Consider the reaction 2CO(g) + 2NO(g)2CO2(g) + N2(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 2.00 moles of CO(g) react at standard conditions. S°surroundings = J/K Are You Sure? Please check your answer for mistakes. Submit Answer

The value of for the surrounding when given amount of CO gas is reacted is 197.77 J/K

Explanation:

Entropy change is defined as the difference in entropy of all the product and the reactants each multiplied with their respective number of moles.

The equation used to calculate entropy change is of a reaction is:

For the given chemical reaction:

The equation for the entropy change of the above reaction is:

We are given:

Putting values in above equation, we get:

Entropy change of the surrounding = - (Entropy change of the system) = -(-197.77) J/K = 197.77 J/K

We are given:

Moles of CO gas reacted = 2.00 moles

By Stoichiometry of the reaction:

When 2 mole of CO gas is reacted, the entropy change of the surrounding will be 197.77 J/K

So, when 2.00 moles of CO gas is reacted, the entropy change of the surrounding will be =

Hence, the value of for the surrounding when given amount of CO gas is reacted is 197.77 J/K

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.