Please answer Consider the following reaction at constant P. Use theinformation here to determine the value of ASurr at35°C. Predict whether or not this reaction will bespontaneous at this temperature.CH4(8) + 202(8) -> CO2{3) + 2H2O(1)AH°nn-890.4 kJASsurr = +25.44 kJ/K, reaction is spontaneous%3DASsurr = -25.44 kJ/K, reaction is spontaneous%3DO ASsurr = -2.23 kJ/K, reaction is non-spontaneous= + 2.23 kJ/K, reaction is spontaneousASsurrASsurr =+2.23 kJ/K, it is not possible to predict thespontaneity of this reaction without more information.%3DASurr +25.44 kJ/K, it is not possible to predict thespontaneity of this reaction without more information.ASaurr-2.23 kJ/K, it is not possible to predict thespontaneity of this reaction without more information.O ASurr-25.44 kJ/K, it is not possible to predict thespontaneity of this reaction without more information.

The reaction taking place is given as, => CH4 (g) + 2 O2 (g) -----> CO2 (g) + 2 H2O (l)…

Consider the following reaction at constant P. Use the information here to determine the value of ASurr at 35°C. Predict whether or not this reaction will be spontaneous at this temperature. CH4(8) + 202(s) -> CO2(3) + 2H2O(1) AH nn -890.4 kJ O ASsurr = +25.44 kJ/K, reaction is spontaneous %3D ASurr = -25.44 kJ/K, reaction is spontaneous %3D O ASsurr = -2.23 kJ/K, reaction is non-spontaneous %3D ASqurr = + 2.23 kJ/K, reaction is spontaneous O ASsurr = +2.23 kJ/K, it is not possible to predict the spontaneity of this reaction without more information. %3D O ASurr+25.44 kJ/K, it is not possible to predict the spontaneity of this reaction without more information. ASsurr - -2.23 kJ/K, it is not possible to predict the spontaneity of this reaction without more information. O ASsurr-25.44 kJ/K, it is not possible to predict the spontaneity of this reaction without more information.

Consider the following reaction at constant P. Use the information here to determine the value of ASurr at 35°C. Predict whether or not this reaction will be spontaneous at this temperature. CH4(8) + 202(s) -> CO2(3) + 2H2O(1) AH nn -890.4 kJ O ASsurr = +25.44 kJ/K, reaction is spontaneous %3D ASurr = -25.44 kJ/K, reaction is spontaneous %3D O ASsurr = -2.23 kJ/K, reaction is non-spontaneous %3D ASqurr = + 2.23 kJ/K, reaction is spontaneous O ASsurr = +2.23 kJ/K, it is not possible to predict the spontaneity of this reaction without more information. %3D O ASurr+25.44 kJ/K, it is not possible to predict the spontaneity of this reaction without more information. ASsurr - -2.23 kJ/K, it is not possible to predict the spontaneity of this reaction without more information. O ASsurr-25.44 kJ/K, it is not possible to predict the spontaneity of this reaction without more information.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter17: Chemcial Thermodynamics

Section: Chapter Questions

Problem 17.109QE: Chemists and engineers who design nuclear power plants have to worry about high-temperature...

See similar textbooks

Similar questions

Many plastic materials are organic polymers that contain carbon and hydrogen. The oxidation of these plastics in air to farm carbon dioxide and water is a spontaneous process; however, plastic materials tend to persist in the environment. Explain.
What types of experiments can be carried out to determine whether a reaction is spontaneous? Does spontaneity have any relationship to the final equilibrium position of a reaction? Explain.
Consider two processes: sublimation of I2(s) and melting of I2(s) (Note: the latter process can occur at the same temperature but somewhat higher pressure). I2(s)I2(g)I2(s)I2(l) Is S positive or negative in these processes? In which of the processes will the magnitude of the entropy change be greater?
On the basis of your experience, predict which of the following reactions are spontaneous. (a) CO2(s)CO2(g) at 25°C (b) NaCl(s)NaCl(l) at 25°C (c) 2NaCl(s)2Na(s)+Cl2(g) (d) CO2(g)C(s)+O2(g)
In a spontaneous process, S(universe) is (a) 0 (b) = 0 (c) 0
The reaction CO2(g)+H2(g)CO(g)+H2O(g) is not spontaneous at room temperature but becomes spontaneous at a much higher temperature. What can you conclude from this about the signs of H and S , assuming that the enthalpy and entropy changes are not greatly affected by the temperature change? Explain your reasoning.
Given that H f for HF(aq) is -320.1 kJ/mol and S for HF(aq) is 88.7 J/mol K, find Ka for HF at 25C.
In the thermodynamic definition of a spontaneous process, why is it important that the phrase “continuous intervention” be used rather than just “intervention?”
When ammonium chloride is added to water and stirred, it dissolves spontaneously and the resulting solution feels cold. Without doing any calculations, deduce the signs of G, H, and S for this process, and justify your choices.
Explain why absolute entropies can be measured.
Show by calculation, using Appendix 1, whether dissolving lead(II) chloride PbCl2(s)Pb2+(aq)+2Cl(aq) is spontaneous at 25C (a) when [ Pb2+ ]=1.0M;[ Cl ]=2.0M. (b) when [ Pb2+ ]=1.0105M;[ Cl ]=2.0105M.
For the reaction CH3OH(l)+32O2(g)2H2O(l)+CO2(g) the value of G is 702.2 kJ at 25C. Other data are as follows: Hf (kJ/mol) at 25C S (J/molK) at 25C CH3OH(l) 238.7 126.8 H2O(l) 285.8 70.0 CO2(g) 393.5 213.7 Calculate the standard entropy, S, per mole of O2(g).