If 45.0 ml of ethanol (density = 0.789 g/ml) initially at 8.0 ∘c is mixed with 45.0 ml of water (density = 1.0 g/ml) initially at 28.6 ∘c in an insulated beaker, what is the final temperature of the mixture, assuming that no heat is lost? (cetoh=2.42j/(g⋅∘

Answer : The final temperature of the mixture is,

Explanation :

First we have to calculate the mass of ethanol and water.

and,

Now we have to calculate the final temperature of the mixture.

In this problem we assumed that heat given by the hot body is equal to the heat taken by the cold body.

where,

= specific heat of ethanol =

= specific heat of water =

= mass of ethanol = 35.5 g

= mass of water = 45.0 g

= final temperature of mixture = ?

= initial temperature of ethanol =

= initial temperature of water =

Now put all the given values in the above formula, we get:

Therefore, the final temperature of the mixture is,

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation:

answer:

technetium is the most reactive. this is followed by silver. the least reactive out of these three elements is strontium.