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- Calculate ΔG°rxn, ΔH°rxn, and ΔS°rxn of the following reaction: 2O3(g) -> 3O2(g)Calculate ΔHrxn for the reaction using the following data. Target Reaction: WO3 (s) + 3H2 (g) → W (s) + 3H2O (g) Reaction 1: W (s) + 3/2 O2 (g) → WO3 (s) ΔH = ‒842.7 kJ Reaction 2: H2 (g) + 1/2 O2 (g) → H2O (g) ΔH = ‒238.9 kJ Group of answer choices A)‒2289.2 kJ B)126 kJ C)‒1559.4 kJ D)1559.4 kJ E)‒1081.6For the reaction given below, the arrhenius actication energy is 15.5 kj.mol-1. Find Δ≠ H0
- Which reaction do you expect to have the smallest orientation factor?(a) H(g) + I(g)¡HI(g)(b) H2(g) + I2(g)¡2 HI(g)(c) HCl(g) + HCl(g)¡H2(g) + Cl2(g)What is the free energy change for the reaction below? 2VO2+(aq) + 4H+(aq) + Ni(s) ® 2VO2+(aq) + 2H2O(l) + Ni(s) E� = 1.23V 118.68 kJ 237.35 kJ -237.35 kJ -118.68 kJWhat is the value of the rate law constant for the reaction shown below? 1. -1.9 x 10^4 2. +1.9 x 10^4 3. -5.2 x 10^-5 4. +5.2 x 10^-5 5. +6.2
- Find ∆H◦, ∆S◦, and ∆G◦ for each of the following reactions. Calculate ∆H◦ − T ∆S◦ and compare it with ∆G◦ to check the consistency of the dataa. CaCO3(calcite,s) + HCl(g) = CaCl2(s) + H2O(l) + CO2(g)b. CH4(g) + Cl2(g) = CHCl3(l) + HCl(gI am having trouble solving this problem: The isomerization reaction shown here is temperature dependent. Given the starting material and the Kc, identify the number of molecules of reactant and product observed for each reaction. A=30 Kc: 5 Kc: .5 How would I set this up to solve the problem? I just need some direction I know Kc= B/A but it isn't working outA reaction between the substances A and B gives the following data: 3A + 2B->2C + D [A] (mol/L) [B] (mol/L) rate apperance of C (mol/L-hr) 1.0x10^-2 1.0 0.3x10^-6 1.0x10^-2 3.0 8.1x10^-6 2.0x10^-2 3.0 3.24x10^-5 2.0x10^-2 1.0 1.20x10^-6 3.0x10^-2 3.0 7.3x10^-5 Use the data above to calculate the reaction order with respect of A and B, the rate law, and the rate constant.
- For the following reaction: 2 SO2(g) + O2(g) ⇌ 2 SO3(g) Kc = 1.6 × 104 [SO3]= 2.5M [O2]=0.0035M Calculate [SO2]eq Group of answer choicesCH4(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 = 2.00M10. The conversion of reactant I to product G is preferred at _____ temperature and is under ______ control. a. low, kinetic b. low, thermodynamic c. high, kinetic d. high, thermodynamic 11. The conversion of reactant I to product H is preferred at _____ temperature and is under ______ control. a. low, kinetic b. low, thermodynamic c. high, kinetic d. high, thermodynamic