Search for question
Question
1. Consider the following equilibrium system: \mathrm{C}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})=\quad \Delta H_{\mathrm{r}}^{\circ}=+120 \mathrm{~kJ} Indicate the shift in equilibrium, if any, for each of the following scenarios: a) Adding CO2(g) b) Adding C c)
Lowering the temperature d) Increasing pressure e) Adding a catalyst
Fig: 1
Fig: 2
Fig: 3
Fig: 4
Fig: 5
Fig: 6
Fig: 7
Fig: 8
