Identify the oxidizing agent in the reaction: sn(s) + 2h+(aq) → sn2+(aq) + h2(g) sn2+ h2 h+ sn

H⁺(aq)

Explanation:

Let's consider the following redox reaction.

Sn(s) + 2 H⁺(aq) → Sn²⁺(aq) + H₂(g)

We can identify both half-reactions.

Oxidation: Sn(s) → Sn²⁺(aq) + 2 e⁻

Reduction: 2 H⁺(aq) + 2 e⁻ → H₂(g)

Sn(s) undergoes oxidation so it is the reducing agent, while H⁺(aq) undergoes reduction so it is the oxidizing agent.

here we have to get the change of moles on decrease the volume of the reaction in gas phase.

the   per the given options it will decrease by (d) 11-50%

we know, on decreasing the volume of the gas phase reaction the reaction moves to the product side.

the reaction:                     so₂cl₂ (g) = so₂ (g) + cl₂ (g)         total

the moles at equilibrium:   1 - α                 α               α           = 1+α

concentrations:                   1 - α               α               α           = 1 + α

(concentration = moles/volume, as volume is 1 l)

(where α is the degree of dissociation)

now the dissociation constant in terms of concentration is :

=  

or,

or,   = (at v = 1l)

the reaction:                     so₂cl₂ (g) = so₂ (g) + cl₂ (g)         total

the moles at equilibrium:   1 - α                 α               α           = 1+α

concentrations:               (1 - α)/0.5           α/0.5         α/0.5       = (1 + α)/0.5

thus, the dissociation constant in terms of concentration is :

or,  

=  

so, the change of 1 : 1/0.5

or, 1: 2

thus it will decrease by 50%.

or, as per the given options it will decrease by 11-50%

h let me think