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![For the reaction below, what is A[CH,O]/At with respect to
A[O2]/A?
C,H,(g) + O3(g) → 2CH,0(g) + ½O2(g)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4cb71868-6f58-4dcf-8038-c59a628909aa%2Fc370aeb3-d201-4a56-a4a1-80362771e83c%2Fuinfly7_processed.png&w=3840&q=75)
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- 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+B➡️P t=0 :C(A)=C(B) t=500sec 20% of react t=? Sec 60% of complQ26 (D) Explain with figure the role of a catalyst on speed of areaction.
- Determine the ΔSsystem given the reaction. C6H12O6(s) + O2(g) ----> CO2(g) + H2O(l).Conventional equilibrium considerations do not apply when a reaction is driven by light absorption and the steady-state concentration of products and reactants might differ significantly from equilibrium values. For instance, suppose the reaction A → B is driven by light absorption, and that its rate is Ia, but that the reverse reaction B → A is bimolecular and second order with a rate kr[B]2. What is the stationary state concentration of B? Why does this ‘photostationary state’ differ from the equilibrium state?For a reaction with DH= 10 kJ/mol and DS =100J/K·mol, the DGis ______ at 25°C.A)-29790J/mol B)-19800J/molC)7500J/mol D)-7kJ/mol E)7kJ/mol
- rate law is r=k[ClO2][OH-]CH4(g) + 2O2(g) ↔ CO2(g) + 2H2O(g) Identify which way the reaction above would shift given the following initial conditions. You must prove it using math. [CH4]0 = 1.00M [O2]0 = 1.00M [CO2]0 = 2.00M [H2O]0 = 2.00MConsider the following mechanism: 1) Br2(g) = 2Br(g) Kc1 = 2.2 x 10^-3 2) Br(g) + H2(g) = HBr(g) + H(g) Kc2 = 7.5 x 10^6 3) H(g) + Br(g) = HBr(g) Kc3 = 350 calculate Kc for the overall reaction
- As described in Problem P17D.5, reaction with the hydroxyl radical OH is the main path by which CH4 is removed from the lower atmosphere. T. Gierczak et al. (J. Phys. Chem. A 101, 3125 (1997)) measured the rate constants for the bimolecular gas-phase reaction CH4 + OH → CH3 + H2O and found A = 1.13 × 109 dm3 mol−1 s−1 and Ea = 14.1 kJ mol−1 for the Arrhenius parameters. (a) Estimate the rate of consumption of CH4 under the following conditions: take the average OH concentration to be 3.5 × 10−15 mol dm−3, that of CH4 to be 40 nmol dm−3, and the temperature to be −10 °C. (b) Estimate the global annual mass of CH4 consumed by this reaction (which is slightly less than the mass introduced to the atmosphere) given an effective volume for the Earth’s lower atmosphere of 4 × 1021 dm3.The value of ΔS° for the catalytic hydrogenation of acetylene to ethane, C2H2 (g) + 2H2 (g) → C2H6 (g) is __________ J/K∙ mol. A) -76.0 B) +440.9 C) -232.5 D) +232.5 E) +28.7What is the molecularity of the rate limiting step for the mechanism below? Step 1: H2O2 (aq) + I–(aq) → H2O(l) + OI–(aq) (slow)Step 2: H2O2 (aq) + OI–(aq) → H2O(l) + O2 (g) + I–(aq) (fast)