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![For the reaction (NH4)2S (s) = N2 (g) + H2S (g) + 3 H2 (g), the expression for Ke Is
Kc = [N₂][H₂S][H₂]³
Kc
[N₂][H₂S][H₂]
[(NH4)2S]
Kc = [(NH4)2S]
Кс
Kc
[N₂] + [H₂S] + [H₂]³
[(NH4)zS]
=
[N₂] [H₂S] [H₂]³
[(NH4)2S]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8afd3e8f-293d-45a8-8702-4440333f37df%2Fd0e1bcba-9465-4fe0-afe8-bcf145a24b71%2Flk53aka_processed.jpeg&w=3840&q=75)
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- Given ΔHoformation, (CO2(g)) = -395,51 kJ/mol ΔHoformationCp(CO2) = 37.11J/Kmol-1, ΔHoformationCp(O2) = 29.355 J/Kmol-1, and ΔHoformationCp(C) = 8.527J/Kmol-1, T2 = 125o, T1 = 20oC. Find ΔH2o for the reaction: C(s) + O2(g)-à CO2(g), when Cp is independent of T.Explain the difference between Kf and Ksp.Write the expression for Keq for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous. H2(g) + I2(g) 2 HI(g) Keq = 2 PHI / (PH2 PI2) Keq = PH2 PI2 / 2 PHI Keq = PH2 PI2 / PHI2 Keq = PHI2 / (PH2 PI2)
- Consider the reaction NH3(aq) + H2O(l) NH4+(aq) + OH–(aq). Kb for NH3 is 1.8 x 10–5 at 25°C. What is Ka for the NH4+ion at 25°C?Nitrogen dioxide is a toxic pollutant that contributes to photochemical smog. One way it forms is through the following sequence: (1) N2(g) + O2(g) ↔ 2NO(g) Kc1 5 4.3x1025 (2) 2NO(g) + O2(g) ↔ 2NO2(g) Kc2 5 6.4x109 (a) Show that the overall Qc for this reaction sequence is the same as the product of the Qc expressions for the individual reactions. (b) Given that both reactions occur at the same temperature, find Kc for the overall reaction.A research group discovers a new version of happyase, which they call happyase*, that catalyzes the chemical reaction The researchers begin to characterize the enzyme. a)In the first experiment, with [Et] at 4 nM, they find that the Vmax is 1.6 μM s-1. Based on this experiment, what is the kcat for happyase*? (Include appropriate units.) b)In another experiment, with [Et] at 1 nM and [HAPPY] at 30 μM, the researchers find that V0300 nM s-1. What is the measured Km of happyase* for its substrate HAPPY? (Include appropriate units.) c)Further research shows that the purified happyase* used in the first two experiments wasactually contaminated with a reversible inhibitor called ANGER. When ANGER is carefully removed from the happyase* preparation, and the two experiments repeated, the measured Vmax in (a) is increased to 4.8 μM s-1, and the measured Km in (b) is now 15 μM. For the inhibitor ANGER, calculate the values of αand α’.
- What is the std heat of reaction at 800 degrees celsius (1073.15K) for a complete combustion of liquid ethanol (C2H5OH) to carbon dioxide (CO2) and liquid water (H2O)?The reaction is carried out with [PCl5]i =0.40M at 25°C PCl5(g)⇌PCl3(g)+Cl2(g) K=0.00105 Use the small x approximation and "test x." Report the percent, to two decimal places, when testing x.Use the standard reaction energies given below to determine DeltaG^°rxn for the following reaction: 2XO2(g) —> 2XO(g) + O2(g) From the standard reaction energy of X2(g) + O2 —> 2XO(g) DG^°= 155.52 Kjxmol-1 X2(g) + 2O2 —> 2XO2(g) DG^°= 168.55 Kjxmol-1 Given answer in Kj/mol. Give answer to two decimal places.
- A solution of 710.5 ml of 0.00056 M A3B2 is mixed with a solution of 502.5 ml of 0.00044 M C1D2. Find the value of pQ (the minus log of Q) for the formation of C3B2.Consider the following ∆H°f and S° at 300K: Chemical species ∆H°f S° (in J/mol. K) C2H6(g) -83.7 229.6 H2O(g) -241.82 188.83 CO2(g) -110.53 199.42 O2(g) 0 205.138 A) Determine the ∆H°rnx of the following reaction at 300K (in kJ/mol) C2H6(g) + 7/2 O2(g) → 3 H2O (g) + 2 CO2(g) B) Determine the ∆S°rnx of the following reaction at 300K (in kJ/mol) C2H6(g) + 7/2 O2(g) → 3 H2O (g) + 2 CO2(g) C) Determine the ∆G°rnx of the following reaction at 300K (in kJ/mol) C2H6(g) + 7/2 O2(g) → 3 H2O (g) + 2 CO2(g) Show the process and calculationsUrea, CO(NH2)2 is slowly converted to ammonia (NH3) at 25.0 °C according to the following reaction. CO(NH2)2 (aq) + H2O (l) → CO2 (aq) + NH3 (aq) The following data were obtained for this reaction Compound ∆H°f (kJ/mol) CO(NH2)2 (aq) -319.2 H2O (l) -412.9 CO2 (aq) -285.8 NH3 (aq) -80.3 A) Calculate ∆H° for the reaction B) What type of reaction is this (endothermic, exothermic, neither) c)Calculate the change in enthalpy (∆H°) for the decomposition of 2.00 g of urea.