https://ejercicios-fyq.com/ Ejercicios Resueltos, Situaciones de aprendizaje y VÍDEOS de Física y Química para Secundaria y Bachillerato es SPIP - www.spip.net https://ejercicios-fyq.com/local/cache-vignettes/L144xH25/siteon0-da713.png?1758361862 https://ejercicios-fyq.com/ 25 144 https://ejercicios-fyq.com/Gibbs-free-energy-and-spontaneity-8296 https://ejercicios-fyq.com/Gibbs-free-energy-and-spontaneity-8296 2024-08-29T18:59:47Z text/html es F_y_Q Gibbs free energy Spontaneity SOLVED <p>The standard enthalpy of reaction between methane and dichlorine to produce chloromethane and hydrogen chloride is . Knowing the standard entropy change is , calculate the standard Gibbs free energy change at a given temperature, and determine if the process is spontaneous under these conditions.</p> - <a href="https://ejercicios-fyq.com/Thermodynamics" rel="directory">Thermodynamics</a> / <a href="https://ejercicios-fyq.com/Gibbs-free-energy" rel="tag">Gibbs free energy</a>, <a href="https://ejercicios-fyq.com/Spontaneity" rel="tag">Spontaneity</a>, <a href="https://ejercicios-fyq.com/SOLVED" rel="tag">SOLVED</a> <div class='rss_texte'><p>The standard enthalpy of reaction between methane and dichlorine to produce chloromethane and hydrogen chloride is <img src='https://ejercicios-fyq.com/local/cache-vignettes/L150xH20/58a2d546f6803730f6efe2b8d19092a4-01394.png?1733007203' style='vertical-align:middle;' width='150' height='20' alt="-114\ kJ\cdot mol^{-1}" title="-114\ kJ\cdot mol^{-1}" />. Knowing the standard entropy change is <img src='https://ejercicios-fyq.com/local/cache-vignettes/L182xH20/d1138ee893e0e8a0a67378b323d1fc3b-45e4e.png?1733007203' style='vertical-align:middle;' width='182' height='20' alt="11.1\ J\cdot K^{-1}\cdot mol^{-1}" title="11.1\ J\cdot K^{-1}\cdot mol^{-1}" />, calculate the standard Gibbs free energy change at a given temperature, and determine if the process is spontaneous under these conditions.</math></p></div> <hr /> <div <div class='rss_ps'><p>The reaction to be studied is: <br/> <br/> <img src='https://ejercicios-fyq.com/local/cache-TeX/8887882de9836064e56232b016ec4a6c.png' style="vertical-align:middle;" width="436" height="23" alt="\color[RGB]{2,112,20}{\textbf{\ce{CH4(g) + Cl2(g) -> CH3Cl(g) + HCl(g)}}}" title="\color[RGB]{2,112,20}{\textbf{\ce{CH4(g) + Cl2(g) -> CH3Cl(g) + HCl(g)}}}" /> <br/> <br/> The expression to calculate the Gibbs free energy is: <br/> <br/> <img src='https://ejercicios-fyq.com/local/cache-TeX/6630ed8319780bf0283f2ec4d878574c.png' style="vertical-align:middle;" width="222" height="20" alt="\color[RGB]{2,112,20}{\bm{\Delta G^0 = \Delta H^0 - T\Delta S^0}}" title="\color[RGB]{2,112,20}{\bm{\Delta G^0 = \Delta H^0 - T\Delta S^0}}" /> <br/> <br/> Simply substitute the values provided in the statement, considering that the enthalpy is given in kJ, and perform the calculation: <br/> <br/> <p class="spip" style="text-align: center;"><img src='https://ejercicios-fyq.com/local/cache-TeX/1177fa3a7f4b90b8ebf1d14a2b7118d5.png' style="vertical-align:middle;" width="619" height="47" alt="\Delta G^0 = - 114\cdot 10^3\ \frac{J}{mol} - 298\ \cancel {K}\cdot 11.1\ \frac{J}{\cancel {K}\cdot mol} = \fbox{\color[RGB]{192,0,0}{\bm{-1.17\cdot 10^5\frac {J}{mol}}}}" title="\Delta G^0 = - 114\cdot 10^3\ \frac{J}{mol} - 298\ \cancel {K}\cdot 11.1\ \frac{J}{\cancel {K}\cdot mol} = \fbox{\color[RGB]{192,0,0}{\bm{-1.17\cdot 10^5\frac {J}{mol}}}}" /></p> </math></p></div>