CO(g) + H\(_2\)O(g) \(\to\) \(CO_{2g}\) + H\(_2\)(g) \(\Delta\)H = - 4100J. Which of the following factors favour the formation of hydrogen in the above reaction? i. high pressure. ii. low pressure iii. high-temperature iv. use of excess steam
i, iii and iv
iii only
ii, iii and i
iv only
Explanation
Video Explanation
No video available
Post your Contribution
Discussions (4)
COg + h2Og --->CO2g +h2g ∆h=-4100j
The number of moles of gases on the left hand side is same as that on the right hand side (which is 2 on both sides)
Therefore, pressure won't have an effect on the forward or backward reaction
Since the forward reaction is exothermic,it will proceed at low temperature
Only using excess steam will have on effect on the forward reaction
Steam Concentration (iv): Adding excess steam (a reactant) increases the concentration of reactants. According to Le Chatelier's Principle, the system shifts to the right to consume the excess, thereby favouring the formation of hydrogen.
