An intermediate step in the process that ultimately produces sulfuric acid, is t

Question

An intermediate step in the process that ultimately produces sulfuric acid, is the catalytic oxidation of SO2 to SO3. Vanadium(V) oxide is the catalyst. The three chemical species in the reaction are in equilibrium as follows:

2SO2(g)+O2(g)2SO3(g)

Which of the following are true statements about this reaction?

1.When SO2 is mixed with O2 in a container, the initial rate of the forward reaction (production of SO3) is faster than the initial rate of the reverse reaction (production of SO2).

2.As SO2 is used up and SO3 accumulates, the rate of the forward reaction increases and the rate of the reverse reaction decreases.

3.At equilibrium the rate of production of SO3 reaches zero.

4.At equilibrium the concentration of SO2 will no longer be changing.

Explanation / Answer

Answer – We are given the reaction

2SO2(g) + O2 <----> 2SO3(g)

We know initial when SO2 reacts with O2 there is initial rate of the forward reaction (production of SO3) is faster than the initial rate of the reverse reaction, because reverse reaction is start when equilibrium occurred. The first statement is correct.

So as the reaction SO2 gets all sued there is reversed reaction rate increase than forward reaction, so second statement is incorrect.

We know at the equilibrium both rate of forward and backwards are same, so at equilibrium the rate of production of SO3 reaches zero and at equilibrium the concentration of SO2 will no longer be changing. So third and fourth one also correct

So statement number 1, 3 and 4 are true.

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.