A chemical engineer is studying the two reactions shown in the table below.
In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 25.0 °C and constant total pressure.
Then, she measures the reaction enthalpy $\Delta H$ and reaction entropy $\Delta S$ of the first reaction, and the reaction enthalpy $\Delta H$ and reaction free energy $\Delta G$ of the
second reaction. The results of her measurements are shown in the table.
Complete the table. That is, calculate $\Delta G$ for the first reaction and $\Delta S$ for the second. (Round your answer to zero decimal places.) Then, decide whether, under
the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous
because the system is at equilibrium.
$\Delta H = 1353 \text{ kJ}$
$\Delta S = 4538 \frac{J}{K}$
$\Delta G = \text{ } \text{ kJ}$
$2CO_2(g) + 4H_2(g) \rightarrow 2CH_3OH(g) + O_2(g)$
Which is spontaneous?
$\circ$ this reaction
$\circ$ the reverse reaction
$\circ$ neither
$\Delta H = -70 \text{ kJ}$
$\Delta S = \text{ } \frac{J}{K}$
$\Delta G = 22 \text{ kJ}$
$TiCl_4(g) + 2H_2O(g) \rightarrow TiO_2(g) + 4HCl(g)$
Explanation
Check
