Consider the following reaction at 298 R. 2 SO₂(g) + O₂(g) → 2 SO 3(9) An equilibrium mixture contains O₂(g) and SO3(9) at partial pressures of 0.57 atm and 2.5 atm, respectively. Using data from the Thermodynamic Data table, determine the equilibrium partial pressure of SO₂ in the mixture. atm Will this reaction be most favored at a high or a low temperature, assuming standard conditions? O high temperature O low temperature

Consider the following reaction at 298 R. 2 SO₂(g) + O₂(g) → 2 SO 3(9) An equilibrium mixture contains O₂(g) and SO3(9) at partial pressures of 0.57 atm and 2.5 atm, respectively. Using data from the Thermodynamic Data table, determine the equilibrium partial pressure of SO₂ in the mixture. atm Will this reaction be most favored at a high or a low temperature, assuming standard conditions? O high temperature O low temperature

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 78E: Consider the following reaction at 298 K: 2SO2(g)+O2(g)2SO3(g) An equilibrium mixture contains O2(g)...

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Consider the following reaction at 298 K: 2SO2(g)+O2(g)2SO3(g) An equilibrium mixture contains O2(g) and SO3(g) at partial pressures of 0.50 atm and 2.0 atm, respectively. Using data from Appendix 4, determine the equilibrium partial pressure of SO2 in the mixture. Will this reaction be most favored at a high or a low temperature, assuming standard conditions?
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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 decomposition of diamond to graphite [C(diamond) C(graphite)] is thermodynamically favored, but occurs slowly at room temperature. a. Use fG values from Appendix L to calculate rG and Keq for the reaction under standard conditions and 298.15 K. b. Use fH and S values from Appendix L to estimate rG and Keq for the reaction at 1000 K. Assume that enthalpy and entropy values are valid at these temperatures. Does heating shift the equilibrium toward the formation of diamond or graphite? c. Why is the formation of diamond favored at high pressures? d. The phase diagram shows that diamond is thermodynamically favored over graphite at 20,000 atmospheres pressure (about 2 GPa) at room temperature. Why is this conversion actually done at much higher temperatures and pressures?

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