What is the value for δsºreaction for the following reaction, given the standard entropy values?
al2o3(s) + 3h2(g) → 2al(s) + 3h2o(g)

substance sº(j/mol*k)
al2o3(s) 51
h2(g) 131
al(s) 28
h2o(g) 189

The of the reaction is

Explanation:

Entropy change of the reaction is defined as the difference between the total entropy change of the products and the total entropy change of the reactants.

Mathematically,

For the given chemical equation:

We are given:

Putting values in above equation, we get:

Hence, the of the reaction is

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.