2SO2(g) + O2(g) ⇄ 2SO3(g), ΔH = −395.7 kJ mol−1. In the reaction above, the concentration of SO3(g) can be increased by
Decreasing the pressure
Decreasing the temperature
Increasing the temperature
Adding a catalyst
The minimum amount of energy required for a reaction to take place is
Lattice energy
Ionization energy
Activation energy
Kinetic energy
In the graph above, the activation energy of the catalyzed reaction is
100 kJ
300 kJ
250 kJ
200 kJ
3Fe(s) + 4H2O(g) ⇄ Fe3O4(s) + 4H2(g). The equilibrium constant, K, of the reaction above is represented as
\(\dfrac{[\mathrm{Fe_3O_4}][\mathrm{H_2}]}{([\mathrm{Fe}][\mathrm{H_2O}])}\)
\(\dfrac{[\mathrm{H_2O}]^{4}}{[\mathrm{H_2}]^{4}}\)
\(\dfrac{[\mathrm{H_2}]^{4}}{[\mathrm{H_2O}]^{4}}\)
\(\dfrac{[\mathrm{Fe}]^{3}[\mathrm{H_2O}]^{2}}{([\mathrm{Fe_3O_4}][\mathrm{H_2}]^{4})}\)
Which of the following compounds is a neutral oxide?
Carbon(IV) oxide
Sulphur(VI) oxide
Sulphur(IV) oxide
Carbon(II) oxide
