(a)[2]
Explain why this reaction is endothermic, using bond breaking and bond forming.
(b)[2]
Calculate the energy absorbed when $240\,\text{dm}^3$ of hydrogen, measured at room temperature and pressure, is produced.
(c(i))[2]
Predict, with a reason, how the equilibrium position changes when the pressure is increased at constant temperature.
(c(ii))[2]
Predict, with a reason, how the equilibrium position changes when the temperature is increased at constant pressure.
(d(i))[1]
Suggest one disadvantage of using this reaction as a hydrogen source.
(d(ii))[1]
Give one advantage of making hydrogen by reacting carbon with steam instead of using crude oil.