Question

Two chemical reactions are given.
i. Sulphur dioxide combines with oxygen to form sulphur trioxide.
ii. Sodium reacts with water.
a) Write the balanced chemical equation for any one of the above reactions.
b) Which of the above reactions is a reversible reaction?
c) What is the effect of pressure and temperature on this reversible reaction? Give reason.

Answer 1

Hint:We know that at the point when particles pick up or lose electrons to yield particles, or join with different atoms, their symbols are changed to produce substances that are properly formed to these species. Stretching out this symbol to represent and the overall amounts of substances going through a synthetic (or physical) change includes balancing chemical equations.

Complete answer:
(a)We have to remember that the sulphur dioxide that reacts with oxygen gives sulphur trioxide. We can write the chemical equation for this reaction as,
\[2S{O_2} + {O_2} \rightleftharpoons 2S{O_3}\]
We have to know when the sodium reacts with water to form sodium hydroxide. We can write the chemical equation for this reaction as,
 \[2Na + 2{H_2}O \to 2NaOH + {H_2}\]
(b) The formation of sulphur trioxide by the reaction of sulphur dioxide and oxygen is a reversible reaction.
\[2S{O_2} + {O_2} \rightleftharpoons 2S{O_3}\]
(c) There are three molecules on the reactant side and two molecules on the product side. So, the increase in the pressure of the system will help the forward reaction. That means more products will be produced. As heat is freed during the reaction among oxygen and sulphur dioxide, further increase in temperature will help backward reaction. That means the product will decompose to reactants.

Note: We have to know that the essential parts for balancing chemical equation:
The substances going through response are called reactants, and their recipes are set on the left half of the condition.
The substances created by the response are called items, and their recipes are set on the correct sight of the condition.
Besides signs \[\left( + \right)\] separate individual reactant and item recipes, and a bolt \[\left( \to \right)\] isolates the reactant and item (left and right) sides of the condition.
The general quantities of reactant and item species are called to by coefficients. The numbers put promptly to one side of every chemical formula is called coefficient. A coefficient of 1 is normally discarded.