and predict the favoured direction of the reaction.d) Explain the effect on equilibrium of:i) Increasing temperatureii) Increasing pressureiii) Decreasing the concentration of oxygeniv) Increasing the concentration of carbon dioxidev) Adding a catalystWhat is the mass-action expression, Qc, for the following chemical reaction? 4H30*(aq) + 2CI"(aq) + MnO2(s) Mn2+(aq) + 6H2O() + Cl2(g) ABBREVIATIONS AND SYMBOLS RFaraday constant A free energy atm frequency ugas constant NA gram "Chour e joule C kelvin dkilo prefix E liter Emeasure of pressure mm Hg vapor pressure Hmilli prefix S molal Kmolar CONSTANTS amount of substance ampere atmosphere atomic mass unit Avogadro constant Celsius temperature centi- prefix coulomb density electromotive force energy of activation enthalpy F molar mass mole Planck's constant M mol R-8.314 J motK R-0.08314 L bar mol K pressure rate constant reaction quotient second K speed of light k temperature, K time F-96,500 C mol F=96,500 J V'mol NA-6.022 x 102 mol h-6.626 x 10 MJS e-2.998 x 10 ms VP 0°C-273.15 K volt V I atm -1.013 bar - 760 mm Hg Specific heat capacity of H;0- 4.184 Jg'K m - volume M entropy equilibrium constant 1 PERIODIC TABLE OF THE ELEMENTS 18 1A 1 H 8A 2 13 14 4A 15 16 17 Не 1.008 ЗА 4.003 7A…
- JO(g) at high (g), with the gases treated as perfect. E6A.5(b) Write the equilibrium constant for the reaction CH₂(g) + 3 Cl₂(g) ⇒CHCl,(1) + 3 HCl(g), with the g CHC1₂(1) + 3 HCl(g), with the gases treated as perfect. A diiw 1000 ABOUT E6A.6(a) Use data founde Resource section to decide which ofHypochlorous acid (HOCI) is produced by bubbling chlorine through an agitated suspension of mercury(II) oxide in water. The chemical equation for this process is 2 Cl2(g) + 2 HgO(s) + H;O(€)=HgO · HgCl2(s) + 2 HOC(aq) Write the equilibrium expression for this reaction.(a) N₂(g) + O₂(g) = 2NO(g) (b) BaSO3(s) BaO(s) + SO₂(g) (c) NH3(aq) + H₂O (1) For the following reactions, write the mathematical expression for the reaction quotient, Qc,: NH4+ (aq) + OH-(aq) (d) Br₂(g) = 2Br(g) (e) 2SO₂(g) + O₂(g) = 2SO3(g) (f) NH₂(g) +20₂(g) = CO₂(g) + 2H₂O(1) 10 (h) N₂(g) + 3H₂(g) = 2NH3(g) (i) NH₂Cl(s) = NH3(g) + HCl(g) (1) CO₂(g) + H₂(g) = CO(g) + H₂O(g) openstax Which systems are homogeneous (heterogeneous) equilibria? acid-base equilibria?
- 2 When 50 cm' of hydrochloric acid of concentration 2.0 mol dm is added to 50 cm' of sodium hydroxide solution of concentration 2.0mol dm, the temperature increase is 13.0°C HCl(aq) + NAOH(aq) + NaCl(aq) + H,O(1) The experiment is repeated using 25 cm of the same hydrochloric acid and 50 cm' of the same sodium hydroxide solution. What is the temperature increase? O A 4.9°C I B 6.5°C I C 8.7°C D 13.0°Ca sealed one liter reaction vessel was loaded with 0.245mol n2o and 0.574 mol o2. the system (represented by the balanced chemical equation) was allowed to reach equilibrium. where the concentration of no2 was measured to be 0.194M. 2N2O(g)+3O2(g)=4NO2. Determine the equilibrium constant (Kc) for the reaction under these conditions.In the gas phase reaction 2 A(g) + B(g) = 3 C (g) + 2 D (g) it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25oC, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate (a) the mole fractions of each species, (b) KX, (c) KP and (d) △Go . Answer: [0.087 (A); 0.370 (B); 0.196 (C); 0.348 (D); 0.326; 0.325; 2.76 kJ]