Consider reaction
S(s) + O2(g) - S02
State of so, in this reaction is
A. Liquid
B. Solid
C. Gaseous
D. All the three
Answers
Answer:
In the reaction, 2SO
2
(g)+O
2
(g)⇌2SO
3
(g)+Xcal most favourable conditions of temperature and pressure for greater yield of SO
2
are high pressure and low temperature.
High pressure is maintained because the moles of the product are less than the moles of reactants.
Δn
g
=2−(2+1)=−1
Δn
g
<0
When pressure is increased, the equilibrium will shift to product side (which contains less number of moles of gaseous species). This nullifies the effect of increase in pressure. Hence, more and more product will be formed.
According to Le Chatelier's principle, when a system at equilibrium is disturbed, the position of the equilibrium shifts in a direction so that the effect of the change is nullified.
Low temperature favours exothermic reaction. Heat is evolved during the reaction (positive value of enthalpy change).
Answer:
B. Solid put like for me THANK YOU