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6)
delta Ho (Cl2) = 0 KJ/mol
delta Ho (Br-) = -121.55 KJ/mol
delta Ho (Br2) = 0 KJ/mol
delta Ho (Cl-) = -167.16 KJ/mol
deltar HO = delta Ho (Br2) + 2*delta Ho (Cl-) - delta Ho
(Cl2) + 2*delta Ho (Br-)
= 0 + 2* (-167.16) - 0 - 2*( -121.55)
= -334.32 + 243.1
= - 91.22 KJ/mol
Answer: - 91.22 KJ/mol
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Help w 6&7
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Help with both questions please!
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Can someone help me out with #7. The chart above states the chemicals being used. 6....
Can someone help me out with
#7. The chart above states the chemicals being used.
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Help with both questions please!
6. The following reaction takes place in a 1.00L vessel at 500°C 2 Hlig Hae late Equilibrium concentrations were found to be 1.76 mol/L HL 0.200 mol/L. Hy and 0.200 mol/Liina vessel. If an additional 0.500 mol of hydrogen iodide gas is introduced at the same temperature, what are the new concentrations of all gases once equilibrium has been reestablished? A) Use the given concentrations to calculate Ke B) After the addition of an 0.500...
Can someone help me out with
#7. The chart above states the chemicals being used.
6. Determine the equilibrium concentrations of each of using the table provided below (ICE table). Fill in all blank values concentrations of each of the reactants and products in solution B-5 [Fe3+] (SCN) [Fe(SCN)2+) Initial Concentration Change in Concentration 10.00091 12.1 E-4 T7.0x10-4 Equilibrium Concentration To 00090 1-2.1 E-4 16.9x16-4 +2.12 E-4 201810-9 7. What is the expression for the equilibrium expression for the reaction...
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