b) Calculate the equilibrium constant and the reversed for the reaction: 2A + E >3 D + B given the following information Rxn 1: A +B >D+C Rxn 2: A + E >C + D + F Rxn 3: C + E > B K1 = 0.60 K2 = 0.20 K3 = 4.0 Rxn 4: F + C <>D + B+E K4 = 8.0 %3D
Q: When does the value of Q = K? %3D
A: Given-> Q=Kc
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- In the synthesis of hydrocarbons, the carbon source is carbon dioxide. Although the CO2 concentra?on in the atmosphere raises at a drama?c speed, point sources are probably the easier sources for a PtX process. Iden?fy 3 possible point sources, explain why CO2 is formed and what challenges each of the three CO2 streams presentsA reaction mixture (mixture 1) at 298 K has a N2O4(g) partial pressure of 0.1 bar anda NO2(g) partial pressure of 0.05 bar. Calculate the reaction Gibbs energy (∆??) formixture 1 at 298 K. A second reaction mixture (mixture 2) is prepared at 298 K with a N2O4(g) partialpressure of 0.05 bar and a NO2(g) partial pressure of 0.10 bar. (i) Calculate the reaction Gibbs energy (∆??) for mixture 2 at 298 K. (ii) Comment on the spontaneity of the forward reaction for mixture 1 and mixture 2.Support your answer with the values of ∆?? calculated for the two mixtures. please give solution and answerBy the use of Henderson Hasselbalch equation; pH = pKa + log{[acetate ion]/[acetic acid]} 4.5 = 4.75 + log{[0.10 M]/[acetic acid]} -0.25 = log{[0.10 M]/[acetic acid]} [Acetic acid] = 0.10 M/ 10-0.25 [Acetic acid] = 0.10 M/0.56 [Acetic acid] = 0.1786 M Moles of sodium acetate dissolved in 250 mL buffer solution = 0.10 M× (250mL/1000mL) × 1L = 0.025 mol Weight (w) of sodium acetate (purity 100%) dissolved to prepare 250 mL of solution with buffer concentration of 0.10 M is calculate as follow; w100% = 0.025 mol × 82.0343 g/mol = 2.051 g Weight (w) of sodium acetate (purity 99%) is calculate as follow; w99% = 2.051 g× (100/99) = 2.072 g What was the volume of 6.12 M acetic acid HC2H3O2 needed to prepare the 250 mL acetic acid/acetate ion buffer solution required in this part? Show your calculations.
- Calculate the standard reaction enthalpy in J/mol at 315 K for the reaction A+B<-> AB with equilibrium constant expressed as In K= A + B/T +C/T2 at 150K to 1500K, where A = 1.25, B = -630.885 K, C = 2.371x105K2The reaction A(g) + B(g) ↔ C(g) + D(g) has ΔGrxn° = -28.62 kJ mol-1 and Kp = 0.63 at 980 °C. A rigid cylinder at that temperature contains 1.2 atm of A, 0.20 atm of B, 0.30 atm of C, and 0.27 atm of D. What is the reaction Gibbs energy?Hexanoic acid was added to an immiscible biphasic solvent system, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D2) of hexanoic acid in water with respect to CCl4.
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