At -5.58 °C the concentration equilibrium constant K =7.3 × 10 for a certain reaction.Here are some facts about the reaction:. If the reaction is run at constant pressure, 113. kJ/mol of heat are released.The net change in moles of gases is 2.•The constant pressure molar heat capacity C= 2.78 J-mol ¹.K™!Using these facts, can you calculate Kat 4.9 °C?If you said yes, then enter your answer at right. Round it to2 significant digits.If you said no, can you at least decide whether Kat4.9 °C will be bigger or smaller than Kat -5.58 °C?Yes.O No.0Yes, and K will bebigger.Yes, and K will besmaller.No.

Answer: Given data: K1=7.3×10-5∆H=113kJ/molT1=-5.58°C = -5.58+273 K =267.42KT2=4.9°C=4.9+273 K=…

At -5.58 °C the concentration equilibrium constant K = 7.3 × 10 for a certain reaction. Here are some facts about the reaction: . If the reaction is run at constant pressure, 113. kJ/mol of heat are released. . The net change in moles of gases is 2. • The constant pressure molar heat capacity C= 2.78 J-mol¹ K Р Using these facts, can you calculate Kat 4.9 °C? If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether Kat 4.9 °C will be bigger or smaller than Kat -5.58 °C? Yes. O No. 0 Yes, and K will be bigger. Yes, and K will be smaller. No.

At -5.58 °C the concentration equilibrium constant K = 7.3 × 10 for a certain reaction. Here are some facts about the reaction: . If the reaction is run at constant pressure, 113. kJ/mol of heat are released. . The net change in moles of gases is 2. • The constant pressure molar heat capacity C= 2.78 J-mol¹ K Р Using these facts, can you calculate Kat 4.9 °C? If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether Kat 4.9 °C will be bigger or smaller than Kat -5.58 °C? Yes. O No. 0 Yes, and K will be bigger. Yes, and K will be smaller. No.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 5RQ

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For the reaction BaCO3(s) BaO(s) + CO2(g), rG = +219.7 kJ/mol-rxn. Using this value and other data available in Appendix L, calculate the value of fG for BaCO3(s).
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
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?
Consider the reaction 2HCl(aq)+Ba(OH)2(aq)BaCl2(aq)+2H2O(l)H=118KJ Calculate the heat when 100.0 rnL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M Ba(OH)2 Assuming that the temperature of both solutions was initially 25.0C and that the final mixture has a mass of 400.0 g and a specific heat capacity of 4.18 J/C g, calculate the final temperature of the mixture.
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?
For the reaction TiCl2(s) + Cl2(g) TiCl4(), rG = 272.8 kj/mol-txn. Using this value and other data available in Appendix L, calculate the value of fG for TiCl2(s).
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
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.)
The formation of aluminum oxide from its elements is highly exothermic. If 2.70 g Al metal is burned in pure O2 to give A12O3, calculate how much thermal energy is evolved in the process (at constant pressure).
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