Phosgene is an organic chemical substance with the formula COCI2, which is a valued industrial intermediate for producing polycarbonate plastics and urethane. The typical synthesis of phosgene by carbon monoxide and chlorine gases is conducted between 50°C to 150° The chemical equation of the above reaction is written as: CO (g) + Cl2 (g) <---> COCI2 (g) a) When the equilibrium is reached at 100°C, the no. of moles of CO (g), Cl2 (g), and COCI2 (g) in a 1.0-L reactor are 8.68 × 10-2 ,9.16 x 10-2 , and 3.16, respectively. Calculate the equilibrium constant K at 100°C for the above reaction. [ Select ] b) Find the concentrations of all gases at equilibrium state if 10.00 mol of phosgene is decomposed in a 1.0 L container at 100°C. COCI2 (g) = [ Select ] mol/L CO (g : [ Select ] mol/L Cl2 (g = [ Select ] mol/L c) If the concentration of the reactant was doubled, what would happen to the equilibrium constant? [ Select ]

In the late eighteenth century Priestley prepared ammonia by reacting HNO3(g) with hydrogen gas. The thermodynamic equation for the reaction is HNO3(g)+4H2(g)NH3(g)+3H2O(g)H=637kJ (a) Calculate H when one mole of hydrogen gas reacts. (b) What is H when 10.00 g of NH3(g) are made to react with an excess of steam to form HN3(g) and H2 gases?

Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.

Monochloroethane (C2H5Cl) can be produced by the direct reaction of ethane gas (C2H6) with chlorine gas or by the reaction of ethylene gas (C2H4) with hydrogen chloride gas. The second reaction gives almost a 100% yield of pure C2H5Cl at a rapid rate without catalysis. The first method requires light as an energy source or the reaction would not occur. Yet G for the first reaction is considerably more negative than G for the second reaction. Explain how this can be so.

Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.

Silicon forms a series of compounds analogous to the al-kanes and having the general formula SinH2n+2. The first of these compounds is silane, SiH4, which is used in the electronics industry to produce thin ultrapure silicon films. SiH4(g) is somewhat difficult to work with because it is py-ropboric at room temperature—meaning that it bursts into flame spontaneously when exposed to air. (a) Write an equation for the combustion of SiH4(g). (The reaction is analogous to hydrocarbon combustion, and SiO2 is a solid under standard conditions. Assume the water produced will be a gas.) (b) Use the data from Appendix E to calculate ? for this reaction. (c) Calculate G and show that the reaction is spontaneous at 25°C. (d) Compare G for this reaction to the combustion of methane. (See the previous problem.) Are the reactions in these two exercises enthalpy or entropy driven? Explain.

Determine the standard free energy change, Gf, for the formation of S2-(aq) given that the Gf for. Ag*(aq) and Ag2S(s) are 77.1 kJ/mole and 395 kJ/mole respectively, and the solubility product for Ag2S(s) is 81051.

For the following reactions at constant pressure, predict if HE,HE,orH=E a. 2HF(g)H2(g)+F2(g) b. N2(g)+3H2(g)2NH3(g) c. 4NH3(g)+5O2(g)4NO(g)+6H2O(g)

5.11. Determine the numerical value of Q for the reaction conditions indicated.

Given the data in the table below, AHrxn for the reaction Ca(OH); + 2H;AsO4 → Ca(H;AsO4)2 + 2H;O is _ kJ. [A] -4219 (B] -130.4 [C] -4519 [D] -76.4 AH, (kJ/mol) -986.6|| Substance Ca(ОН), HASO, Ca(H;AsOa)2 -900.4 -2346.0 H;0 -285.9 O A В C D