contestada

Step 1:H2(g)+ICl(g)→HI(g)+HCl(g)(slow)Step 2:HI(g)+ICl(g)→HCl(g)+I2(g)(fast)The reaction is carried out at constant temperature inside a rigid container. Based on this mechanism, which of the following is the most likely reason for the different rates of step 1 and step 2 ?

Respuesta :

H2(g)+2ICl(g) → 2HCl(g)+I2(g)H2(g)+2ICl(g)→2HCl(g)+I2(g)

rate=k[HI][ICl]

What is Rate of Reaction?

The pace at which the products are created from the reactants in a chemical reaction is referred to as the rate of reaction. It provides some understanding of how quickly a response might occur. For instance, the combustion of cellulose in fire has a very rapid response rate and is finished in a fraction of a second.

The pace at which reactants change into products is known as the rate of reaction or reaction rate. It goes without saying that the pace at which chemical reactions take place varies greatly. While certain chemical reactions occur almost instantly, others often take time to achieve their ultimate equilibrium.

Rate of reaction=Amount of reactant used/Time taken for the                           consumption of the reactant

Learn more about Rate of Reaction from given link

https://brainly.com/question/12904152

#SPJ4

Otras preguntas