Acalorimeter contains 22.0 ml of water at 14.0 ∘c . when 2.50 g of x (a substance with a molar mass of 82.0 g/mol ) is added, it dissolves via the reaction x(s)+h2o(l)→x(aq) and the temperature of the solution increases to 28.0 ∘c . calculate the enthalpy change, δh, for this reaction per mole of x. assume that the specific heat of the resulting solution is equal to that of water [4.18 j/(g⋅∘c)], that density of water is 1.00 g/ml, and that no heat is lost to the calorimeter itself, nor to the surroundings.

The enthalpy change in the the reaction is -47.014 kJ/mol.

Explanation:

Volume of water in calorimeter = 22.0 mL

Density of water = 1.00 g/mL

Mass of the water in calorimeter = m

Mass of substance X = 2.50 g

Mass of the solution = M = 2.50 g + 22 g = 24.50 g

Heat released during the reaction be Q

Change in temperature =ΔT = 28.0°C - 14.0°C = 14.0°C

Specific heat of the solution is equal to that of water :

c = 4.18J/(g°C)

Heat released during the reaction is equal to the heat absorbed by the water or solution.

Heat released during the reaction =-1.433 kJ

Moles of substance X=

The enthalpy change, ΔH, for this reaction per mole of X:

if the temperature drops and becomes cool

then the atmosphere can be freezing as the water vapor in the air is at maximum (100%) and can be severely cold

also can be snowing lightly as the moisture in the air will start to solidify

and btw this is not chemistry but