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 -119 °C, Keq = 0.472 for the reaction: (a) What is the value of Keq for the reaction NOBr(g) NO(g) + 1/2 Br₂(g)? = 2.12 (b) What is the value of Keq for the reaction 2 NO(g) + Br₂(g) = 2 NOBr(g)? Keq=0.944 NO(g) + 1/2 Br₂(g) = NOBr(g) |x Keq=1.06 (c) What is the value of Keq for the reaction 2 NOBr(g) = 2 NO(g) + Br₂(g)? XH3C. (k) Zn/CH;COOH > 1Q + 1R heat H3C
- Ammonium sulfate, (NH,),SO4, is used as a fire retardant and wood preservative; it is prepared industrially by the highly exothermic reaction of gaseous ammonia with sulfuric acid: 2 NH, (g) + H,SO,(aq)→ (NH, ),SO, (s) The value of AH°, ammonium sulfate (in kilojoules per mole). is -179.4 kJ/g H, SO. Use the data in Table T1 to calculate the standard enthalpy of formation of rxnAt 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 =Carbon dioxide from the atmosphere "weathers," or dissolves, limestone (CaCO3) by the reaction CACO3(8) + CO2(9) + H2O(1) → Ca²+ (aq) + 2HCO3¯(aq) Obtain AH° for this reaction using the following data: AH;(CaCO3(8)) = –1206.9 kJ/mol AH;(CO2(9)) = -393.5 kJ/mol AH;(H2O(1)) = –285.8 kJ/mol AH;(Ca²+ (ag) -542.8 kJ/mol AH;(HCO3¯(aq)) = -692.0 kJ/mol ΔΗ kJ %3D
- 3.2 The standard Gibbs energy of formation of H20 at 25.0 °C, 4G, is -228.57 kJ.mot', for a standard state of 1 atm. The reaction is: 2 H30 (g) - O (g) + 2H, (g) (a) Calculate 4 G° (kJ.mol) for the above reaction. (b) Calculate the value of the equilibrium constant, K, for the above reaction. (c) Calculate the value of K at 5 atm.At -179 °C, Keq = 28.7 for the reaction: (a) What is the value of Keq for the reaction NOBr(g) = NO(g) + 1/2 Br₂(9)? Keq = (b) What is the value of Keq for the reaction 2 NO(g) + Br₂(g) = 2 NOBr(g)? Keq = (c) What is the value of Keq for the reaction 2 NOBr(g) 2 NO(g) + Br₂(g)? Keq = NO(g) + 1/2 Br₂(g) = NOBr(g)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?
- 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 -0.2079b) 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 -0.2079When 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 kJmol1