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Calculate delt G for
a.) CH3NH2(aq) + H2O (l) -> CH3NH3+ (aq) + OH-(aq)
T= 25C
kp= 4.4x 10-4
b.) Pbl2(s) + Pb2+(aq) +2I-(aq)
T= 25C
Kp= 8.7x10-9
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- Using the following data to calculate Ksp for PbSO4. ε° PbO2 + 4H+ + SO42- + 2e-→ PbSO4(s) + 2H2O +1.69 PbO2 + 4H+ + 2e-→ Pb2+ + 2H2O +1.46 (Hint: Write the general reaction for PbSO4) a. 1.7 × 10-8 b. 5.9 × 107 c. 2.5 × 10-107 d. 4.0 × 10106 e. 3.4 × 10-18CaCO3(s)<->Ca^2+(aq)+CO3^2-(g). write down Ksp for this reactionCalculate ΔSsys° (J/K) for the catalytic hydrogenation of acetylene to ethane: C2H2(g) + H2(g) → C2H4(g) Substance S° (J/K·mol) C2H2(g) 200.8 H2(g) 130.58 C2H4(g) 219.4
- Ff.24. With explanation ......What is ΔSsurr for a reaction at 19 °C with ΔHsys = -7.3 kJ mol-1 ? Express your answer in J mol-1 K-1 to at least two significant figures.Determine the Ksp of the following reactions. a. NaC2H3O2 Na+ + C2H3O2- b. HBr H+ + Br c. Zn(OH)2 Zn+2 + 2HO- d. PbCl2 Pb+2 + 2Cl- e. SnSO4 Sn+2 + SO4-
- 1. 2A + 4C → 3B (rate constant = k1) 2. 5A + C → 2D + E (rate constant = k2) 3. E → F + 4G (rate constant = k3) 4. 2D + B → G (rate constant = k4) Identify the intermediate(s) (MULTIPLE ANSWERS POSSIBLE) a.B b.F c.A d.E e.C f.D g.G1. Given the SEPs: Br2(l) + 2e- ↔ 2Br- E0 = 1.078 V Br2(aq) + 2e- ↔ 2Br- E0 = 1.098 V a. Calculate the Keq for the reaction: Br2(l) ↔ Br2(aq)For the reaction 2Na (g) Na2 (g) the following values of K have been determined (C. T. Ewinget al., J. Chem. Phys. 1967, 71, 473):T (K) K900 1.321000 0.471100 0.211200 0.10From these data, estimate rxnH° for the reaction.
- How would the equilibrium be affected in regards to the value of Qc or Kc for each of the following conditions?: Fe3+ (aq) + SCN- (aq) ⇌ FeSCN2+ (aq) Adding KSCN (aq) Adding Fe(NO3) (aq) Adding NaF (s) Placing the solution into a hot water bath Placing the solution into an ice bath (To whom this may concern, Could you at least explain one as simply as possible so I'm able to understand the others enough to explain them myself? Thanks in anvance!)Rate = -(Delta[RCl])/Delta t andln[RCl]t=-k*t+ln[RCl]0 < [R-Cl]-time equation Test tube A = 0.30 of 0.10M NaOH(aq), 6.70ml DI H2O & 1 drop of bromophenol bue Test Tube B = 3.00M of 0.10M R-CL in acetone. Mix together in 3 water baths Bath A Trial 1= 20C, 53.6s Trial 2= 20C, 49s for color to changeBath B Trial 1= 32C, 18s Trail 2= 32C, 20s Bath C Trial 1= 10C, 204s Trial B= 10C, 200sQ.6 Rearrange the Arrhenius equation into a linear form relating k and TQ.6a To determine Ea, a graph of (xaxis) ____ (in units of ___) vs. (yaxis) ____ needs to be made. This will yioeld a _____ line with a slope = ____ Q.6b enter values used in the table Q.6c Determine the exp. values of Ea with correct sig figs and unitsWhich of the following is a spontaneous reaction.? a. Rxn with ΔH =- 10Kj/mol ΔS= -5J/mol T= 300K b. NaCl +H20 -> NaOH + HCl 25C c. H20(l) -> H2O(s) Temp: 25C d. Dissolution of 100g of solid sugar in 100 mL ice tea. Consider following reaction: HgO (s) -> Hg(l) + ½ O2 (g) Delta H = +90.7 kj/mol. What quantity of heat in kj/mol is required to produce one mole HgO? Write your answer without units. Given the following data 2ClF(g) + O2(g) --> Cl2O(g) + F2O (g) Delta H= 167.4 kJ I 2ClF3(g) + 2O2(g) --> Cl2O(g) + 3F2 O (g) Delta H= 341.4 kJ II 2 F2(g) + O2(g) ---> 2F2O (g) Delta H= -43.4 kJ III Calculate the delta H in kJ for below reaction: ClF(g) + F2(g) ---> ClF3(g)