A chemical reaction has ( Delta H^{circ}=-5.7 mathrm{~kJ} mathrm{~mol}^{-1} ) and an equilibrium constant of 9.5 at ( T=298 mathrm{~K} ). Assuming that ( Delta H^{circ} ) is constant over the temperature range in question, what is the equilibrium constant at ( T=360.1 mathrm{~K} ) ?
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314 J/mol·K). Show more…
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The change in enthalpy $\left(\Delta H_{\mathrm{rxn}}^{\mathrm{p}}\right)$ for a reaction is $-25.8 \mathrm{~kJ} / \mathrm{mol} .$ The equilibrium constant for the reaction is $1.4 \times 10^{3}$ at $298 \mathrm{~K}$. What is the equilibrium constant for the reaction at $655 \mathrm{~K} ?$
The change in enthalpy $\left(\Delta H_{\mathrm{rxn}}^{\mathrm{r}}\right)$ for a reaction is $-25.8 \mathrm{kJ} / \mathrm{mol}$ . The equilibrium constant for the reaction is $1.4 \times 10^{3}$ at 298 $\mathrm{K}$ . What is the equilibrium constant for the reaction at 655 $\mathrm{K}$ ?
The change in enthalpy ( $\Delta H_{\mathrm{rxn}}^{\circ}$ ) for a reaction is $-25.8 \mathrm{~kJ} / \mathrm{mol}$. The equilibrium constant for the reaction is $1.4 \times 10^{3}$ at $298 \mathrm{~K}$. What is the equilibrium constant for the reaction at $655 \mathrm{~K}$ ?
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