A25.5 −g aluminum block is warmed to 65.9 ∘c and plunged into an insulated beaker containing 55.2 g water initially at 22.1 ∘c. the aluminum and the water are allowed to come to thermal equilibrium.

Hi, this question is incomplete. The complete question is "A 25.5-g aluminum block is warmed to and plunged into an insulated beaker containing 55.2 g water initially at 22.1^{0}\textrm{C}. The aluminum and the water are allowed to come to thermal equilibrium. Assuming that no heat is lost, what is the final temperature of the water and aluminum?"

Final temperature is 26.1^{0}\textrm{C}

Explanation:

Let's assume final temperature is T where

As no heat is lost therefore in equilibrium-

amount of heat released by Al block = amount of heat consumed by water

or,

Here m represents mass, C represents specific heat and represents change in temperature

So,

or,

So, the final temperature is

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.

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.