Dd.57. Consider the chemical reaction and thermochemical information and initial partial pressures of the reaction components given below:CH3OH(g) + HCI(g) = CH3CI(g) + H₂O(g)AH° (kJ/mol)5° (J mol-¹ K-¹)CH3OH -201.50239.80#]!186.90234.6188.84HCI-92.31CH3CI -81.9H₂O-241.83P (atm)0.5400.8585.082.87Determine AG (in kJ) for this reaction at 400.4 K. Assume AH°f and Sº do not vary as a function of temperature. Report your answer to two decimal places in standard notation (i.e. 123.45 kJ).

Consider the chemical reaction and thermochemical information and initial partial pressures of the reaction components given below: CH3OH(g) + HCl(g) = CH3CI(g) + H₂O(g) CH3OH -201.50 239.80 # -92.31 186.90 CH3CI -81.9 234.6 H₂O -241.83 188.84 HCI AH/° (kJ/mol) 5° (J mol-¹ K-¹) P (atm) 0.540 0.858 5.08 2.87 Determine AG (in kJ) for this reaction at 400.4 K. Assume AHºf and Sº do not vary as a function of temperature. Report your answer to two decimal places in standard notation (i.e. 123.45 kJ).

Consider the chemical reaction and thermochemical information and initial partial pressures of the reaction components given below: CH3OH(g) + HCl(g) = CH3CI(g) + H₂O(g) CH3OH -201.50 239.80 # -92.31 186.90 CH3CI -81.9 234.6 H₂O -241.83 188.84 HCI AH/° (kJ/mol) 5° (J mol-¹ K-¹) P (atm) 0.540 0.858 5.08 2.87 Determine AG (in kJ) for this reaction at 400.4 K. Assume AHºf and Sº do not vary as a function of temperature. Report your answer to two decimal places in standard notation (i.e. 123.45 kJ).

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 23Q: Monochloroethane (C2H5Cl) can be produced by the direct reaction of ethane gas (C2H6) with chlorine...

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Some water is placed in a coffee-cup calorimeter. When 1.0 g of an ionic solid is added, the temperature of the solution increases from 21.5C to 24.2C as the solid dissolves. For the dissolving process, what are the signs for Ssys, Ssurr, and Suniv?
Given the following information at 25C, calculate G at 25C for the reaction 2A(g)+B(g)3C(g) Substance Hf(kJ/mol) S(J/molK) A(g) 191 244 B(g) 70.8 300 C(g) 197 164 a 956 kJ b 956 kJ c 346 kJ d 346 kJ e 1.03 103 kJ
Silver carbonate, Ag2CO3, is a light yellow compound that decomposes when heated to give silver oxide and carbon dioxide: Ag2CO3(s)Ag2O(s)+CO2(g) A researcher measured the partial pressure of carbon dioxide over a sample of silver carbonate at 220C and found that it was 1.37 atm. Calculate the partial pressure of carbon dioxide at 25C. The standard enthalpies of formation of silver carbonate and silver oxide at 25C are 505.9 kJ/mol and 31.05 kJ/mol, respectively. Make any reasonable assumptions in your calculations. State the assumptions that you make, and note why you think they are reasonable.
9.96 Most first aid "cold packs" are based on the endothermic dissolution of ammonium nitrate in water: NH4NO3(s)NH4+(aq)+NO3(aq) H= 25.69 kJ A particular cold pack contains 50.0 g of NH4NO3 and 125.0 g of water. When the pack is squeezed, the NH4NO3dissolves in the water. If the pack and its contents are initially at 24.0°C, what is the lowest temperature that this bag could reach? (Assume that the ammonium nitrate solution has a specific heat of 4.25J g-l K-l, and that the heat capacity of the bag itself is small enough to be neglected.)
Consider the reaction H2(g)+Br2(g)2HBr(g) where H = 103.8 kJ/mol. In a particular experiment, equal moles of H2(g) at 1.00 atm and Br2(g) at 1.00 atm were mixed in a 1.00-L flask at 25C and allowed to reach equilibrium. Then the molecules of H2 at equilibrium were counted using a very sensitive technique, and 1.10 1013 molecules were found. For this reaction, calculate the values of K, G, and S.
9.83 A student performing a calorimetry experiment combined 100.0 mL of 0.50 M HCl and 100.0 mL of 0.50 M NaOH in a coffee cup calorimeter. Both solutions were initially at 20.0°C, but when the two were mixed, the temperature rose to 23.2°C. (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 mL of 0.50 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCl and 100.0 mL of 1.00 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why?
What determines Ssurr for a process? To calculate Ssurr at constant pressure and temperature, we use the following equation: Ssurr = H/T. Why does a minus sign appear in the equation, and why is Ssurr inversely proportional to temperature?
What is the difference between S, S , and S 298 for a Chemical change?
Why is it usually easier to use G to determine the spontaneity of a process rather than Su ?
When a fossil fuel burns, is that fossil fuel the system? Explain your answer.
Given the thermochemical expression CaO(s) + 3C(s) CaC2(s) + CO(g) rH = 464.8 kJ/mol calculate the quantity of energy transferred when (a) 34.8 mol CO(g) is formed by this reaction. (b) A metric ton (1000 kg) of CaC2(s) is manufactured. (c) 0.432 mol carbon reacts with CaO(s).
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.

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