12) Calculate AS° (in JK' mol³) of the following reaction: 2NO; [g] → 2NO (g) +0₂ (g) = (S" JK mol: (0) 205 (NO)-211, (NO)=240) B) 136 (147) D) 172
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![12) Calculate AS° (in JK' mol³) of the following reaction:
2NO; [g] → 2NO (g) +0₂ (g)
=
(S" JK mol: (0) 205 (NO)-211, (NO)=240)
B) 136
(147)
D) 172](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd505ccdb-d31d-449e-82dd-9dc3d3223c88%2F3549cd02-030b-4840-b0c9-2d65eb3c97c3%2Frxeq5dr_processed.jpeg&w=3840&q=75)
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- 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 catalystAt 432 °C, Keq = 0.00309 for the reaction: (a) What is the value of Keq for the reaction NOBr(g) NO(g) + 1/2 Br₂(g)? Kea NO(g) + 1/2 Br₂(g) → NOBr(g) (b) What is the value of Keq for the reaction 2 NO(g) + Br₂(g) = 2 NOBr(g)? Kea = (c) What is the value of Keq for the reaction 2 NOBr(g) 2 NO(g) + Br₂(g)? Kea =snip
- The emission of NO, by fossil fuel combustion can be prevented by injecting gaseous urea into the combustion mixture. The urea reduces NO (which oxidizes in air to form NO2) according to the reaction: 2 CO(NH;)»(3) + 4 NO(3) + O2(8) 4 Na(8) + 2 CO;(g) + 4 H¿O(g) Suppose that the exhaust stream of an automobile has a flow rate of 2.55 L/s at 655 Kand contains a partial pressure of NO of 12.4 torr. What total mass of urea is necessary to react complete- ly with the NO formed during 8.0 hours of driving?At 475 oC, Keq = 0.230 for the reaction: 1/3 NO2(g) + 1/3 N2O(g) (equilibrium arrows) NO(g) (a) What is the value of Keq for the reaction NO(g) 1/3 NO2(g) + 1/3 N2O(g)?Keq = .(b) What is the value of Keq for the reaction NO2(g) + N2O(g) 3 NO(g)?Keq = .(c) What is the value of Keq for the reaction 3 NO(g) NO2(g) + N2O(g)?Keq = .b) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction СO(g) +2H2(g) — CHОН (g) At 298.15 K, AH.co (0)= -26.41 kcal/mol, AH AG.co (9)= -32.8079 kcal/mol, AG cH,oh(9)= -38.69 kcal/mol, °.CH20H(9)= -48.08 kcal/mol, The standard heat capacity of various components is given by, CO = a + bT + cT² + dT³, where C, is in cal/mol-K and T is in K b x10² с х105 d x10° Соmponent CH3OH а 4.55 2.186 -0.291 -1.92 CO 6.726 0.04 0.1283 -0.5307 H2 6.952 -0.0457 0.09563 -0.2079
- b) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction Co(g) +2H2(g) → CH;OH (g) At 298.15 K, AH?.co )= -26.41 kcal/mol, AH?.CH,OH()= -48.08 kcal/mol, AG.co )= -32.8079 kcal/mol, AG.CH,OH(@)= -38.69 kcal/mol, The standard heat capacity of various components is given by. CS = a + bT + cT2 + dT³, where C is in cal/mol-K and T is in K |Component b x10 e x105 d x10° a -0.291 CH3OH CO 4.55 2.186 -1.92 6.726 0.04 0.1283 -0.5307 H2 6.952 -0.0457 0.09563 -0.2079When ethanol (CH;CH;OH) burns in oxygen, carbon dioxide and water are formed. (i) Write the equation which describes this reaction. (ii) Using the data below, calculate the value for AH° for the combustion of ethanol. AH; (CH;CH2OH(1)) = - 277.0 kJmol1 AH, (CO2(g)) = - 393.7 kJmol1 AH: (H2O()) = - 285.9 kJmol1Potassium chromate and lead (II) acetate are both dissolved in a beaker of water, where they react to form solid lead (II) chromate. What is the balanced equation describing this reaction? K:Cro.(aq) + Pb(C-H:O-):(sq) → PbCrO«(,) + KC:H:0:(3q) O 2K:Cro.(aq) + Pb(C:H:O-):(sq) PbCrO.() + 2KC:H.0:(aq) O K:Cro.(aq) + Pb(C:H.O:):(aq) -> PbCrO.(.) + 2KC:H:0:(aq) 2K.CrO.(sq) + Pb(C:H:0:):(aq) - PbCrO-(.) + KC:H:0:(aq) -->
- (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?› Calculate the value of the equilibrium constant, Kỵ, for the reaction Q(g) + X(g) — 2M(g) + N(g) given that Kc = M(g) — Z(g) 6R(g) 2 N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9R(g) Kc1 = 3.48 Kc2 Kc3 = 0.587 = = 13.6Calculate the value of the equilibrium constant, Kc , for the reaction Q(g)+X(g)↽−−⇀2M(g)+N(g) given that M(g)↽−−⇀Z(g) Kc1=3.92 6R(g)↽−−⇀2N(g)+4Z(g) Kc2=0.494 3X(g)+3Q(g)↽−−⇀9R(g) Kc3=14.0
